METHOD AND APPARATUS FOR CHARACTERIZING HIGH-ENERGY ELECTROCHEMICAL CELLS USING POWER FUNCTIONS OBTAINED FROM CALORIMETRY

Abstract: Characterizing electrochemical cell components and a response of an electrochemical cell to a specified operating condition involves preparing a sample of an electrode material in contact with an electrolyte. Self-heating, power-temperature or power-time data is obtained for the sample using a calorimetry technique, such as by use of an accelerating rate calorimetry technique or a differential scanning calorimetry technique. A power function is developed for the sample using the self-heating, power-temperature or power-time data. The power function is representative of thermal power per unit mass of the sample as a function of temperature and amount of reactant remaining from a reaction of the sample electrode material and electrolyte. A first power function is developed that characterizes a reaction between the cathode material and the electrolyte in terms of thermal power per unit mass of a cathode sample material, and a second power function is developed that characterizes a reaction between the anode material and the electrolyte in terms of thermal power per unit mass of the anode sample material. An electrode material sample from which a power function is developed is prepared using less than about 100 grams of the electrode material, such as between about 1 and 10 grams, but may be as little as between about 1 milligram and 1 gram. A computer system and computer-readable medium are provided to electronically design and test cells of arbitrary size and shape using power functions developed for individual electrode/electrolyte combinations.

Description: METHOD AND APPARATUS FOR CHARACTERIZING HIGH-ENERGY ELECTROCHEMICAL CELLS USING POWER FUNCTIONS OBTAINED FROM CALORIMETRY Field of the Invention The present invention relates generally to high-energy electrochemical cells, such as lithium-based cells, other secondary cells, and batteries constructed therefrom. More particularly, the present invention relates to systems and methods for characterizing electrochemical cells and for predicting the response of such cells to thermal, mechanical or electrical abuse based on power functions obtained from calorimetry. Background of the Invention Rechargeable electrochemical cells are currently used to power a wide variety of portable electronic devices, including laptop computers, cell phones, cameras, and personal organizers, for example. The increased use of such mobile devices has placed a greater demand on the battery manufacturing industry to provide high powered cells that may be used safely in a wide spectrum of consumer and industrial applications. In order to minimize size and weight, battery technologies with high-energy density are normally used. Larger versions of such technologies may, for example, be used in hybrid or all-electric vehicles. High-energy density cells store large amounts of energy in relatively small volumes. If this energy is released quickly and in an uncontrolled manner, however, thermal runaway is possible, leading to safety concerns. Lithium-ion and lithium-ion polymer cells (collectively referred to as lithium-ion cells in the following discussion), for example, exhibit the largest energy density of all ambient-temperature rechargeable cell technologies. Lithium-ion cells are carefully engineered to meet a variety of safety test standards, including, for example, UL-1642 (Underwriters Laboratories) and IEC-61960 (International Electrotechnical Commission) standards. The tests defined by these standards include oven exposure, short-circuit, forced overcharge, forced discharge, shoc and vibration. Other proposed tests include nail penetration tests. It is desirable that cells and batteries constructed from such cells do not emit smoke or flame when subjected to thermal, electrical, and mechanical stress associated with the above-identified tests. In addition to the electrical energy which lithium-ion cells can deliver during discharge, these and other high-energy cells can also evolve a considerable amount of heat due to the reaction ofthe electrode materials with the electrolyte. During short-circuiting of a cell, for example, both the electrical energy ofthe cell and the chemical heat resulting from the electrode/electrolyte reactions are dissipated as heat within the cell. Thermal runaway can occur if the sum of these thermal powers is greater than the power that can be transported from the cell to the environment. The UL and IEC oven exposure tests probe the severity of electrode/electrolyte reactions. These reactions are most severe when the cell is fiilly charged. In accordance with these oven exposure tests, a fiilly charged cell is placed into an oven and exposed to a temperature of 150°C (UL) or 130°C (IEC) for a predetermined duration of time. Short-circuiting ofthe cell under test normally does not occur and the cell temperature rises above the oven temperature to the point where the power generated by electrode/electrolyte reactions is equal to the power that can be transferred to the environment. However, if the former is always larger than the latter, thermal runaway occurs. It is noted that, although cells in consumer use are typically not placed in ovens at high temperature, they may be exposed to 85°C environments in battery cases that inadvertently are thermally well-insulated. If electrode/electrolyte reactions proceed significantly at such temperatures, insulated batteries could exhibit thermal runaway. The total power generated by the electrode/electrolyte reactions (under a specific set of circumstances) is proportional to the total volume ofthe cell. That is, if two cells have the same chemistry, the same construction details and the same charging history, but one has twice the volume ofthe other, then the larger cell will evolve twice the power due to electrolyte/electrode reactions at elevated temperature than the smaller one. The power that can be transferred to the environment, however, is proportional to the cell surface area. Therefore, it is expected that the cell surface area to volume ratio should be maximized to optimize cell safety. This is not always possible due to cell manufacturing constraints or physical size limitations of a device within which the cell will be housed. Given the issues discussed above, it can be appreciated that cell designers are faced with a complex task. The cell designer is often asked to maximize cell performance, cell energy density, and cell safety. Design changes that maximize energy density may, however, adversely compromise safety. Design changes to cell shape and cell size also affect safety. Selection ofthe electrode materials and electrolyte affect performance and safety. Typically, designers are able to make simple cell performance and energy density estimates based on projections from data collected in lab cells. However, it has heretofore not been possible to reliably predict safety test results of practical cells (e.g., full-scale consumer batteries) based on test results at the lab scale. In order to conduct reliable safety studies, prototyping of a potential product in actual cell hardware, followed by extensive testing, is presently necessary. Moreover, large quantities of electrode materials must be produced in order to properly construct prototype cells for safety testing and evaluation. Conventional cell attery design and development techniques typically require the production and availability of 10 kilograms or more of sample electrode material. Those skilled in the art readily appreciate that designing, developing, and testing electrochemical cells and batteries, particularly those having a custom, non- industry standard configuration, using conventional approaches is extremely time consuming and costly. There is a need in the battery manufacturing industry for systems and methods that assist in the design of electrochemical cells and batteries of varying technologies, and which require the production of small quantities of sample electrode materials. There exists a further need for such systems and methods that eliminate the present need to construct full-scale cell/battery prototypes in order to fiilly evaluate the safety aspects of a given cell/battery design. The present invention fulfills these and other needs. Summary of the Invention The present invention is directed to methods and apparatuses for characterizing electrochemical cell components and for characterizing a response of an electrochemical cell to a specified operating condition. According to one embodiment ofthe present invention, characterizing electrochemical cell components involves preparing a sample of an electrode material in contact with an electrolyte. Self-heating, power-temperature or power-time data is obtained for the sample using a calorimetry technique, such as by use of an accelerating rate calorimetry technique or a differential scanning calorimetry technique, for example. Obtaining self-heating data, for example, may involve obtaining temperature versus time data ofthe sample during substantially adiabatic reaction. A power function is developed for the sample using the self-heating, power-temperature or power-time data. The power function is representative of thermal power per unit mass ofthe sample as a function of temperature and amount of reactant remaining from a reaction ofthe sample electrode material and electrolyte. In general, preparing the electrode material sample involves preparing the sample using less than about 100 grams ofthe electrode material. According to one embodiment, preparing the electrode material sample involves preparing the sample using between about 1 gram and about 10 grams ofthe electrode material. In another embodiment, preparing the electrode material sample involves preparing the sample using between about 1 milligram and about 1 gram ofthe electrode material. Improvements in calorimetry techniques may provide for the development of power functions for electrode material samples using nanograms ofthe electrode material samples. The electrode material may be a cathode material or an anode material. The electrode material may, for example, include lithium. In accordance with another embodiment, characterizing electrochemical cell components involves preparing a first sample of a cathode material in contact with an electrolyte and preparing a second sample of an anode material in contact with the electrolyte. First and second self-heating, power-temperature or power- time data are obtained for the first and second samples, respectively, using a calorimetry technique. A first power function for the first sample and a second power function for the second sample are developed using the first and second self- heating, power-temperature or power-time data, respectively. The first power function characterizes a reaction between the cathode material and the electrolyte in terms of thermal power per unit mass ofthe cathode sample material, and the second power function characterizes a reaction between the anode material and the electrolyte in terms of thermal power per unit mass ofthe anode sample material. Preparing the first sample typically involves preparing the first sample using less than about 100 grams ofthe cathode material, and preparing the second sample typically involves preparing the second sample using less than about 100 grams ofthe anode material. According to one embodiment, preparing the first sample involves preparing the first sample using between about 1 and 10 grams of the cathode material, and preparing the second sample involves preparing the second sample using between about 1 and 10 grams ofthe anode material. In another embodiment, preparing the first sample involves preparing the first sample using between about 1 milligram and about 1 gram ofthe cathode material, and preparing the second sample involves preparing the second sample using between about 1 milligram and about 1 gram ofthe anode material. The cathode and anode material may each include lithium. The calorimetry technique employed may be an accelerating rate calorimetry technique or a differential scanning calorimetry technique. According to another embodiment ofthe present invention, characterizing an electrochemical cell involves defining one or more physical parameters ofthe electrochemical cell. A first power function characterizing a reaction between a cathode and an electrolyte in terms of thermal power per unit mass of cathode material is provided. Also provided is a second power function characterizing a reaction between an anode and the electrolyte in terms of thermal power per unit mass of anode material. A response ofthe cell to a specified operating condition is predicted using the first and second power functions and the physical parameters of the electrochemical cell. In one embodiment, characterizing the electrochemical cell in this manner is implemented using a computer and user-interface coupled to the computer. Defining one or more physical parameters ofthe cell may further involve adjusting the physical parameters ofthe cell. Predicting the response ofthe cell, in this case, involves predicting the response ofthe cell using the first and second power functions and the adjusted physical parameters ofthe cell. Defining one or more physical parameters ofthe cell may also involve receiving user input data representative of physical parameters ofthe cell. Receiving user input data may further involve presenting to a user an input field corresponding to each physical parameter ofthe cell and receiving input data from the user in each ofthe input fields. Defining one or more physical parameters of the cell may also involve receiving physical parameters ofthe cell electronically, such as from an external local or remote host processor. Defining one or more physical parameters ofthe cell may further involve defining one or more physical parameters for each of an anode and a cathode ofthe cell. Defining physical parameters for each ofthe anode and cathode ofthe cell may further involve adjusting the physical parameters of one or both ofthe anode and cathode. Predicting the response ofthe cell in this case further involves predicting the response ofthe cell using the first and second power functions and the adjusted physical parameters of one or both ofthe anode and cathode. The specified operating condition may, for example, include a condition of constant or varying ambient temperature, a condition of a constant or varying current applied to the cell, a condition of an external short-circuit connected to the cell or a condition of a short-circuit internal to the cell. A system for characterizing an electrochemical cell, in accordance with yet another embodiment ofthe present invention, includes a processor and a user- interface coupled to the processor. The user-interface includes an input device operable by a user for entering one or more physical parameters ofthe electrochemical cell. The system further includes memory coupled to the processor. The memory stores a cathode power function characterizing a reaction between a cathode and an electrolyte in terms of thermal power per unit mass of cathode material, and further stores an anode power function characterizing a reaction between an anode and the electrolyte in terms of thermal power per unit mass of anode material. The processor computes a response of an electrochemical cell to a specified operating condition using the cathode and anode power functions and the physical parameters ofthe electrochemical cell. The input device is further operable by the user to enter physical parameters of an anode and a cathode ofthe cell. The processor, according to this embodiment, computes the response ofthe electrochemical cell to a specified operating condition using the cathode and anode power functions and the user- entered physical parameters ofthe anode and cathode ofthe electrochemical cell. The input device is also operable by the user to adjust physical parameters ofthe cell, and the processor further computes the response ofthe electrochemical cell to a specified operating condition using the cathode and anode power functions and the adjusted physical parameters ofthe electrochemical cell. A user may also use the input device to adjust physical parameters of an anode and a cathode ofthe cell, and the processor computes the response ofthe electrochemical cell to the specified operating condition using the cathode and anode power functions and the adjusted physical parameters ofthe anode and cathode ofthe electrochemical cell. The system may further include a display. The input device is operable by the user for entering physical parameters ofthe electrochemical cell into input fields presented on the display. Physical parameters of an anode and a cathode of the electrochemical cell may also be entered using the input device into input fields presented on the display. The system may further include a calorimeter system coupled to the processor. The calorimeter system may include an accelerating rate calorimeter or a differential scanning calorimeter. The memory ofthe system may be situated proximate the processor, situated remotely from the processor or distributed at locations local to and/or remote from the processor. The memory that stores the anode and cathode power functions, for example, may be partially or completely situated remotely from the processor. Power functions developed for a number of electrode/electrolyte combinations may be stored in a database or in libraries. Power functions and libraries of power functions may be accessed via a network connection. Characterizing electrochemical cell components in accordance with another embodiment ofthe present invention involves defining one or more physical parameters of an electrochemical cell, and characterizing a reaction between a cathode and an electrolyte in terms of thermal power per unit mass of cathode material by defining a first power function. A reaction between an anode and the electrolyte in terms of thermal power per unit mass of anode material is also characterized by defining a second power function. The response ofthe cell to a specified operating condition is estimated using the first and second power functions and the physical parameters ofthe electrochemical cell. Characterizing the respective cathode/electrolyte and anode/electrolyte reactions according to this embodiment involves modeling the respective reactions assuming an autocatalytic reaction mechanism. The first power function, P c , associated with the cathode/electrolyte reaction may be characterized by the following equations: ^- = k(l -u)(/? + U ° 5 ) dT άu dt C\ dt P c = H dw/dt where, u represents a dimensionless fractional degree of conversion, k represents a reaction rate constant defined by k = γ exp(-E a /kbT), γ represents a frequency factor expressed in terms of minutes "1 , E a represents activation energy, IQ, represents Boltzmann's constant, T represents a temperature ofthe cell, β represents a dimensionless parameter of autocatalysis, h represents total heat which can be evolved by a sample of cathode material during reaction expressed in terms of Joules, C' tot represents a total heat capacity ofthe reactant and a sample calorimeter bomb expressed in terms of J/K, and H represents total heat generated by the cathode/electrolyte reaction per gram of cathode material. The second power function, P a , associated with a lithium intercalated carbon anode/electrolyte reaction, may be characterized by: P =H 2 \ ^-\ +H. \ ^- [13] 2 1 dt λ dt where, ^ -^ exp^ */ 5 [14], and dx. dx x dx [16] dt dt dt dt and where, xi represents an amount of type 1 lithium measured as x in Li x C6, x 2 is an amount of type 2 lithium, measured per six carbons, and x 3 is an amount of type 3 lithium, measured per six carbons, xι 0 , x 2 o, and x 3o are initial amounts of lithium after electrochemical discharge and before heating, Et and E 2 are activation energies, and γi and γ 2 are frequency factors, f is a constant of proportionality that governs how fast the layer of reaction products on the surface ofthe carbon grows as type 1 lithium is converted to type 3 lithium, and Hi and H 2 are the heat per gram of carbon due to the changes Δxi = -1 and Δx 2 =-1, respectively. Characterizing the cathode/electrolyte reaction may involve characterizing the cathode/electrolyte reaction using less than about 100 grams of cathode material, and characterizing the anode/electrolyte reaction may involve characterizing the anode/electrolyte reaction using less than about 100 grams of anode material. According to one embodiment, characterizing the cathode/electrolyte reaction involves characterizing the cathode/electrolyte reaction using between about 1 and 10 grams of cathode material, and characterizing the anode/electrolyte reaction involves characterizing the anode/electrolyte reaction using between about 1 and 10 grams of anode material. In another embodiment, characterizing the cathode/electrolyte reaction involves characterizing the cathode/electrolyte reaction using between about 1 milligram and about 1 gram of cathode material, and characterizing the anode/electrolyte reaction involves characterizing the anode/electrolyte reaction using between about 1 milligram and about 1 gram of anode material. The cathode and anode material may each include lithium. Characterizing the first and second power functions may involve obtaining temperature versus time data, power versus temperature data or power versus time data for each ofthe cathode/electrolyte and anode/electrolyte reactions. The first and second power functions are preferably characterized using a calorimetry technique, such as an accelerating rate calorimetry technique or a differential scanmng calorimetry technique. The specified operating condition may involve a condition of constant or varying ambient temperature, a condition of a constant or varying current applied to the cell, a condition of an external short-circuit connected to the cell or a condition of a short-circuit internal to the cell. In accordance with yet another embodiment, a computer readable medium embodying program instructions for characterizing electrochemical cell components is provided. The computer medium embodies program instructions executable by a processor that characterize a reaction between a cathode and an electrolyte in terms of thermal power per unit mass of cathode material by defining a first power function, and further characterize a reaction between an anode and the electrolyte in terms of thermal power per unit mass of anode material by defining a second power function. The program instructions executable by the processor further provide for defining one or more physical parameters ofthe electrochemical cell, and predicting a response ofthe cell to a specified operating condition using the first and second power functions and the physical parameters ofthe electrochemical cell. According to this embodiment, characterizing the respective cathode/electrolyte and anode/electrolyte reactions involves modeling the respective reactions assuming an autocatalytic reaction mechanism. The first power function, P c , associated with the cathode/electrolyte reaction, and the second power function, P a , associated with the anode/electrolyte reaction, may be respectively computed using the equations provided hereinabove. Defining one or more physical parameters ofthe cell may further involve adjusting the physical parameters ofthe cell, and predicting the response ofthe cell further involves predicting the response ofthe cell using the first and second power functions and the adjusted physical parameters ofthe cell. Defining one or more physical parameters ofthe cell may also involve receiving user input data representative of physical parameters ofthe cell. Receiving user input data further may involve presenting to a user an input field corresponding to each physical parameter ofthe cell, and receiving input data from the user in each ofthe input fields. Defining one or more physical parameters ofthe cell may further involve receiving physical parameters ofthe cell electronically. One or more physical parameters ofthe cell may be defined for each of an anode and a cathode ofthe cell. Defining physical parameters for each ofthe anode and cathode ofthe cell may involve adjusting the physical parameters of one or both ofthe anode and cathode, and predicting the response ofthe cell involves predicting the response ofthe cell using the first and second power functions and the adjusted physical parameters of one or both ofthe anode and cathode. The specified operating condition may involve a condition of constant or varying ambient temperature, a condition of a constant or varying current applied to the cell, a condition of an external short-circuit connected to the cell or a condition of a short-circuit internal to the cell. The above summary ofthe present invention is not intended to describe each embodiment or every implementation ofthe present invention. Advantages and attainments, together with a more complete understanding ofthe invention, will become apparent and appreciated by referring to the following detailed description and claims taken in conjunction with the accompanying drawings. Brief Description of the Drawings Fig. 1 is a detailed diagram of an accelerating-rate calorimeter which may be used to determine self-heating profiles of electrochemical cell material from which power functions may be derived in accordance with the principles ofthe present invention; Fig. 2 is a schematic of a coin cell used to prepare carbon electrodes for accelerating rate calorimeter experiments according to an embodiment ofthe present invention; Fig. 3 is a schematic of a lithium-ion coin cell used to prepare Li x CoO 2 for accelerating rate calorimeter samples in accordance with an embodiment ofthe present invention; Fig. 4 is a graph of temperature vs. time data for an accelerating rate calorimeter experiment on a Li x CoO ∑ /electrolyte sample according to an embodiment ofthe present invention; Fig. 5 is a plot ofthe natural logarithm ofthe self-heating rate vs. temperature for accelerating rate calorimeter experiments on Li x CoO 2 (4.2 V) in electrolyte heated to various initial starting temperatures in accordance with an embodiment ofthe present invention; Figs. 6A-6E are plots ofthe natural logarithm ofthe self-heating rate vs. temperature for accelerating rate calorimeter experiments on a Li x CoO 2 sample initially heated to (A) 150°C, (B) 160 °C, (C) 170 °C, (D) 175 °C, and (E) 180 °C, respectively, according to an embodiment ofthe present invention; Figs. 7A-7B show data for lithiated mesocarbon microbeads (MCMB) in electrolyte at two different starting temperatures compared to the calculated profile with particular power function parameters in accordance with an embodiment of the present invention; Fig. 8 is a diagram of a cross-section of a cylindrical cell in accordance with an embodiment ofthe present invention; Fig. 9 is a cross-section of a prismatic cell used for thermal modeling in accordance with an embodiment ofthe present invention; Figs. 10A-10B are temperature vs. time graphs illustrating a comparison of the calculated and measured oven-exposure profiles for cells from a first manufacturer (Manufacturer A) according to an embodiment ofthe present invention; Figs. 11 A-l IB are temperature vs. time graphs illustrating a comparison of the calculated and measured oven-exposure profiles for cells from a second manufacturer (Manufacturer B) according to an embodiment ofthe present invention; Fig. 12 is a temperature vs. time graph illustrating calculated oven exposure profiles (150°C) as a function of cell radius for cells using the parameters in Table 2 below; Fig. 13 is a depiction of a user-interface screen presented on a computer system display which provides for user interaction with a cell/battery modeling program in accordance with the principles ofthe present invention; Fig. 14 is a depiction of a user-interface screen presented on a computer system display which provides for user input and adjustment to various cathode parameters in accordance with a cell/battery modeling program embodiment ofthe present invention; Fig. 15 is a depiction of a user-interface screen presented on a computer system display which provides for user input and adjustment to various data concerning accelerating rate calorimetry cathode calculations in accordance with a cell/battery modeling program embodiment ofthe present invention; Fig. 16 is a depiction of a user-interface screen presented on a computer system display which provides for user input and adjustment to various data concerning differential scanning calorimetry cathode calculations in accordance with a cell/battery modeling program embodiment ofthe present invention; Fig. 17 is a depiction of a user-interface screen presented on a computer system display which provides for user input and adjustment to various anode parameters in accordance with a cell/battery modeling program embodiment ofthe present invention; Fig. 18 is a depiction of a user-interface screen presented on a computer system display which provides for user input and adjustment to various battery parameters in accordance with a cell/battery modeling program embodiment ofthe present invention; Fig. 19 is a depiction of a user-interface screen presented on a computer system display which provides for user input and adjustment to various parameters of a battery having a cylindrical configuration in accordance with a cell attery modeling program embodiment ofthe present invention; and Fig. 20 is a depiction of a user-interface screen presented on a computer system display which provides for user input and adjustment to various parameters of a battery having a prismatic configuration in accordance with a cell/battery modeling program embodiment ofthe present invention. While the invention is amenable to various modifications and alternative forms, specifics thereof have been shown by way of example in the drawings and will be described in detail hereinbelow. It is to be understood, however, that the intention is not to limit the invention to the particular embodiments described. On the contrary, the invention is intended to cover all modifications, equivalents, and alternatives falling within the scope ofthe invention as defined by the appended claims. Detailed Description of Various Embodiments In the following description ofthe illustrated embodiments, references are made to the accompanying drawings which form a part hereof, and in which is shown by way of illustration, various embodiments in which the invention may be practiced. It is to be understood that other embodiments may be utilized, and structural and functional changes may be made without departing from the scope ofthe present invention. In accordance with the principles ofthe present invention, the response of high-energy electrochemical cells, such as lithium-based cells, to conditions of thermal, electrical and mechanical abuse may be predicted using experimental data collected from calorimetry studies on electrode materials in electrolyte. Accelerating-rate calorimetry or, alternatively, differential scanning calorimetry experiments on small quantities of electrode materials prepared in lab cells may be used to extract mathematical expressions, referred to herein as "power functions," for the particular electrode/electrolyte pair as a function of temperature and chemical reaction history. A power function developed for a particular electrode material may be characterized as the thermal power per gram of electrode material in electrolyte as a function of temperature and amount of remaining reactant, due to the electrode/electrolyte reaction. The power functions for the positive and negative electrodes of a cell, the thermal conductivity ofthe cell, the heat capacity ofthe cell, the mass of electrodes in the cell, and the cell surface heat conductivity may be used to accurately predict the response of a cell of arbitrary size and shape to various safety and performance tests, such as an oven exposure test. Cell response to an overcharge test requires the above described data inputs, as well as electrical power dissipated in the cell. The effect ofthe R- value of insulation around battery packs may also be readily evaluated. Well-known heat equations and Newton's law of cooling, along with equations and methodologies developed by the inventors as disclosed herein, are used to perform the calculations associated with each of these tests. Methods and apparatuses implemented in accordance with the principles ofthe present invention will be extremely useful to cell designers and to designers of battery packs, particularly those designed to be incorporated into portable electronics, vehicles, and backup power modules. Power functions may be developed for a large variety of electrode/electrolyte combinations. These power functions may be organized to form libraries of power functions, which may be organized in many different ways depending on user requirements. The power functions/libraries of power functions may be stored on a permanent storage medium, such as a magnetic or optical storage disk or in an integrated circuit memory or combinational logic device (e.g., non-volatile memory, such as flash memory, electronically erasable programmable read-only memory (EEPROM), gate arrays, and the like). A battery designer may model the performance and response of cells developed from selected electrode/electrolyte combinations by selecting, directly or indirectly, power functions corresponding to the selected electrode/electrolyte combinations from the power function library. One skilled in the art will readily appreciate the substantial time and cost savings that may be realized when designing a cell/battery using a power function-based modeling approach consistent with the principles ofthe present invention. By way of further example, a computer system operable by a battery designer may access power functions and/or power function libraries from memory or other processing devices located proximate to or remotely from the designer's computer system. A power function library resource or service may be made accessible to battery designers, from which selected power functions or power function libraries are obtained. Such a service may significantly assist the design and development efforts of numerous battery manufactures. A given battery manufacturer, for example, may access and use established power functions for specified electrode material/electrolyte combinations during the design and evaluation of "virtual" cells of arbitrary size and shape, rather than constructing actual full-scale battery prototypes. It is noted that, for purposes of simplicity and clarity, aspects ofthe present invention will be described generally with reference to lithium-ion cells, which is intended to represent any lithium-based cell technology. The methods and apparatuses ofthe present invention also have utility in overcoming problems associated with thermal runaway of cells having a non-lithium chemistry, such as a nickel-metal hydride, nickel-cadmium, lead-acid, or sodium sulfur-based chemistry, for example. It will be understood that the principles ofthe present invention are applicable to a wide variety of cell technologies and are not limited to those (e.g., lithium-ion) specifically described herein. In the development of power functions for a particular cell chemistry, a sample cell is developed using a given electrode material/electrolyte combination. Importantly, this sample cell need only be developed once for a given electrode material/electrolyte combination. From this sample cell, power functions are derived which may be used to characterize various characteristics (e.g., thermal characteristics) of cells of varying shapes and sizes fabricated from the same electrode material/electrolyte combination as that ofthe sample cell. It is significant that only a relatively small quantity ofthe sample cell material need be produced for purposes of developing power functions, which may be used to characterize cell components and their response to specified operating conditions (e.g., hostile temperature conditions, a short-circuit condition, an overcharge condition, a nail penetration condition). As was discussed in the Background, conventional cell/battery design and development techniques typically require the production and availability of 10 kilograms or more of sample electrode material. In stark contrast to such conventional approaches, less than about 100 grams of sample electrode material is required to develop power functions that characterize a given electrode/electrolyte combination in accordance with the present invention. In a preferred embodiment, between about 1 and 10 grams of sample electrode material is required. Preparing sample electrode materials in accordance with the principles ofthe present invention need be performed only once. After a power function has been determined for a given electrode material/electrolyte combination, this power function is stored for future use. Power functions for a wide variety of electrode material/electrolyte combinations may be developed from such small electrode material samples. Referring to the drawings, and more particularly to Fig. 1, there is illustrated an embodiment of an accelerating rate calorimeter (ARC) 100 suitable for measuring the self-heating of electrochemical cell samples from which power functions are developed in accordance with the principles ofthe present invention. The accelerating rate calorimeter 100 shown in Fig. 1 is representative of an apparatus initially developed by the Dow Chemical Company, but later commercialized by Columbia Scientific (model ARC-2000). The accelerating rate calorimeter 100 maintains a sample in adiabatic conditions once an exothermic reaction has been detected and measures sample temperature as a function of time. The accelerating rate calorimeter 100 includes a base canister 102 and an upper canister 103 which is detachable with respect to the base canister 102. The base canister 102 includes a nickel-plated copper jacket 104 within which a sample bomb, shown generically in Fig.l as spherical bomb 114, is situated when the upper portion 103 is mounted to the base canister 102. The jacket 104 is surrounded by insulation 106 and defines three heating zones, namely, a top, side, and base heating zone, which are provided with heaters 116, 108, and 110, respectively. Each ofthe heating zones is individually heated and monitored by Nicrosil/Nisil type N thermocouples 118, 114, and 112, respectively, each of which is referenced with respect to an ice point reference. The canister 102, 103 ofthe accelerating rate calorimeter 100 is placed within a 1" thick steel shell to provide a barrier in case of an explosion during the experiment. The shell also contains four micro-switches (not shown ) that must be depressed before any heat can be provided to the instrument. The sample bomb 114 and bomb thermocouple 120 configuration has been modified from that shown in Fig. 1 due to limitations imposed by the reactive materials ofthe sample cells described in the Examples provided hereinbelow. The modified bomb 114 is mounted directly onto a thermocouple 120 hanging in the middle of the jacket 104, in a fishhook-like manner. The accelerating rate calorimeter 100 measures the self-heating of samples in an adiabatic environment by maintaining the bomb and jacket temperatures exactly equal, thus there is no heat flow to or from the sample. Although these were the ideals set out by the designers, in reality, the calorimeter 100 is at a slightly lower temperature than the sample, so that it does not supply heat to the bomb and an accurate self-heating profile ofthe sample can be obtained. The change in temperature, ΔT (K), ofthe calorimeter 100 during analysis is proportional to the thermal energy released during the exothermic process. The amount of thermal energy, Q (J), released for a particular reaction is proportional to the total specific heat ofthe reactant(s) and bomb, ot (JK ' V 1 ), and the mass of reactant(s) and bomb present, mtot (g). These relationships may be combined to give: Q = C tot m tot ΔT, [1] Equation [1] above governs all reactions taking place in the accelerating rate calorimeter 100. Equation [1] is identical to the total heat capacity, C'^ (JK 1 ), ofthe sample multiplied by the change in temperature. For a multi-component mixture, such as a sample cell according to the present invention, the total heat capacity ofthe mixture is equal to the sum ofthe individual heat capacities, as is given by the following equation: Total Heat Capacity = Σ Individual Heat Capacities [2] C' tot = «! « €„ = ∑m i C i [3] where, mi is the mass of component i and is its specific heat. By rearranging Equation [1] above, and solving for temperature and taking the derivative with respect to time, the following self-heating rate ofthe reaction equation is provided as: dT/dt = dQ/dt [mtot C'tot] '1 [4] The quantity dQ/dt is the power, P, (in watts, W) evolved from the sample. The variation in self-heating rates with respect to electrode materials, temperature, and conditions must be understood to properly extract the power functions for a given sample cell according to the present invention. After proper calibration, the accelerating rate calorimeter 100 is able to determine the self-heating profiles of different samples. The accelerating rate calorimeter 100 is operated in a heat- wait-search (HWS) mode which involves heating to a desired temperature, waiting for thermal equilibrium to be achieved for a set time, then searching for a temperature increase greater than or equal to the set sensitivity (usually 0.02°C/min). If the rate is less than the pre-established sensitivity after the search period, the accelerating rate calorimeter 100 will proceed to the next temperature step and this HWS sequence continues until an exotherm is detected or a stop temperature is reached. If an exotherm is detected, the accelerating rate calorimeter 100 will track it by maintaining adiabatic conditions until the completion ofthe exotherm. The operator has the ability to change the heating rate, and wait and search times during the setup ofthe experimental run. To study the kinetics ofthe reactions occurring in the accelerating rate calorimeter 100, it is often useful to force accelerating rate calorimeter samples to temperatures above that at which the exotherm is known to onset. The initial self heating rates measured as a function of starting temperature may be used to obtain kinetic parameters of importance, which will be discussed in greater detail hereinbelow. The preparation of one particular sample cell will now be described for purposes of illustration. It is understood that the following description of a sample lithium-ion cell is not to be construed as limiting the scope and applicability ofthe principles ofthe present invention as to other electrode/electrolyte combinations. In accordance with the following exemplary embodiment, positive electrode material, Li x CoO 2 , and negative electrode material Li x C6, is prepared, from which a sample coin cell is constructed for each ofthe electrode materials in combination with a selected electrolyte. Each electrode/electrolyte combination (e.g., Li x CoO 2 /electrolyte and Li x Cβ/electrolyte) is then subjected to accelerating rate calorimetry experimentation from which power functions for each electrode/electrolyte combination are derived. Within the context of this exemplary embodiment, as a lithium-ion cell is charged, lithium atoms leave the Li x CoO 2 positive electrode and intercalate within the carbon ofthe negative electrode. Both Li x CoO 2 and Li x Cβ react in electrolyte. In order to examine the thermal power produced by each electrode, it is necessary to build accelerating rate calorimeter samples which have only one electrode and electrolyte in contact. This is conveniently accomplished in laboratory coin-type cells, using pellet-shaped electrodes, as described in the following examples. Example #1 Sample electrodes were prepared by combining the electrode powder with 7%, by mass, each of Super S carbon black (MMM carbon, Belgium) and polyvinylidene difluoride (PVDF) binder (9.5% in n-methyl-pyrrolidinone (NMP), National Research Council of Canada (NRC), Ottawa, Canada). The carbon black ensures electrical contact between all ofthe grains in the electrode, while the binder is used to ensure that the electrode holds together. N-methyl pyrrolidinone is then added in excess to make a slurry. The slurry is poured in a shallow layer and dried at 105°C to remove the NMP. After drying, the powder was lightly ground in a mortar and then passed through a 300 μm sieve. The subsequent procedure differs for carbon and for LiCoO 2 , as will be described with reference to Figs. 2 and 3, respectively. Approximately 300 mg ofthe carbon/binder mixture was then placed in a stainless steel mold to which 2000 psi (13.8 MPa) was applied to produce a 1 mm thick carbon pellet. With reference to Fig. 2, the carbon pellet 134 was then placed in a cell casing bottom 132 and the cell 130 was assembled in a manner depicted generally in Fig. 2 within an argon-filled glovebox. Electrolyte (lMLiPFβ EC:DEC 33:67, vol:vol, Mitsubishi Chemicals) was added to the electrode pellet 134 until it was fully wetted, and then two polypropylene separators 136 (Celgard 2502, Celanese) were placed on top ofthe wet pellet 134. Four pieces of 125 μm thick lithium foil (FMC) 140 were added on top of a stainless steel mesh 138 to ensure full electrical contact with all ofthe lithium. A stainless steel spacer 142 was then added above the lithium foil layers 140 to provide pressure on the contents ofthe cell 130. Finally, the cell top 146, with polypropylene gasket 144, was attached and the cell 130 was crimped shut to seal it from the outside environment. The lithium/carbon electrochemical cells 130 were fully discharged to 0 V, until the cells' relaxation voltage under open circuit was less than 50 mV after 24 hours. The cells 130 were then transferred to an argon-filled glovebox for accelerating rate calorimeter sample preparation, which will be described in greater detail hereinbelow. Example #2 With reference to the cell 160 shown in Fig. 3, 0.75 g of a LiCoθ 2 /binder mixture was placed in a stainless steel mold to which 2000 psi (13.8 MPa) was applied to produce an electrode pellet. Both carbon (made as described above) and lithium cobalt oxide pellets were then transferred to the glovebox, and cells were assembled as depicted generally in Fig. 3. Electrolyte (1ML_PF 6 E DEC 33:67, vol/vol, Mitsubishi Chemicals) was first added to the carbon electrode 164 provided in a casing bottom 162 until fully wetted, and then three polypropylene separators 166 were added on top of it, to which the lithium cobalt oxide pellet 168 was added. A casing top 172 and gasket 170 were added above the lithium cobalt oxide electrode 168, and the can 162, 172 was crimped shut. When the electrochemical cells 130, 160 were removed from the glovebox, stainless steel tabs were spot-welded to the outer casing and the cells 130, 160 were then connected to a charger system. A variety of experiments were performed with the cells 130, 160 on the charger system to simulate a variety of charging characteristics. After the tests were finished, the cells 130, 160 were transferred to an argon-filled glovebox for accelerating rate calorimeter sample preparation. Accelerating rate calorimeter samples were enclosed in welded stainless steel type 304 tubes. The tubes had a 0.006" (0.152 mm) wall, a 0.250" (6.35 mm) diameter and a 1.54" (39.1 mm) length. A stainless steel "pocket" made of 0.001" thick foil was attached to the side ofthe tubes by spot welding. Because ofthe moisture sensitivity ofthe samples, a method was developed to seal the tubes in an inert atmosphere. Tungsten Inert Gas (TIG) welding was used to seal the ends of the stainless steel tubes in the glovebox itself. The electrochemical cells 130, 160 were carefully disassembled in the glovebox and the pellets 134, 164 were recovered. The wet pellets 134, 164 were lightly ground and then each was transferred to the accelerating rate calorimeter sample bomb as described previously with regard to Fig. 1. One end ofthe bomb had been previously welded shut by Tungsten Inert Gas (TIG) welding. Typically, 350 mg (carbon) or 400 g (LiCoO 2 ) ofthe wet electrode was transferred, with an equal amount of excess electrolyte added to the bomb. The bomb was then crimped closed and finally TIG welded shut. The accelerating rate calorimeter sample was mounted in the calorimeter by hooking the pocket ofthe stainless steel tube over the thermocouple in a fishhook-like manner as discussed previously. The calorimeter was then sealed and experiments were performed. Figure 4 shows typical temperature-time data 180 for an accelerating rate calorimeter experiment on a sample of LiCoO 2 charged to 4.2 V versus lithium concentration. At temperatures below 150°C, the accelerating rate calorimeter is in heat- wait-search mode. At 150°C, the self-heating rate is initially above 0.02°C/min, so the accelerating rate calorimeter follows the exotherm under adiabatic conditions. As the sample self-heats, the self-heating rate continually increases as the reaction rate accelerates with increasing temperature. To carefully examine the kinetics ofthe reactions, it is more useful to plot the natural logarithm ofthe self- heating rate, In dT/dt, versus T. Figure 5 shows In dT/dt versus temperature results for Li x CoO 2 in electrolyte initially heated to a number of starting temperatures. Once accelerating rate calorimeter results of this type have been collected, the power functions can then be obtained, as will now be discussed in further detail. In general, power functions are derived for individual electrode/electrolyte material combinations. In particular, power functions are obtained for each ofthe cathode and anode material/electrolyte combinations of a subject cell using accelerating rate calorimetry or differential scanning calorimetry techniques. Once the power functions for particular electrode/electrolyte material combinations are obtained, they are stored for subsequent use. In stark contrast to conventional cell design techniques which require development of full-scale cell/battery prototypes in order to evaluate a given design, power functions obtained from relatively small quantities of sample cell electrode material in accordance with the present invention provide for the characterization and prediction of a cell/battery constructed from like electrode materials having any desired size, shape, weight, form factor, and operating temperature profile. Example #3 In accordance with the following example, power functions for a cathode of a particular chemistry will be described for purposes of illustration. The inventors have performed a careful accelerating rate calorimeter study ofthe reaction between Li x CoO 2 and electrolyte. Two different samples, referred to hereinbelow as Sample #1 and Sample #2, were studied and found to display similar behavior. In both cases, the reaction of Li x CoO 2 in electrolyte was accurately modeled assuming an autocatalytic reaction mechanism. In order to model the reaction ofthe Li x CoO 2 electrode material in electrolyte at 4.2 V, a reaction pathway was hypothesized. The experimental data shown in Fig. 5 suggest a possible autocatalytic mechanism, because the self- heating rate ofthe 150°C start temperature sample at 160°C was larger than an identical sample heated directly to 160°C. Similarly, the self-heating rate ofthe 160°C start temperature sample at 170°C was larger than an identical sample heated directly to 170°C. This behavior is consistent with the acceleration of a reaction by the presence of products as described in the literature (see, e.g., T. Grewer, Thermochimica Acta, 225, 165 (1993)). The differential equation describing the autocatalytic model used in the instant example is given by: where, u is the dimensionless fractional degree of conversion, k a reaction rate constant (k = γ exp(-E a /kbT)), β is the parameter of autocatalysis, and kb represents Boltzmann's constant. The reaction describing this autocatalytic process is given as: B-^→A+P [6] where, the substance B is converted, in the presence of A, to the product P and A. Thus, as the reaction continues, the reaction rate increases due to the presence of more A product and then decreases when the amount of B reactant runs out. If «=0 in Equation [5] above, the autocatalytic reaction has not been initiated, and as u increases, the fractional amount of reactant present decreases. A high degree of autocatalysis implies a small value of β. The temperature influences the kinetics characterized by Equation [2] through the temperature dependence ofk. The power 0.5 in Equation [5] above implies that the catalyst is most effective at the start ofthe reaction. The temperature rise during the autocatalytic reaction is proportional to Equation [5] above and may be characterized by: dT h άu — = * — , [7] dt C' tot dt where, h is the total heat which can be evolved by the sample due to the reaction (Joules) and C'^ is the total heat capacity ofthe reactant and the bomb (JK 1 ). The term h/C'tot was chosen to correspond to the temperature rise from the onset ofthe exotherm to the end ofthe first exothermic behavior (ΔT, 60°C, see, e.g., Fig. 5), because: dT J f— At dt = ΔT , and [8] since for the complete consumption ofthe reactant, thus, ΔT = [10] Figures 6A-6E show that Equations [5] and [7] above may be used to fit the accelerating rate calorimeter results of Fig. 5 closely for a specific choice ofthe parameters E a , γ, β and h/C'tot- Figures 6A-6E are plots ofthe natural logarithm of the self-heating rate versus temperature for accelerating rate calorimeter experiments on the Li x CoO 2 sample of Example #1 above (hereinafter referred to as Sample #1) initially heated to 150 °C (Fig. 6A), 160 °C (Fig. 6B), 170 °C (Fig. 6C), 175 °C (Fig. 6D), and 180 °C (Fig. 6E), respectively. For the fits in Figs. 6A- 6E, the parameters were E a = 1.6 eV, γ = 1.9 x 10 16 min "1 , β = 0.2 and h/C'tot = 60°C. The model fits only the lowest temperature exothermic process. This process is the one that controls thermal runaway in lithium-ion cells, as will be evident from the discussion provided below. The same model may be used to fit the results of accelerating rate calorimeter experiments on Li x CoO 2 at different voltages in electrolyte. Table 1 below shows the parameters that fit accelerating rate calorimeter results for two different Li x CoO 2 samples at a variety of voltages. The data shown in Table 1 are parameters for the power functions which may be characterized using Equation [11] below derived for the Li x CoO 2 samples of Examples #1 and #2 above at selected voltages versus lithium concentration. TABLE 1. In order to calculate the power evolved by the reaction of Li x Coθ2 with electrolyte in a practical cell, the reaction power per gram of sample is calculated. The power per gram of LiCoO 2 is given by: P c = H d«/dr [11] where, H is the total heat generated by the reaction per gram of LiCoO 2 and u and t are as described previously. Using the definition of h in Equation [7] above, H = h/m, where m is the mass of LiCoO 2 in the accelerating rate calorimeter sample. In order to obtain h for Sample #1 of Example #1 above, the value of h/C'tot = 60°C is used, as is the heat capacity of Sample #1. C' to t may be calculated from the specific heats, a, and masses, mi, ofthe materials in Sample #1. The specific heats of EC and DEC ofthe electrolyte and stainless steel were obtained from the literature (Y.S. Touloukian and E H. Buyco, "The Thermophysical Properties of Matter - The TRPC Data Series, Volume 5, Specific Heat - Nonmetallic Solids " Plenum (1970)), and that of LiCoθ2 was estimated from the law of Dulong and Petit (see, e.g., C. Kittel, "Introduction to Solid State Physics " 7 th ed., Wiley and Sons, New York (1996)). For a typical accelerating rate calorimeter specimen of LiCoθ2, the heat capacity is approximated by : where the terms arising from LiCoO 2 , stainless steel, and electrolyte are indicated above and it is assumed that the 0.35 g of wet electrode added is made up of 0.3 g Li x CoO 2 and 0.05 g of electrolyte. Therefore, h = 60°C 1.3 J K = 80 J, and H = h/0.3g = 270 J/g. Similar calculations for accelerating rate calorimeter specimens of Sample #2 of Table 1 above give H = 410 J/g. The power function for Li x CoO 2 in electrolyte is now specified. Equation [5] above is used to calculate duldt and Equation [11] above is used to calculate the evolved power per gram of Li x CoO 2 . The parameters provided in Table 1 above are also used. It will be appreciated by one skilled in the art that the parameters of the power functions for other cathode samples may be determined in a similar way. Given the starting value of u, the starting temperature and the thermal boundary conditions, the temperature-time profiles of Li x CoO∑/electrolyte mixtures may be calculated. Example #4 In accordance with the following example, power functions for an anode of a particular chemistry will be described for purposes of illustration. Lithium intercalated carbon prepared electrochemically has three types of lithium atoms: 1) those intercalated within the structure; 2) those incorporated in metastable products on the surface ofthe carbon due to reactions between lithium atoms and electrolyte; and 3) those in stable reaction products on the surface ofthe carbon. Lithium atoms of types 1 and 2 can react further with electrolyte as the temperature increases, but type 3 cannot. Lithium atoms of type 1 must pass through the film of reaction products (due to type 2 and type 3 lithium) before they can reach the electrolyte and react. Type 2 lithium atoms become type 3 lithium atoms after reaction. Type 1 lithium atoms become type 3 lithium atoms after reaction as well. The initial surface layer on the carbon comprising type 2 and type 3 lithium atoms is referred to as the "solid electrolyte interphase" (see, e.g., M.N. Richard and J.R. Dahn, J. Electrochem. Soc. 146, 2078-2086 (1999)), and this layer protects the intercalated lithium from spontaneous reaction with electrolyte. If the temperature becomes large (i.e., greater than about 80°C), this surface layer begins to decompose (type 2 lithium reacting to become type 3 lithium) and then lithium/electrolyte reactions begin. Both the reaction of type 2 lithium to become type 3 lithium and the reaction of type 1 lithium to type 3 lithium evolve heat. The power function for LiCβ (mesocarbon micro beads from Osaka Gas) in 1M LiPFβ/EC/DEC (33:67 v:v) electrolyte is given by: P =H 2 \^\ +H, \^-\ [13] 1 ώ l l l dt 1 where, dx. dt ^ - r2 exp-^ * 2 05 [14], — = -Y χ exp " * ,/ * tr x x eX « *»+ * »M ' » -* M ' »+*») [15] dt and ^3_ = _ ^_ _ ^2_ r 161 dt dt dt In Equations [13] to [16] above, xi is the amount of type 1 lithium measured as x in Li x Cδ, x 2 is the amount of type 2 lithium, again measured per six carbons, and x 3 is the amount of type 3 lithium, again measured per six carbons in the host. The terms xι 0 , ∑o, and x 3o are the initial amounts of lithium after electrochemical discharge and before heating. For carbons from MCMB discharged to 0.0V versus lithium concentration, xι 0 is about 0.8, 2 0 is about 0.1, and x 3o is about 0.05. The terms Ei and E2 are activation energies, and γi and 72 are frequency factors. For carbons from MCMB discharged to 0.0V versus lithium concentration, Ei and E2 are about 1.4 eV, γi is about 4 x 10 15 min "1 , and γ ∑ is about 7.5 x 10 16 min "1 . The parameter f is a constant of proportionality that governs how fast the layer of reaction products on the surface ofthe carbon grows as type 1 lithium is converted to type 3 lithium. The term f depends on the carbon surface area. For carbons with a surface area near 1 m 2 /g, f is near 2 to 5. The terms Hi and H 2 are the heat per gram of carbon due to the changes Δxi = -1 and Δx 2 = -1, respectively. For carbons from MCMB discharged to 0.0V versus lithium concentration, Hi is about 1700 J/g and H 2 is about 600 J/g. Using Equations [4], [12] and [13] above, it is possible to calculate the response of accelerating rate calorimeter samples. Figures 7A-7B shows data for lithiated MCMB in electrolyte at two starting temperatures, 80°C and 100°C, respectively, compared to the calculated profile with the following power function parameters: xι 0 = 0.75; x 2o = 0.1; x 3o = 0.033; Ei = E 2 = 1.4eV; hi/C = 400; h 2 /C = 150; γi = 4 x 10 15 ; and 72 = 7.5 x 10 16 where, hi is the heat produced by the accelerating rate calorimeter sample due to the complete reaction of type 1 lithium to type 3 lithium, I 2 is the heat produced by the sample due to the complete reaction of type 2 lithium to type 3 lithium, and C is the total heat capacity ofthe sample plus that ofthe tube/bomb (referred to previously hereinabove as C'tot). It can be seen from Figs. 7A-7B that agreement between the experimental and prediction data curves is quite good. As an alternative to using an accelerating rate calorimetry method as described hereinabove, the results of differential scanning calorimetry experiments may be used to extract power functions. According to this approach, a series of differential scanning calorimetry experiments at different scan rates are needed. A differential scanning calorimeter measures the power produced (Watts/g) by a sample as it is heated at a fixed rate. Differential scanning calorimetry experiments typically produce output data in the form of power versus temperature (i.e., power-temperature) data or power versus time (i.e., power-time) data. It has been found, however, that it is difficult to distinguish autocatalytic reactions from simple reactions obeying first order reaction kinetics. Accordingly, the use of an accelerating rate calorimeter approach is preferred, but not required. Once the electrode/electrolyte power functions are known for a particular electrode/electrolyte combination, the response of full-scale cells of any desired form factor to thermal, mechanical or electrical abuse may be calculated. This is accomplished using a numerical method, assuming radial heat flow, that is, no heat flow through the ends ofthe can is assumed. It is understood that models other than a radial heat flow model may be assumed, such as a fiilly-three dimensional heat flow model. Figure 8 shows a cross-section of a cylindrical cell with the inner, r a , and outer, η > , radii of a jelly roll configured cell. The cell can has inner and outer radii, n > and r c , as indicated. The jelly roll is then divided into n annular rings ofthe same thickness. The outer radius ofthe largest annular ring, r„, is equal to π > . The outer radius ofthe i Λ ring is n as shown. For the i ft interior ring, the change of temperature, ΔTi, in a time interval Δt is given by: In Equation [17] above, P«i and Pd are the anode and cathode power functions (per gram of anode material or cathode material, respectively), L is the length ofthe cylinder, and \ and p c are the average densities of active anode or cathode material per unit volume of jelly roll. The term Pei is the electrical power generated per unit volume ofthe cell and πL(ri 2 -ri-ι 2 ) is the volume ofthe i Λ annular ring. The term K is the average thermal conductivity of the jelly roll material, Ti is the temperature ofthe i* annular ring, C is the average jelly roll specific heat capacity, and p is the average jelly roll density. The terms in Equation [17] above may be easily understood by one skilled in the art. The first term is the heat added (in time Δt) to the i Λ ring by the chemical reactions and by the dissipation of electrical energy. The second term is the heat conducted to the i A ring by its outer neighbor and the third term is the heat conducted to the raring by its inner neighbor. For the ring in contact with the can, the change of temperature, ΔTi, in a time interval Δt, is given by: where, KΆ Λ is the thermal conductivity ofthe can and Tea,, is the can surface temperature. For the can surface, the change of temperature, ΔTca„, in a time interval Δt is given by: ΔT |^ B (T - T )2^ nL + (T T )A2 L || At } [19] where, A is the can surface heat conductivity per unit area, 2πrcL is the surface area ofthe cell, and T e is the environmental temperature in which the cell is placed. Ccan and p can are the specific heat capacity and density ofthe material ofthe can, respectively. The first term of Equation [19] above is the heat conducted from the can to the outer ring ofthe jelly roll. The second term is the heat transferred to or from the environment to the cell can. Equations [17-19] are solved iteratively by computer. Each ofthe variables describing the anode (xi, x 2 , and x 3 ) and cathode (u) reaction history are made a function of cell radius, that is xi = xn, etc. The initial boundary conditions ofthe cell are set, that is, T e and each Tj are initialized, and each of xn, x 2 i, x 3 i and Ui are set to their initial values. For purposes of illustration, it is assumed that for a 150°C oven exposure test with a fully charged (4.2 V) cell at room temperature placed instantly into a heated oven, one would set: T e = 150°C, Tc * , = 21°C, Tj = 21°C for all i, ui = 0 for all i, xn = 0.8 for all i, x ∑ i = 0.1 for all i, and x 3 i =0.05 for all i. Small time intervals (e.g., 0.1 second) are taken and Equations [5, 11, 13-19] above are used to calculate the changes in the reaction history parameters and the temperatures ofthe annuli in the small time intervals. These changes are added to the initial values and the calculation is repeated numerous times, until the reactions cease due to the depletion of reactants (i.e., both u = 1 and xi = 0 for all rings) or until one is satisfied that no runaway reaction will occur. A computer program implementing this model has been reduced to practice using both a Fortran program and a Visual C++ program. Equations [17-19] are easily modified for planar geometry, assuming that heat flows only perpendicular to the plane ofthe cell. This assumption is valid in cases commonly found in prismatic lithium-ion and lithium-ion polymer cells, where the cell thickness is normally less than one tenth the cell length or width. Figure 9 shows a cross-section of a prismatic cell. The cell has a length, L, a width, W, and a thickness, 2r c . The cell stack has a total thickness of 2r„. The cell stack is divided into 2n slabs as indicated in the drawing. In cases where there is symmetric heating or cooling at the cell surface, there will be no flow of heat across the center ofthe cell, which is denoted by the heavy line. For the 1 th interior slab, the change in temperature, ΔTi, which occurs in time Δt, is (by analogy to the cylindrical cell) given by: If, i = 1, then the third term on the right-hand side of Equation [20] is omitted to account for the lack of heat flow to the center ofthe cell. For the n Λ interior slab the change in temperature, ΔT n , which occurs in time Δt, is (by analogy to the cylindrical cell) given by: For the can surface, the change of temperature, ΔTcan, in a time interval Δt is given by: Equations [20-22] above are solved iteratively by computer. Each ofthe variables describing the anode (xi, X2, and x 3 ) and cathode (u) reaction history are made a function of cell thickness, that is, xi = xn, etc. The initial boundary conditions ofthe cell are set, that is, T e and each Ti are initialized, and each xn, X2i, x 3 i and Ui are set to their initial values. As an example, for a 150°C oven exposure test, with a fully charged (4.2 V) cell at room temperature placed instantly into a heated oven, one would set: T e = 150°C, T^ = 21°C, Tj = 21°C for all i, u ; = 0 for all i, xn = 0.8 for all i, x ∑ i = 0.1 for all i and x 3 i =0.05 for all i. Small time intervals (e.g., 0.1 second) are taken and the Equations [5, 11, 13-16, 20-22] above are used to calculate the changes in the reaction history parameters and the temperatures of the slabs in the small time intervals. These changes are added to the initial values and the calculation is repeated many times, until the reactions cease due to the depletion of reactants (i.e., both u = 1 and xi = 0 for all rings) or until one is satisfied that no runaway reaction will occur. In order to confirm the predictive power ofthe method described above, accurate temperature-time data for cylindrical lithium-ion cells placed into a heated oven must be obtained. According to one approach, a VWR Scientific 1330 GM gravity convection oven is used. The oven has a 3" diameter hole centered in its top, through which cells may be lowered via an attached thermocouple. A second thermocouple is placed in a small brass block on the oven shelf to monitor the oven temperature. The oven is allowed to equilibrate at the test temperature for at least 4 hours, and the oven temperature stabilizes to within ± 0.2°C ofthe set temperature. The cell thermocouple is tied to the cell with 3 small wires, like twist ties. A small amount of Wakefi eld's Thermal Compound is placed at the site where the thermocouple junction touches the cell to ensure good thermal contact therebetween. The thermocouple junction is then covered with a small amount of glass wool. At the beginning ofthe test, the cell with attached thermocouple is lowered into the stabilized oven and hung in the center ofthe oven. The cell is at least 5 cm away from any oven shelf or wall. Then the oven and cell temperatures are measured automatically by computer until thermal runaway occurs or for 24 hours, which ever occurs first. In order to use Equations [ 17-22] above, a variety of parameters are needed. These include the surface heat conductivity per unit area, A, the cell thermal conductivity, K, and the jelly roll specific heat, C. The surface heat conductivity, N was measured by experiments using solid stainless steel, brass or aluminum cylinders of known radius, r, length, L, mass, m, specific heat, C, and density, p. A thermocouple was attached to the cylinder, and the cylinder was lowered into the oven. The temperature ofthe cylinder was measured as a function of time. Assuming that the temperature within the cylinder is uniform (it is a good approximation since the thermal conductivity of metals is large), the following is obtained for the oven temperature versus time: A L 2πr(T e -T) = C m dT/dt [23] where, T e is the environment temperature (oven temperature) and T is the cell temperature. Rearranging Equation [23] above gives: dT/dt = 2A(T e - T)/(rCp) [24]. A plot of dT/dt versus (T e - T) yields 2A/(rCp) as the slope. Since C and p are known for common metals, A is determined. A=0.00127 W/(cm 2 K) is measured for stainless steel. It is understood that surface heat conductivity depends on the details ofthe surface. For example, a stainless steel cylinder wrapped with a cell label has surface heat conductivity that is different from that of a bare stainless steel cylinder (i.e., cylinder without the label). In such a case, an actual label used on an actual cell may, for example, be applied to a known cylinder and the surface heat conductivity may be determined therefrom. The thermal conductivity of the jelly roll were taken from literature values (H. Maleki, A. Said, J.R. Selman, R. Dinwiddie, H. Wang, J Electrochem. Soc., 146 947 (1999)). The heat capacity of 18650 cells from manufacturer A were also obtained from the manufacturer. These parameters may be measured for arbitrary cells using the methods described in H. Maleki, A. Said, J.R. Selman, R. Dinwiddie, H. Wang, J. Electrochem. Soc, 146 947 (1999). Example #5 In the following example, oven exposure test results were calculated and compared to predicted results obtained in accordance with the principles ofthe present invention. MCMB and LiCoθ2 powders were obtained from battery manufacturer A. These powders are believed to be the similar to those used in 18650 size lithium-ion cells produced by that manufacturer. Using the accelerating rate calorimeter, power functions for the anode/electrolyte (0 V) and cathode/electrolyte (4.2 V) reactions were determined as described above. The power functions are given by Equation [7] for the cathode/electrolyte reaction and Equation [13] for the anode electrolyte reaction. The parameters used for these power functions are listed in Table 2 below. TABLE 2 Oven exposure test predictions were made using these power functions and Equations [17-19] with P e = 0.0. Oven temperatures of 140°C, 145°C, 150°C and 155°C were simulated. Figure 10A shows the results. Oven exposure experiments were made on 18650 size lithium-ion cells from manufacturer A. Start temperatures of 140°C, 145°C, 150°C and 155°C were used. The experimental results are plotted in Fig. 10B. It is clear that the calculation predicts the oven exposure results well. It is noted that the magnitude ofthe thermal runaway (for the 155°C oven test) is weaker in the calculation because only the first cathode/electrolyte exotherm is included in the model. Oven exposure experiments were also made on 17670 cells from manufacturer B. Power functions were not developed for the electrode materials used in those cells. Figure 1 IB shows the oven exposure test results. Clearly, the cells made by manufacturer B are less stable than those made by manufacturer A. If power functions for the materials used by manufacturer B were developed, the results in Fig. 1 IB could be predicted. On the other hand, attempting to match the results in Fig. 1 IB, such as by varying the parameters ofthe power functions, allows reasonable estimates to be made. Figure 11 A shows calculations to simulate the experiments in Fig. 1 IB. Only parameters ofthe cathode power functions were changed from the values listed in Table 2 above. The parameter H was increased to 450 J/g and γ was increased to 1.5 x 10 17 min "1 . Using this approximate set of parameters, predictions about the safety of other cell sizes and shapes could be made. Example #6 Once confidence in the method is achieved, it is then possible to predict oven exposure results for cells of different diameters. Figure 12, for example, shows predictions for oven exposure tests at 150°C for cells from manufacturer A as a function of cell radius. Clearly, it is evident that decreasing the cell radius improves the thermal stability ofthe cell. A critical radius of 1.2 cm is found for cells that can pass extended exposure to 150°C. It is appreciated that determining the critical radius for a particular cell design using the modeling approach ofthe present invention is significantly less complex, less time consuming, and less costly than assembling many cells of different diameters and then testing the assembled cells. Similar predictions may be made for planar cells without ever having to build planar prototype cells. The methodology described hereinabove for obtaining power functions and using same to model cell and battery level behavior in response to user prescribed thermal conditions and/or thermal abuse conditions may also be used to predict the response of such cells and batteries to other forms of environmental conditions/abuse, such as mechanical and electrical abuse. The discussion provided thus far has focused on how power functions determined by accelerating rate calorimetry or differential scanning calorimetry may be used to predict the behavior of lithium-ion batteries in the oven exposure test. Power functions may also be used to model cell/battery behavior when subjected to an overcharge test, a short-circuit test, and a nail penetration test, for example. In order to predict the response of cylindrical and planar cells to overcharge conditions, one only needs to add the electrically generated power per unit volume, P e , to the oven exposure scenario, and set the environmental temperature to a temperature near room temperature. The electrically generated power may be approximated by multiplying the current by the cell overvoltage. The cell overvoltage is defined as the terminal voltage under load minus the open circuit voltage at the nominal top of charge. For example, if a 3 A charging current is forced through a cell with a 4 V overvoltage, then 12 W of electrical power is dissipated in the cell. This value of electrical power is divided by the cell volume to arrive at P e . Calculations are then straightforward. According to one embodiment of an overcharge test modeling approach, a cell is charged for several times its rated capacity using a current that would normally give a full charge in a duration of time defined by 1/C of an hour. Normally C is selected to be 1 or 3 in this test. Once the normal chemistry ofthe charge process has been completed, the cell voltage rises to a value, V, which can be a volt or more above the open circuit voltage, V c , ofthe charged cell. The electrical power dissipated in the cell is then approximated by the equation P=I(V- V c ). This causes heating ofthe cell above ambient temperature. Eventually, the cell will reach a temperature where chemically generated power from the electrodes becomes significant. This can be calculated using the above-described power function approach. In order to make reasonable predictions of cell behavior during overcharge, a reasonable understanding ofthe variation of cell voltage with respect to time and current during the overcharge process is required. Also required is a knowledge ofthe amount of metallic lithium electroplated on the negative electrode during overcharge. For most lithium-ion cells, this is a concern. Power functions for negative electrodes containing plated metallic lithium would need to be developed in this case. Further, knowledge ofthe effect of electrolyte decomposition products at the positive electrode on the positive electrode power functions is required. Modeling of cell/battery behavior in response to an overcharge condition may be enhanced by performing experiments to first determine the various unknowns, which would otherwise be obtained using reasonable estimations and refinement of such estimations during the modeling exercise. In accordance with one embodiment of a short-circuit test modeling approach, a fully charged cell is equilibrated at some temperature, T. The cell is then short-circuited externally through a low impedance connection. Current flows and power is dissipated within the cell due to its internal impedance (I 2 R). This impedance varies as a function of temperature. The temperature ofthe cell rises, and the state of charge ofthe electrodes changes as the electrodes discharge. Once the cell reaches the separator shutdown point (e.g., near 130°C for a lithium-ion cell), the current flow stops and heat generated within the cell may be predicted by the power functions that correspond to the cell's present state of charge. Newton's law of cooling may be used to estimate heat transfer to the environment. Modeling of a short-circuit test is relatively straightforward, assuming that a good model for cell impedance as a function of temperature and state of charge is employed. Measurements could determine this accurately. Straightforward modeling ofthe short-circuit test also assumes that the power functions over the range ofthe state of charge ofthe cell "traversed" during the short-circuit are known. This would require measurements of power fiinctions at several lithium concentrations in both the positive and negative electrodes. In accordance with one embodiment of a nail penetration modeling approach, a nail having a point of a specified radius is forced into a cell at a specified rate. This causes an internal short-circuit ofthe cell. This results in intense heating at the site ofthe short-circuit which can lead to thermal runaway. Normally, cells are f illy charged before the test. As such, power functions for fully charged materials are needed. Cells filled with solvent only (not electrolyte) may be characterized by nail penetration. The resistance between the cell electrodes as a function of time may be measured as the nail is inserted. Once this resistance is known, then the short- circuit current that flows, as the nail is inserted in an electrolyte-filled cell, may be estimated. The electrically generated power, V 2 /R, is dissipated in the vicinity ofthe point ofthe nail. This causes local heating. The heat flow from this point may be treated with the above-described heat equation, preferably using a three- dimensional form with small spatial grid. As the temperature rises, the chemically generated power may be estimated using the power functions and hence a complete description ofthe nail penetration process may be obtained. A cell/battery behavior modeling approach which is based on power functions developed in accordance with the principles ofthe present invention may be implemented using modeling software running on a computer-based processing facility, such as a workstation, personal computer or other microprocessor-based computing system. In accordance with one embodiment, a software program provides for user- interactive cell/battery behavior modeling using a WINDOWS-like interface. Figures 13-20 are screen images of such an interface according to an embodiment ofthe present invention. In general terms, the user-interface allows the battery designer to create "virtual" cells of any shape and size and to predict the response ofthe virtual cells to user-specified conditions of thermal, electrical, and mechanical abuse. The user-interface allows the battery designer to load and modify anode, cathode, battery, and environmental parameters, and to graphically display the predicted behavior ofthe anode, cathode, and battery based on the loaded/modified parameters. As such, incremental changes may be made to the various virtual cell parameters to refine the behavior of a particular battery design. The cell/battery modeling software ofthe present invention provides for accurate mathematical modeling of virtual cell behavior based on power fiinctions developed from accelerating rate calorimetry or differential scanning calorimetry experiments on small quantities of particular electrode/electrolyte materials prepared in lab cells. One skilled in the art will immediately appreciate the significant cost and time saving advantages of a cell/battery design and modeling approach which requires the availability of only small amounts of sample electrode/electrolyte materials, and one in which cell prototype building and testing is completely eliminated. The cell/battery design and modeling approach ofthe present invention is particularly useful when developing "new" or advanced electrode/electrolyte materials which may be produced in small quantities but would be cost or time prohibitive to produce in large quantities. Since the power functions needed to f illy characterize cell-level/battery-level behavior for a new electrode/electrolyte material may be developed from calorimetry experiments on small quantities ofthe new material, it is believed that the cell modeling system and software ofthe present invention may significantly assist in the research and development of advanced cell technologies. According to one embodiment, the behavioral data of a known battery (e.g., a commercially available 18650 lithium-ion battery) when subjected to a thermal abuse test may be made available to the battery designer for purposes of providing a performance baseline or standard for a known cell technology. For example, experimentally derived temperature-time data for any number of known battery or cell types may be stored and accessed by the cell designer. Assuming that a "new" battery material has been developed and power functions obtained from a small sample of same in a manner discussed previously, the modeling software ofthe present invention may be used to plot temperature-time data for an 18650 battery having the new battery material. This plot may be compared against that of one or more known 18650 cell types to determine if the "new" battery is as safe, less safe, or safer than the known cell. It is understood that data that characterizes known cells is not necessary to the present invention, but may be used to enhance the process of evaluating new and different cell chemistries and configurations in relation to known cell designs. Referring now to Fig. 13, a main screen 300 of a user-interface according to an embodiment ofthe present invention includes a main menu bar 302 and a template region 304. The main menu bar 302 includes a number of control buttons, including, in particular, a Cathode button 306, an Anode button 307, and a Battery button 309. Each ofthe Cathode, Anode, and Battery buttons 306, 307, 309, when actuated, provides for the selection of additional particularized functions. As shown in Fig. 13, the Cathode button 306 has been activated which allows for additional selections associated with modeling the cathode of a virtual cell. Figure 14 depicts an input screen or dialog box 308 that is activated by selection ofthe Parameters button made available by actuation ofthe Cathode button 306 from the main menu bar 302, as is shown in Fig. 13. Activation ofthe Parameters button results in presentation of a Cathode Parameters dialog box 308, which provides for loading and adjusting of various cathode specific parameters by the battery designer. The Cathode Parameters dialog box 308 may be accessed via another route. Activation ofthe Load Parameters Set button, also shown in Fig. 13, brings up an Open File dialog box, from which the user selects a file. Upon selecting a file, the Cathode Parameters dialog box 308 is presented, which provides for loading and adjusting of various cathode specific parameters associated with the selected file. An input field 310 is provided for entering a value for Gamma, γ, which represents a frequency factor expressed in terms of minutes "1 . An input field 312 is provided for entering a value for the activation energy, E a , which is expressed in terms of electron volts (eV). The parameter u, which is the dimensional fractional (i.e., percentage) degree of conversion, may be entered using input field 314. An input field 316 is provided for entering a value for Beta, β, which represents the dimensionless parameter of autocatalysis. The value of h/C'tot may also be entered using input field 318, where h/C'tot represents the ratio ofthe total heat (h) evolved by the sample due to the reaction and the total heat capacity (C'tot) ofthe reactant and the sample bomb expressed in terms of °C. Figures 15 and 16 show dialog boxes 321 and 320 for entering parameters affecting the cathode calculations using accelerating rate calorimetry and differential scanning calorimetry techniques, respectively. Each ofthe dialog boxes 321 and 320 provided a Starting Temperature input field 323, 322, expressed in terms of °C. The dialog box 321 for inputting cathode accelerating rate calorimetry calculation parameters includes a Time input field 325, expressed in terms of hours. The dialog box 320 for inputting cathode differential scanning calorimetry calculation parameters includes a Heating Rate input field 324, expressed in terms of °C per minute. Figure 17 shows an Anode Parameters dialog box 330 which is activated by selection ofthe Parameters button made available upon actuation ofthe Anode button 307 from the main menu bar 302. Activation ofthe Parameters button results in the presentation ofthe Anode Parameters dialog box 330, which provides for loading and adjusting of various anode specific parameters by the battery designer. The Anode Parameters dialog box 330 may be accessed via a different route. Activation ofthe Load Parameters Set button, which becomes available upon actuating the Anode button 307 shown in Fig. 13, brings up an Open File dialog box from which the user selects a file. Upon selecting a file, the Anode. Parameters dialog box 330 is presented, which provides for loading and adjusting of various anode specific parameters associated with the selected file. An input field 332 is provided for entering a value for Gamma- 1, γi, and input field 334 provides for entering of a value for Gamma-2, γi, which . respectively represent frequency factors expressed in terms of minutes "1 . Input fields 336 and 338 provide for entering a value for activation energy parameters, Ei and E2, each of which is expressed in terms of electron volts (eV). The value of hi/C'tot and h2/C'tot may be entered using input fields 340 and 342, where the terms hi/C'tot and h∑/C'tot have units as described previously in Example #4 hereinabove. Anode Parameters dialog box 330 further includes an Anode m input field 344, where Anode m represents the reaction order for the reaction of type 1 to type 3 lithium. An Order input field 356 allows the designer to enter an Order value, which represents the reaction order for the reaction of type 2 to type 3 lithium. An Xfo input field 348 is provided to allow entering of a value for the anode parameter Xfo, which represents the term x 2o having units as described previously in Example #4 hereinabove. The anode parameter Xio, which represents the term xι 0 having units as described previously in Example #4 hereinabove, may be entered using Xio input field 350. A Zo input field 352 provides for entering of a value for the anode parameter Zo, which represents the term x 3o having units as described previously in Example #4 hereinabove. Figure 18 shows a dialog box 360 which is activated by selection ofthe Battery button 309 from the main menu bar 302. A Battery Parameters dialog box 360 provides for loading and adjusting of various battery level parameters by the battery designer. Input fields 362 and 364 provide for entering of Time (hrs) and Start Temperature (°C) values, respectively. An Oven Temperature field 366 allows the designer to input a temperature (°C) ofthe oven into which the cell will be placed in accordance with an oven exposure test. It is noted that the cell is initially at the Start Temperature. Mass input fields 368 and 370 provide for the input of mass values (g) for the anode and cathode, respectively. In Fig. 18, the Mass input fields 368 and 370 are specific for carbon and cobalt based electrodes, respectively, for a virtual lithium-ion battery. Values for battery heat capacity (J/gK), thermal conductivity (W/cmK), and density (g/cc) may be entered using input fields 372, 374, and 376, respectively. The Battery Parameters dialog box 360 further includes a Can Parameters region 380 which allows for the entering of various data that characterize the can or protective enclosure ofthe virtual battery. Can Parameters region 380 includes input fields 382, 384, 386, and 388 for entering values for can density (g/cc), heat capacity (J/gK), can surface heat conductivity (W/cm K), and can bulk thermal conductivity (W/cmK), respectively. The Battery Parameters dialog box 360 further includes a Battery Geometry region 390 which provides for the selection of several different virtual battery geometries. In the embodiment depicted in Fig. 18, a designer may activate a Cylindrical Geometry button 392 or a Prismatic Geometry button 394. Figure 19 shows a Cylindrical Calculation dialog box 400 which is presented to the designer in response to activating the Cylindrical Geometry button 392 provided in the Battery Geometry region 390. The designer may enter can length (cm) and radius (cm) values using Length and Radius input fields 402 and 404, respectively. The Cylindrical Calculation dialog box 400 further includes a Detail Level region 406 which permits the designer to activate a Full Detail button 408 and a Uniform Temperature button 410. Activation ofthe Full Detail button 408 results in a calculation that assumes that the temperature within the virtual cell varies with radius, as given by the above-described heat equation. Implemented on a PC equipped with a 266 MHz Pentium II processor, the Full Detail computation takes several minutes to complete. Activation ofthe Uniform Temperature button 410 results in a calculation that assumes that the temperature within the virtual cell is uniform (i.e., no radius dependence). This calculation is approximate, but is completed in seconds. The approximation is, however, reasonably accurate. Simulations have demonstrated that the typical core-can temperature difference is only a few degrees C, even during thermal runaway. Figure 20 shows a Prismatic Calculation dialog box 420 which is presented to the designer in response to activating the Prismatic Geometry button 394 provided in the Battery Geometry region 390 shown in Fig. 18. The designer may enter can length (cm), width (cm), and thickness (cm) values using Length, Width, and Thickness input fields 422, 424, and 425, respectively. The Prismatic Calculation dialog box 420 also includes a Detail Level region 426 which permits the designer to activate Full Detail and Uniform Temperature buttons 428 and 430. Activation ofthe Full Detail button 428 results in a calculation that assumes that the temperature within the virtual cell varies with thickness, as given by the above-described heat equation. As in the case of a cylindrical cell geometry, activation ofthe Uniform Temperature button 430 results in a calculation that assumes that the temperature within the virtual cell is uniform (i.e., no thickness dependence). A computer assisted method for predicting the response of electrochemical cells to thermal, electrical, and/or mechanical abuse according to the present invention may thus be effected, for example, by a processor implementing a sequence of machine-readable instructions. These instructions may reside in various types of signal -bearing media. In this respect, another embodiment ofthe present invention concerns a programmed product which includes a signal-bearing medium embodying a program of machine-readable instructions, executable by a digital processor to perform method steps to effect cell modeling and behavior prediction procedures ofthe present invention. The signal-bearing media may include, for example, random access memory (RAM) provided within, or otherwise coupled to, the processor. Alternatively, the instructions may be contained in other signal-bearing media, such as one or more magnetic data storage diskettes, direct access data storage disks (e.g., a conventional hard drive or a RAID array), magnetic tape, alterable or non-alterable electronic read-only memory (e.g., EEPROM, ROM), flash memory, optical storage devices (e.g., CDROM or WORM), signal-bearing media including transmission media such as digital, analog, and communication links and wireless, and propagated signal media. In an illustrative embodiment, the machine-readable instructions may constitute lines of compiled "C" language code or "C++" object-oriented code. The foregoing description ofthe various embodiments ofthe invention has been presented for the purposes of illustration and description. It is not intended to be exhaustive or to limit the invention to the precise form disclosed. Many modifications and variations are possible in light ofthe above teaching. It is intended that the scope ofthe invention be limited not by this detailed description, but rather by the claims appended hereto.

Claims: CLAIMS What we claim is: 1. A method of characterizing electrochemical cell components, comprising: preparing a sample of an electrode material in contact with an electrolyte; obtaining self-heating data, power-temperature data or power-time data for the sample using a calorimetry technique; and developing a power function for the sample using the self-heating, power-temperature or power-time data, the power function representative of thermal power per unit mass ofthe sample as a function of temperature and amount of reactant remaining from a reaction ofthe electrode material and electrolyte ofthe sample. 2. The method of claim 1, wherein preparing the sample comprises preparing the sample using less than about 100 grams ofthe electrode material. 3. The method of claim 1, wherein the electrode material comprises cathode material or anode material. 4. The method of claim 1, wherein obtaining the self-heating data comprises obtaining temperature versus time data ofthe sample during reaction under substantially adiabatic conditions. 5. A method of characterizing electrochemical cell components, comprising: preparing a first sample of a cathode material in contact with an electrolyte; preparing a second sample of an anode material in contact with the electrolyte; obtaining first and second self-heating, power-temperature or power-time data for the first and second samples, respectively, using a calorimetry technique; and developing a first power function for the first sample and a second power function for the second sample using the first and second self-heating, power-temperature or power-time data, respectively, the first power function characterizing a reaction between the cathode material and the electrolyte in terms of thermal power per unit mass ofthe cathode sample material, and the second power function characterizing a reaction between the anode material and the electrolyte in terms of thermal power per unit mass ofthe anode sample material. 6. The method of claim 5, wherein obtaining the first and second self- heating data comprises obtaining temperature versus time data ofthe first and second samples during reaction under substantially adiabatic conditions, respectively. 7. A method of characterizing an electrochemical cell, comprising: defining one or more physical parameters ofthe electrochemical cell; providing a first power function characterizing a reaction between a cathode and an electrolyte in terms of thermal power per unit mass of cathode material; providing a second power function characterizing a reaction between an anode and the electrolyte in terms of thermal power per unit mass of anode material; and predicting, using the first and second power functions and the physical parameters ofthe electrochemical cell, a response ofthe cell to a specified operating condition. 8. The method of claim 7, wherein: defining one or more physical parameters ofthe cell further comprises adjusting the physical parameters ofthe cell; and predicting the response ofthe cell further comprises predicting the response ofthe cell using the first and second power functions and the adjusted physical parameters ofthe cell. 9. The method of claim 7, wherein defining one or more physical parameters ofthe cell further comprises: defining physical parameters for each of an anode and a cathode of the cell; adjusting the physical parameters of one or both ofthe anode and cathode; and predicting the response ofthe cell using the first and second power functions and the adjusted physical parameters of one or both ofthe anode and cathode. 10. A system for characterizing an electrochemical cell, comprising: a processor; a user-interface, coupled to the processor, comprising an input device operable by a user for entering one or more physical parameters ofthe electrochemical cell; and memory, coupled to the processor, that stores a cathode power function characterizing a reaction between a cathode and an electrolyte in terms of thermal power per unit mass of cathode material and further stores an anode power function characterizing a reaction between an anode and the electrolyte in terms of thermal power per unit mass of anode material, the processor computing a response of an electrochemical cell to a specified operating condition using the cathode and anode power functions and the physical parameters ofthe electrochemical cell. 11. The system of claim 10, wherein: the input device is operable by the user to adjust physical parameters ofthe cell; and the processor computes the response ofthe electrochemical cell to the specified operating condition using the cathode and anode power functions and the adjusted physical parameters ofthe electrochemical cell. 12. The system of claim 10, wherein: the input device is operable by the user to adjust physical parameters of an anode and a cathode ofthe cell; and the processor computes the response ofthe electrochemical cell to the specified operating condition using the cathode and anode power functions and the adjusted physical parameters ofthe anode and cathode ofthe electrochemical cell. 13. The system of claim 10, further comprising a calorimeter system coupled to the processor. 14. A method of characterizing electrochemical cell components, comprising: defining one or more physical parameters of an electrochemical cell; characterizing a reaction between a cathode and an electrolyte in terms of thermal power per unit mass of cathode material by defining a first power function; characterizing a reaction between an anode and the electrolyte in terms of thermal power per unit mass of anode material by defining a second power function; and predicting, using the first and second power functions and the physical parameters ofthe electrochemical cell, a response ofthe cell to a specified operating condition. 15. A computer readable medium embodying program instructions for characterizing electrochemical cell components, comprising: characterizing a reaction between a cathode and an electrolyte in terms of thermal power per unit mass of cathode material by defining a first power function; characterizing a reaction between an anode and the electrolyte in terms of thermal power per unit mass of anode material by defining a second power function; defining one or more physical parameters ofthe electrochemical cell; and predicting, using the first and second power functions and the physical parameters ofthe electrochemical cell, a response ofthe cell to a specified operating condition. 16. The respective method and medium of claims 14 and 15, wherein characterizing the respective cathode/electrolyte and anode/electrolyte reactions comprises modeling the respective reactions assuming an autocatalytic reaction mechanism. 17. The respective method and medium of claims 14 and 15, wherein characterizing the first and second power functions comprises using a calorimetry technique. 18. The respective methods and medium of claims 1, 5 and 17, wherein the calorimetry technique comprises an accelerating rate calorimetry technique or a differential scanning calorimetry technique. 19. The method of claims 7 and 14, wherein the specified operating condition comprises a condition of constant or varying ambient temperature, a condition of a constant or varying current applied to the cell, a condition of an external short-circuit connected to the cell, or a condition of a short-circuit internal to the cell. 20. The respective method and medium of claims 14 and 15, wherein characterizing the first and second power functions comprises obtaining temperature versus time data of each ofthe cathode/electrolyte and anode/electrolyte reactions. 21. The respective method and medium of claims 14 and 15, wherein: characterizing the cathode/electrolyte reaction comprises characterizing the cathode/electrolyte reaction using less than about 100 grams of cathode material; and characterizing the anode/electrolyte reaction comprises characterizing the anode/electrolyte reaction using less than about 100 grams of anode material.

Inventors: DAHN JEFFERY R, HATCHARD TIMOTHY D, MACNEIL DEAN D, DAHN, JEFFERY, R., HATCHARD, TIMOTHY, D., MACNEIL, DEAN, D.
Applicants: 3M INNOVATIVE PROPERTIES CO, 3M INNOVATIVE PROPERTIES COMPANY
Application year: 2000
Main classification: H01M10
IPC codes: G01N25, H01M4, H01M10