# Thermodynamic Properties of Hydrogen + Tetra-n-Butyl Ammonium Bromide Semi-Clathrate Hydrate

Authors: Shunsuke Hashimoto; Takaaki Tsuda; Kyohei Ogata; Takeshi Sugahara; Yoshiro Inoue; Kazunari Ohgaki
Journal: Journal of Thermodynamics
 (2010)

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## Abstract

Thermodynamic stability and hydrogen occupancy on the hydrogen + tetra-n-butyl ammonium bromide semi-clathrate hydrate were investigated by means of Raman spectroscopic and phase equilibrium measurements under the three-phase equilibrium condition. The structure of mixed gas hydrates changes from tetragonal to another structure around 95 MPa and 292 K depending on surrounding hydrogen fugacity. The occupied amount of hydrogen in the semi-clathrate hydrate increases significantly associated with the structural transition. Tetra-n-butyl ammonium bromide semi-clathrate hydrates can absorb hydrogen molecules by a pressure-swing without destroying the hydrogen bonds of hydrate cages at 15 MPa or over.


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## Body

## 1. Introduction

Recently, gas  hydrates and other clathrate materials [1] have become one of attractive media that have a huge potential for effective applications of H2 storage and transportation. The H2-mixed gas hydrates with the assistance of suitable additives enable us to perform the H2 storage under much lower-pressure conditions than the simple H2 hydrate [2]. Tetrahydrofuran (hereafter, THF) and tetra-n-butyl ammonium salts are well known as the additives [3–9]. In addition, the reversible technique of storage and/or release of H2 by pressurizing or depressurizing without the destruction of hydrate cages are more suitable for the H2 storage than H2 absorbing alloys. For example, in the case of metal hydride, H2 storage amount of Mg2Ni (A2B type, relatively light material) is 3.6 mass%. However, the H2 storage and release of these metal hydrides are often accompanied by a relatively large enthalpy-change of 30–60 kJ/mol. On the other hand, although H2 storage amount of clathrate hydrate is smaller than that of metal hydride, the heating to release H2 is unnecessary for the reversible technique of storage and release of H2 by pressurizing and depressurizing. There are some reports about above storage and release method on the THF hydrate [10–12].The hydrate formed from tetra-n-butyl ammonium salt solution has been known as a semi-clathrate hydrate where the quaternary ammonium cation and anion are incorporated with the water molecules to construct the hydrate cage [13]. It is reported that tetra-n-butyl ammonium salts can form various unit-cell structures. For example, tetra-n-butyl ammonium bromide (hereafter, TBAB) forms two unit-cell structures (tetragonal and orthorhombic) depending on the concentration of aqueous solution [14, 15]. In our previous study, the cage occupancy of H2 has been investigated by use of phase equilibrium measurements and Raman spectroscopic analyses for two structures of H2 + TBAB semi-clathrate hydrates up to 15 MPa [8]. Most recently, we have reported that hydrogen-induced structural transition from cubic to another structure (probably tetragonal) occurs on H2 + tetra-n-butyl ammonium fluoride (hereafter, TBAF) semi-clathrate hydrate [16]. The storage amount of H2 in H2 + TBAF semi-clathrate hydrate drastically increases with the structural transition. These results imply that hydrogen bonds of semi-clathrate hydrate have flexibility.In the present study onH2 + TBAB semi-clathrate hydrates, we have two research objectives: (1) thermodynamic property including hydrate structures and H2 occupancy,  and (2) capability of reversible storage and release and storage capacity of H2. Firstly, the cage occupancy of H2 and structural transition for the H2 + TBAB semi-clathrate hydrate under the three-phase equilibrium conditions were investigated by use of  in situ Raman spectroscopy. Secondly, phase equilibrium (pressure-temperature) relations for the ternary mixtures of H2 + TBAB + water at two TBAB concentrations were measured in the pressure region of 15–190 MPa. Finally, the capability of reversible storage and release of H2 was evaluated by in situ Raman spectroscopic analysis using isothermal pressure-swing.


## 2. Experimental Section

### 2.1. Materials

Research-gradeH2 (six nine purity), having the maximum impurity of 0.2 ppm nitrogen, was obtained from the Neriki Gas Co., Ltd. Research grade TBAB of 98 mol% up and the distilled water were obtained from the Wako Pure Chemical Industries, Ltd. All of them were used without further purifications.


### 2.2. Apparatus

A high-pressure optical cell for both the phase equilibrium and the Raman spectroscopic measurements had a pair of sapphire (Ti free) windows on both the upper and lower sides. The high-pressure optical cell was the same as previous one [16] except for the window material. The maximum working pressure of high-pressure optical cell was 400 MPa. The temperature-controlled water was circulated constantly in the exterior jacket of the high-pressure optical cell. A ruby ball was enclosed into the high-pressure optical cell. The contents were agitated by the ruby ball, which was rolled around by the vibration from outside.The system temperature was measured within an uncertainty of 0.02 K using a thermistor probe (Takara D-632), which was inserted into a hole in the cell wall. The probe was calibrated with a Pt resistance thermometer defined by ITS-90. The system pressure was measured by a pressure gage (Valcom VPRT) calibrated by RUSKA quartz Bourdon tube gage (Direct Reading Pressure Gage, series 6000) with an estimated maximum uncertainty of 0.01 MPa (low pressure)–0.1 MPa (high pressure).


### 2.3. Procedures

#### 2.3.1. Thermodynamic Property

The aqueous TBAB solution prepared at a desired concentration (x=0.037 which is the stoichiometric concentration of tetragonal TBAB hydrate, or 0.020 which is lower than the stoichiometric concentration of orthorhombic TBAB hydrate [14]) was introduced into the evacuated high-pressure optical cell. The contents were pressurized up to a desired pressure by supplying H2 and then cooled and agitated with an enclosed ruby ball to prepare the gas hydrate. After the formation of gas hydrates, the system temperature was risen gradually (about 0.1 K/hour) to leave a few seed crystals. In this state, the system temperature was kept constant for more than one day, and the three-phase equilibrium condition was determined. Since then the system temperature was dropped little by little (about 0.05 K/hour) to prepare the single crystal of gas hydrate under the three-phase (hydrate + aqueous solution + gas) coexisting state. We also paid enough attention to preparing as few single crystals as possible. This single crystal was analyzed through a sapphire window (Ti free) by in situ Raman spectroscopy using a laser Raman microprobe spectrophotometer with multichannel CCD detector. The argon ion laser beam (wavelength: 514.5 nm) condensed to 2 μm in spot diameter from the object lens was irradiated to the sample through the upper sapphire window. The backscatter of the opposite direction was taken in with the same lens. The spectral resolution was ~0.7 cm-1.


#### 2.3.2. Storage Capacity ofH2

In the isothermal Raman spectroscopic measurement, an aqueous TBAB solution prepared atx=0.037 was introduced into the evacuated high-pressure optical cell. To prepare the TBAB hydrate, the contents were supercooled and agitated with an enclosed ruby ball. After the formation of gas hydrates, the system temperature was kept constant,  and the contents were annealed for more than one day at 283.15 K to complete the hydrate crystallization, which was slightly lower than the equilibrium temperature of TBAB hydrate at atmospheric pressure. Then, the contents were pressurized up to a desired pressure by supplying H2, and the cell was kept static to establish the two-phase (H2 gas and hydrate phases) equilibrium state. After one day, the hydrate phase was analyzed under the isothermal condition (283.15 K) through a sapphire window by in situ Raman spectroscopy.In addition, theH2 + TBAB hydrate was prepared from compressed H2 and aqueous solution in advance, and H2 was once released from the H2 + TBAB hydrate at 283.15 K by depressurization. Then, the TBAB hydrate was pressurized again up to a desired pressure by H2, and after one day or more, the hydrate was analyzed under isothermal two-phase equilibrium condition by in situ Raman spectroscopy. For convenience, the description of  “repressurizing method’’  is adopted hereafter in this paper.


## 2.1. Materials

Research-gradeH2 (six nine purity), having the maximum impurity of 0.2 ppm nitrogen, was obtained from the Neriki Gas Co., Ltd. Research grade TBAB of 98 mol% up and the distilled water were obtained from the Wako Pure Chemical Industries, Ltd. All of them were used without further purifications.


## 2.2. Apparatus

A high-pressure optical cell for both the phase equilibrium and the Raman spectroscopic measurements had a pair of sapphire (Ti free) windows on both the upper and lower sides. The high-pressure optical cell was the same as previous one [16] except for the window material. The maximum working pressure of high-pressure optical cell was 400 MPa. The temperature-controlled water was circulated constantly in the exterior jacket of the high-pressure optical cell. A ruby ball was enclosed into the high-pressure optical cell. The contents were agitated by the ruby ball, which was rolled around by the vibration from outside.The system temperature was measured within an uncertainty of 0.02 K using a thermistor probe (Takara D-632), which was inserted into a hole in the cell wall. The probe was calibrated with a Pt resistance thermometer defined by ITS-90. The system pressure was measured by a pressure gage (Valcom VPRT) calibrated by RUSKA quartz Bourdon tube gage (Direct Reading Pressure Gage, series 6000) with an estimated maximum uncertainty of 0.01 MPa (low pressure)–0.1 MPa (high pressure).


## 2.3. Procedures

### 2.3.1. Thermodynamic Property

The aqueous TBAB solution prepared at a desired concentration (x=0.037 which is the stoichiometric concentration of tetragonal TBAB hydrate, or 0.020 which is lower than the stoichiometric concentration of orthorhombic TBAB hydrate [14]) was introduced into the evacuated high-pressure optical cell. The contents were pressurized up to a desired pressure by supplying H2 and then cooled and agitated with an enclosed ruby ball to prepare the gas hydrate. After the formation of gas hydrates, the system temperature was risen gradually (about 0.1 K/hour) to leave a few seed crystals. In this state, the system temperature was kept constant for more than one day, and the three-phase equilibrium condition was determined. Since then the system temperature was dropped little by little (about 0.05 K/hour) to prepare the single crystal of gas hydrate under the three-phase (hydrate + aqueous solution + gas) coexisting state. We also paid enough attention to preparing as few single crystals as possible. This single crystal was analyzed through a sapphire window (Ti free) by in situ Raman spectroscopy using a laser Raman microprobe spectrophotometer with multichannel CCD detector. The argon ion laser beam (wavelength: 514.5 nm) condensed to 2 μm in spot diameter from the object lens was irradiated to the sample through the upper sapphire window. The backscatter of the opposite direction was taken in with the same lens. The spectral resolution was ~0.7 cm-1.


### 2.3.2. Storage Capacity ofH2

In the isothermal Raman spectroscopic measurement, an aqueous TBAB solution prepared atx=0.037 was introduced into the evacuated high-pressure optical cell. To prepare the TBAB hydrate, the contents were supercooled and agitated with an enclosed ruby ball. After the formation of gas hydrates, the system temperature was kept constant,  and the contents were annealed for more than one day at 283.15 K to complete the hydrate crystallization, which was slightly lower than the equilibrium temperature of TBAB hydrate at atmospheric pressure. Then, the contents were pressurized up to a desired pressure by supplying H2, and the cell was kept static to establish the two-phase (H2 gas and hydrate phases) equilibrium state. After one day, the hydrate phase was analyzed under the isothermal condition (283.15 K) through a sapphire window by in situ Raman spectroscopy.In addition, theH2 + TBAB hydrate was prepared from compressed H2 and aqueous solution in advance, and H2 was once released from the H2 + TBAB hydrate at 283.15 K by depressurization. Then, the TBAB hydrate was pressurized again up to a desired pressure by H2, and after one day or more, the hydrate was analyzed under isothermal two-phase equilibrium condition by in situ Raman spectroscopy. For convenience, the description of  “repressurizing method’’  is adopted hereafter in this paper.


## 2.3.1. Thermodynamic Property

The aqueous TBAB solution prepared at a desired concentration (x=0.037 which is the stoichiometric concentration of tetragonal TBAB hydrate, or 0.020 which is lower than the stoichiometric concentration of orthorhombic TBAB hydrate [14]) was introduced into the evacuated high-pressure optical cell. The contents were pressurized up to a desired pressure by supplying H2 and then cooled and agitated with an enclosed ruby ball to prepare the gas hydrate. After the formation of gas hydrates, the system temperature was risen gradually (about 0.1 K/hour) to leave a few seed crystals. In this state, the system temperature was kept constant for more than one day, and the three-phase equilibrium condition was determined. Since then the system temperature was dropped little by little (about 0.05 K/hour) to prepare the single crystal of gas hydrate under the three-phase (hydrate + aqueous solution + gas) coexisting state. We also paid enough attention to preparing as few single crystals as possible. This single crystal was analyzed through a sapphire window (Ti free) by in situ Raman spectroscopy using a laser Raman microprobe spectrophotometer with multichannel CCD detector. The argon ion laser beam (wavelength: 514.5 nm) condensed to 2 μm in spot diameter from the object lens was irradiated to the sample through the upper sapphire window. The backscatter of the opposite direction was taken in with the same lens. The spectral resolution was ~0.7 cm-1.


## 2.3.2. Storage Capacity ofH2

In the isothermal Raman spectroscopic measurement, an aqueous TBAB solution prepared atx=0.037 was introduced into the evacuated high-pressure optical cell. To prepare the TBAB hydrate, the contents were supercooled and agitated with an enclosed ruby ball. After the formation of gas hydrates, the system temperature was kept constant,  and the contents were annealed for more than one day at 283.15 K to complete the hydrate crystallization, which was slightly lower than the equilibrium temperature of TBAB hydrate at atmospheric pressure. Then, the contents were pressurized up to a desired pressure by supplying H2, and the cell was kept static to establish the two-phase (H2 gas and hydrate phases) equilibrium state. After one day, the hydrate phase was analyzed under the isothermal condition (283.15 K) through a sapphire window by in situ Raman spectroscopy.In addition, theH2 + TBAB hydrate was prepared from compressed H2 and aqueous solution in advance, and H2 was once released from the H2 + TBAB hydrate at 283.15 K by depressurization. Then, the TBAB hydrate was pressurized again up to a desired pressure by H2, and after one day or more, the hydrate was analyzed under isothermal two-phase equilibrium condition by in situ Raman spectroscopy. For convenience, the description of  “repressurizing method’’  is adopted hereafter in this paper.


## 3. Results and Discussion

### 3.1. Thermodynamic Property

The Raman spectra for theH2 + TBAB semi-clathrate hydrate system under the three-phase equilibrium condition are shown in Figures 1 (x=0.037) and 2 (x=0.020). The characteristic Raman peaks derived from TBAB molecule are detected around 700–1500 cm-1  and 2800–3000 cm-1 in the hydrate phase. The figures also include the single peak (4132 cm-1) of H2 stretching vibration and the broad peak (around 3100 cm-1) corresponding to the O–H vibration of host water lattice for the H2 + TBAB semi-clathrate hydrate. The H2 vibration peak is normalized by use of one of TBAB peaks. The position and shape of the peak derived from H2 obtained in the present study agree well with those of previous reports [6, 8]. The Raman spectra reveal that the H2 selectively occupies the empty S-cages of semi-clathrate hydrate, while the butyl-group of TBAB molecule occupies the other cages completely under the present experimental conditions.Figure 1
Raman spectra originated in TBAB,H2, and host lattice of water for the H2 + TBAB semi-clathrate hydrate at x = 0.037. Closed inverted-triangle represents the peak used for the normalization of H2 vibration peak.Figure 2
Raman spectra originated in TBAB,H2, and host lattice of water for the H2 + TBAB semi-clathrate hydrate at x=0.020. Closed inverted-triangle represents the peak used for the normalization of H2 vibration peak.Normalized peak ofH2 vibration becomes larger and larger with the pressure increasing, which means the increase of entrapped H2 molecules. As shown in Figure 1, in the case of x=0.037, Raman peak ratio of H2 to TBAB increases gradually as pressure increasing until ca. 100 MPa, while the increment of H2 peak with pressure increasing seems to become small in the higher-pressure region. On the other hand, in the case of x=0.020, Raman peak ratio of H2 changes discontinuously around 100 MPa as shown in Figure 2 (shaded region). The normalized peak area of H2 in the case of x=0.020 increases dramatically compared with that of x=0.037 at similar pressure more than 99 MPa. In addition, the Raman peaks of TBAB and water change significantly on reaching ca. 100 MPa in x=0.020, which differs in results from the case of x=0.037. The peaks of TBAB at high pressures in x=0.020 are closely similar to those of the other structure (probably orthorhombic) obtained in our previous study [8]. The orthorhombic structure (TBAB∙38H2O) [15] has more empty S-cages and can entrap much more H2 than the tetragonal one (TBAB∙26H2O).The phase equilibrium (pressure-temperature) relations for theH2 + TBAB semi-clathrate hydrate systems are summarized in Table 1 and shown in Figure 3. The three-phase equilibrium curves obtained in the present study join smoothly with those of our previous data [6, 8]. The characteristic slope change (dp/dT) derived from the structural transition on the three-phase equilibrium curve exists at ~95 MPa and 292 K only in the case of x=0.020. The phase behavior and structural transition of H2 + TBAB semi-clathrate hydrate system are closely similar to those of H2 + TBAF semi-clathrate hydrate system [16], except that the transition condition of H2 + TBAB semi-clathrate hydrate is much severer (the transition pressure is ~90 MPa higher) than that of H2 + TBAF semi-clathrate hydrate [16].Table 1
Three-phase equilibrium conditions ofH2 + TBAB semi-clathrate hydrate at the TBAB mole fraction of 0.020 and 0.037 in high-pressure region. The conditions in low-pressure region are shown in our previous papers [6, 8]. x represents the mole fraction of TBAB aqueous solution.
T (K)p  (MPa)T  (K)p (MPa)x=0.020286.4519.5x=0.037288.3523.1288.2335.6tetragonal291.5658.7290.0758.0293.9599.2↑290.9778.8295.86143.9tetragonal291.5391.6297.85185.0new structure292.87101.3↓294.75140.6Figure 3
Three-phase equilibrium curves of theH2 + TBAB semi-clathrate hydrates; closed keys represent the three-phase equilibrium points of simple TBAB semi-clathrate hydrates under the atmospheric conditions. The solid lines are fitting lines for experimental data.


### 3.2. Storage Capacity ofH2

Raman spectroscopy exhibits thatH2 can be absorbed in TBAB hydrates without destroying the hydrogen bonds of hydrate cages at 15 MPa or over by use of isothermal pressure-swing. The results from “repressurizing method” (please refer to the experimental section for details) are shown in Figure 4 accompanied with those of Raman spectroscopic measurement under the stability boundary conditions. The y-axis represents the peak area of H2 normalized by one of peaks corresponding to TBAB molecule. As shown in Figure 4, normalized Raman peak area of H2 resulted from isothermal pressure-swing increases gradually as pressure rises  and is coincident with the H2 peak area measured under the stability boundary conditions. In the case of H2 absorption to fresh TBAB hydrate, Raman peak area of H2 reaches only about 70% of the value obtained from “repressurizing method” at the same pressure. These results disagree with those of s-II THF hydrate system [11]. The discrepancy in hydrate structures results in that H2 cannot diffuse freely in fresh TBAB hydrate because the empty S-cages do not connect successively. In the case of “repressurizing method,”  the release of H2 from H2 + TBAB hydrate induces the secondary structural change of TBAB hydrate; for example, the position of nitrogen or bromine atom connected with host water  may be  changed. In fact, the crystal appearance of TBAB hydrate changes from clear to cloudy at the moment H2 released from H2 + TBAB hydrate. The secondary TBAB hydrate prepared by H2 release from H2 + TBAB hydrate may enable us to perform the reversible H2 storage and release. Figure 4 also shows that the normalized peak area of H2 is not saturated even if the pressure reaches about 200 MPa;  that is, the empty S-cages cannot be occupied completely by H2 at least 200 MPa.Figure 4
Pressure dependence of normalized Raman peak area corresponding toH2 for the H2 + TBAB semi-clathrate hydrate system.


## 3.1. Thermodynamic Property

The Raman spectra for theH2 + TBAB semi-clathrate hydrate system under the three-phase equilibrium condition are shown in Figures 1 (x=0.037) and 2 (x=0.020). The characteristic Raman peaks derived from TBAB molecule are detected around 700–1500 cm-1  and 2800–3000 cm-1 in the hydrate phase. The figures also include the single peak (4132 cm-1) of H2 stretching vibration and the broad peak (around 3100 cm-1) corresponding to the O–H vibration of host water lattice for the H2 + TBAB semi-clathrate hydrate. The H2 vibration peak is normalized by use of one of TBAB peaks. The position and shape of the peak derived from H2 obtained in the present study agree well with those of previous reports [6, 8]. The Raman spectra reveal that the H2 selectively occupies the empty S-cages of semi-clathrate hydrate, while the butyl-group of TBAB molecule occupies the other cages completely under the present experimental conditions.Figure 1
Raman spectra originated in TBAB,H2, and host lattice of water for the H2 + TBAB semi-clathrate hydrate at x = 0.037. Closed inverted-triangle represents the peak used for the normalization of H2 vibration peak.Figure 2
Raman spectra originated in TBAB,H2, and host lattice of water for the H2 + TBAB semi-clathrate hydrate at x=0.020. Closed inverted-triangle represents the peak used for the normalization of H2 vibration peak.Normalized peak ofH2 vibration becomes larger and larger with the pressure increasing, which means the increase of entrapped H2 molecules. As shown in Figure 1, in the case of x=0.037, Raman peak ratio of H2 to TBAB increases gradually as pressure increasing until ca. 100 MPa, while the increment of H2 peak with pressure increasing seems to become small in the higher-pressure region. On the other hand, in the case of x=0.020, Raman peak ratio of H2 changes discontinuously around 100 MPa as shown in Figure 2 (shaded region). The normalized peak area of H2 in the case of x=0.020 increases dramatically compared with that of x=0.037 at similar pressure more than 99 MPa. In addition, the Raman peaks of TBAB and water change significantly on reaching ca. 100 MPa in x=0.020, which differs in results from the case of x=0.037. The peaks of TBAB at high pressures in x=0.020 are closely similar to those of the other structure (probably orthorhombic) obtained in our previous study [8]. The orthorhombic structure (TBAB∙38H2O) [15] has more empty S-cages and can entrap much more H2 than the tetragonal one (TBAB∙26H2O).The phase equilibrium (pressure-temperature) relations for theH2 + TBAB semi-clathrate hydrate systems are summarized in Table 1 and shown in Figure 3. The three-phase equilibrium curves obtained in the present study join smoothly with those of our previous data [6, 8]. The characteristic slope change (dp/dT) derived from the structural transition on the three-phase equilibrium curve exists at ~95 MPa and 292 K only in the case of x=0.020. The phase behavior and structural transition of H2 + TBAB semi-clathrate hydrate system are closely similar to those of H2 + TBAF semi-clathrate hydrate system [16], except that the transition condition of H2 + TBAB semi-clathrate hydrate is much severer (the transition pressure is ~90 MPa higher) than that of H2 + TBAF semi-clathrate hydrate [16].Table 1
Three-phase equilibrium conditions ofH2 + TBAB semi-clathrate hydrate at the TBAB mole fraction of 0.020 and 0.037 in high-pressure region. The conditions in low-pressure region are shown in our previous papers [6, 8]. x represents the mole fraction of TBAB aqueous solution.
T (K)p  (MPa)T  (K)p (MPa)x=0.020286.4519.5x=0.037288.3523.1288.2335.6tetragonal291.5658.7290.0758.0293.9599.2↑290.9778.8295.86143.9tetragonal291.5391.6297.85185.0new structure292.87101.3↓294.75140.6Figure 3
Three-phase equilibrium curves of theH2 + TBAB semi-clathrate hydrates; closed keys represent the three-phase equilibrium points of simple TBAB semi-clathrate hydrates under the atmospheric conditions. The solid lines are fitting lines for experimental data.


## 3.2. Storage Capacity ofH2

Raman spectroscopy exhibits thatH2 can be absorbed in TBAB hydrates without destroying the hydrogen bonds of hydrate cages at 15 MPa or over by use of isothermal pressure-swing. The results from “repressurizing method” (please refer to the experimental section for details) are shown in Figure 4 accompanied with those of Raman spectroscopic measurement under the stability boundary conditions. The y-axis represents the peak area of H2 normalized by one of peaks corresponding to TBAB molecule. As shown in Figure 4, normalized Raman peak area of H2 resulted from isothermal pressure-swing increases gradually as pressure rises  and is coincident with the H2 peak area measured under the stability boundary conditions. In the case of H2 absorption to fresh TBAB hydrate, Raman peak area of H2 reaches only about 70% of the value obtained from “repressurizing method” at the same pressure. These results disagree with those of s-II THF hydrate system [11]. The discrepancy in hydrate structures results in that H2 cannot diffuse freely in fresh TBAB hydrate because the empty S-cages do not connect successively. In the case of “repressurizing method,”  the release of H2 from H2 + TBAB hydrate induces the secondary structural change of TBAB hydrate; for example, the position of nitrogen or bromine atom connected with host water  may be  changed. In fact, the crystal appearance of TBAB hydrate changes from clear to cloudy at the moment H2 released from H2 + TBAB hydrate. The secondary TBAB hydrate prepared by H2 release from H2 + TBAB hydrate may enable us to perform the reversible H2 storage and release. Figure 4 also shows that the normalized peak area of H2 is not saturated even if the pressure reaches about 200 MPa;  that is, the empty S-cages cannot be occupied completely by H2 at least 200 MPa.Figure 4
Pressure dependence of normalized Raman peak area corresponding toH2 for the H2 + TBAB semi-clathrate hydrate system.


## 4. Conclusion

The thermodynamic stability andH2 occupancy for the H2 + TBAB semi-clathrate hydrate system were investigated by phase equilibrium (pressure-temperature) relation and Raman spectra measured at two mole fractions (x=0.020 or 0.037) of TBAB aqueous solution. In the case of x=0.020, the structural transition from tetragonal to another structure is occurred around 95 MPa and 292 K. The structure after the structural transition can store much more H2 molecules than the tetragonal one. Raman spectroscopic analysis with isothermal pressure-swing absorption reveals that H2 can be absorbed in the TBAB hydrates without destroying the hydrogen bonds of hydrate cages. The storage amount of H2 for the repressurization to the used TBAB hydrate after H2 release increases compared with that of fresh TBAB hydrate. It remains possible to perform the reversible storage and release of H2 in TBAB hydrate without destroying hydrate cages.



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*Source: 170819-2009-12-10.xml*