User: 

what makes temperature temperature
Assistant:  ""Temperature" is a measure of how hot or cold something is, which corresponds to the average kinetic energy of the particles (atoms or molecules) in a substance.

Here's what makes temperature *temperature*:

1. **Kinetic Energy of Particles:**  
   Temperature reflects the average kinetic energy of the particles in a material. When particles move faster (vibrate, rotate, or translate), the temperature is higher. When they move slower, the temperature is lower.

2. **Thermal Equilibrium:**  
   Temperature is the property that determines the direction of heat transfer. Heat flows naturally from an object with a higher temperature to one with a lower temperature until both reach the same temperature (thermal equilibrium).

3. **Measurable Quantity:**  
   Temperature is a quantitative property that can be measured using thermometers. It’s expressed in units like degrees Celsius (°C), Fahrenheit (°F), or Kelvin (K).

4. **Thermodynamic Definition:**  
   In thermodynamics, temperature is related to the change in internal energy with respect to entropy. It is a fundamental variable that helps describe the state of a system.

In short, temperature is essentially a measure of the average energy of motion of particles in matter, and it governs how heat energy moves between objects.
User: mathematical relationship?
Assistant:  CertainlyCertainly! The mathematical relationship involving temperature depends on the context. Here are some key formulations that relate temperature to physical quantities:

---

### 1. **Temperature and Average Kinetic Energy (Ideal Gas Approximation)**

For an ideal gas, the average kinetic energy of a single particle is proportional to the absolute temperature \( T \):

\[
\langle E_{\text{kin}} \rangle = \frac{3}{2} k_B T
\]

- \( \langle E_{\text{kin}} \rangle \) = average kinetic energy per particle  
- \( k_B \) = Boltzmann constant \(\approx 1.38 \times 10^{-23} \, \text{J/K}\)  
- \( T \) = temperature in Kelvin (K)  

This formula shows temperature as proportional to the average kinetic energy of particles.

---

### 2. **Thermodynamic Definition**

From the laws of thermodynamics:

\[
\frac{1}{T} = \left(\frac{\partial S}{\partial U}\right)_V
\]

- \( T \) = temperature  
- \( S \) = entropy  
- \( U \) = internal energy  
- The partial derivative is taken at constant volume \( V \)

This means temperature is the inverse of the rate of change of entropy with respect to internal energy.

---

### 3. **Ideal Gas Law**

For an ideal gas:

\[
PV = nRT
\]

- \( P \) = pressure  
- \( V \) = volume  
- \( n \) = number of moles  
- \( R \) = universal gas constant (\(8.314\, \text{J/(mol·K)}\))  
- \( T \) = temperature in Kelvin  

This law connects temperature with measurable macroscopic properties.

---

### Summary —

- At a microscopic level:  
  \[
  \text{Temperature} \propto \text{Average kinetic energy of particles}
  \]

- At a thermodynamic level:  
  \[
  \frac{1}{T} = \left(\frac{\partial S}{\partial U}\right)_V
  \]

- At macroscopic level for gases:  
  \[
  PV = nRT
  \]

If you want, I can expand on any of these relationships!
User: how can it be related to 1/2mv^2
Assistant:  GreatGreat question! The expression \( \frac{1}{2} m v^2 \) is the classical formula for the kinetic energy of a single particle of mass \( m \) moving at speed \( v \). Temperature is directly related to the **average kinetic energy** of the particles in a substance.

### How \( \frac{1}{2} m v^2 \) relates to temperature:

For an ideal gas, the particles move in random directions with a distribution of speeds. The **average kinetic energy per particle** is related to temperature by:

\[
\langle E_{\text{kin}} \rangle = \frac{1}{2} m \langle v^2 \rangle = \frac{3}{2} k_B T
\]

Where:

- \( \langle E_{\text{kin}} \rangle \) = average kinetic energy per particle  
- \( m \) = mass of a single particle  
- \( \langle v^2 \rangle \) = mean squared speed of particles (average of the square of the velocity magnitude)  
- \( k_B \) = Boltzmann constant (~\(1.38 \times 10^{-23} \, \mathrm{J/K}\))  
- \( T \) = absolute temperature in kelvin (K)

### Breaking it down:

- The kinetic energy of one particle at speed \( v \) is \( \frac{1}{2} m v^2 \).
- Because particles have different velocities, we use the average over all particles: \( \frac{1}{2} m \langle v^2 \rangle \).
- This average kinetic energy is proportional to the temperature; the proportionality constant involves \( \frac{3}{2} k_B \) (the factor 3 comes from three degrees of freedom: motion in x, y, and z directions).

### So, in short:

\[
\boxed{
\frac{1}{2} m \langle v^2 \rangle = \frac{3}{2} k_B T
}
\]

This equation tells us that temperature \( T \) is proportional to how "fast," on average, the particles are moving inside the material. Higher temperature means particles have higher average speeds and thus greater average kinetic energy.

---

If you're interested, I can also explain how this extends to rotational and vibrational motion, or how this links to real gases and solids!
User: so is that the boltzman equation
Assistant:  NotNot exactly — the equation

\[
\frac{1}{2} m \langle v^2 \rangle = \frac{3}{2} k_B T
\]

is a specific result from the **kinetic theory of gases**, sometimes called the **equipartition theorem** for translational motion of ideal gas particles, rather than “the Boltzmann equation.”

### What is the Boltzmann equation?

The **Boltzmann equation** is a fundamental equation in statistical mechanics that describes how the distribution function \( f(\mathbf{r}, \mathbf{v}, t) \) of particles in phase space (position \(\mathbf{r}\), velocity \(\mathbf{v}\), time \(t\)) changes due to:

- Particle motion (transport),
- External forces,
- And collisions between particles.

It looks like:

\[
\frac{\partial f}{\partial t} + \mathbf{v} \cdot \nabla_{\mathbf{r}} f + \frac{\mathbf{F}}{m} \cdot \nabla_{\mathbf{v}} f = \left( \frac{\partial f}{\partial t} \right)_{\text{collisions}}
\]

It is much more complex and deals with the full dynamics of particle distributions.

---

### Summary:

- The formula

  \[
  \frac{1}{2} m \langle v^2 \rangle = \frac{3}{2} k_B T
  \]

  describes the average kinetic energy of particles at temperature \( T \) (from the kinetic theory of gases and equipartition theorem).

- The **Boltzmann equation** describes the time evolution of the particle distribution function in phase space — a statistical description of many-particle systems.

---

If you want, I can explain more about the Boltzmann equation, or about how the kinetic theory relates temperature to energy!
User: how is hexagonal phase related to micellar phase
Assistant: