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#### Ideal Gases

A little intro with a bit of text

### 1. Pressure of a Gas

Consider an ideal gas particle. If it has mass and is travelling at speed v before it collides elastically with the side of a container then it will rebound with the same speed ‘v’ but in the opposite direction. Its momentum has changed and therefore it must have experienced a force.

### 2. Boyle's Law

Boyle’s law states that the pressure of an ideal gas is inversely proportional to its volume, provided that the mass of the gas and its temperature remain constant. Basically you squash a gas and its pressure rises.

### 3. Derivation of pV=nRT

By combining the relationships between pressure, volume and temperature we can see how pV/T is a constant: a constant that depends upon the number of moles of gas in the system.

### 4. Boltzmann's Constant

The Boltzmann constant relates the mean kinetic energy of the molecules in a gas to temperature of the gas – a useful link between the microscopic properties of individual particles to the macroscopic properties of the whole system.

### 5. Assumption for the Kinetic Theory of Ideal Gases

These are the assumptions for the Kinetic Theory of Gases.

### 6. Pressure and Temperature for an Ideal Gas

By measuring the pressure of a gas and varying the temperature you can plot this data and extrapolate the line backwards until you reach a point where the temperature is zero – an estimate of absolute zero!