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## Particles in a ideal gas:

- Have no volume
- Have elastic collisions
- Are in constant, random, straight-line motion
- Don’t attract or repel each other
- Have an average KE directly related to kelvin temperature

## Particles in a real gas

- Have their own volume
- Attract each other

## Gas behaviour is most ideal:

- At low pressures
- At high temperatures
- In nonpolar atoms/molecules

## Gas Laws

### Boyle's law

The pressure & volume of a gas are inversely proportional to each other when temperature & mass remain constant

\begin{equation}x_{n+1} + x_{n+2}\end{equation}

### Avagadro's law

Equal volume of any gas at same temperature & pressure will have the same number of molecules

\begin{equation}\frac{V_1}{n_1}=\frac{V_2}{n_2}\end{equation}

### Charles's law

The volume & absolute temperature of a gas are directly proportional at constant mass & pressure

\begin{equation}\frac{V_1}{T_1}=\frac{V_2}{T_2}\end{equation}

### Gay-Lussac's law

Pressure is proportional to absolute temperature with constant mass and volume \begin{equation}P \propto T\end{equation}