Gas Laws Review

Boyle's Law

• Relates volume and pressure (constant temperature and number of particles).

• Decreasing volume increases collisions -> increases pressure (inverse relationship).

• Equation: $P<em>1 V</em>1 = P<em>2 V</em>2$.

• Graph of pressure vs. volume: curved line (inverse relationship).

Pressure Law

• Relates temperature and pressure (constant volume and number of particles).

• Increasing temperature increases kinetic energy -> more frequent and forceful collisions -> increases pressure (direct relationship).

• Equation: $\frac{P<em>1}{T</em>1} = \frac{P<em>2}{T</em>2}$ (use Kelvin for temperature).

• Graph of pressure vs. temperature: straight line (direct relationship); x-intercept at -273°C (absolute zero).

Charles' Law

• Relates temperature and volume (constant pressure and number of particles).

• Increasing temperature causes kinetic energy to rise -> volume increases (direct relationship).

• Equation: $\frac{V<em>1}{T</em>1} = \frac{V<em>2}{T</em>2}$ (use Kelvin for temperature).

• Graph of volume vs. temperature: straight line; x-intercept at -273°C (gas condenses).

Combined Gas Law

• Combines relationships from Boyle's, Pressure and Charles' laws: $\frac{P<em>1 V</em>1}{T<em>1} = \frac{P</em>2 V<em>2}{T</em>2}$.

• Allows ignoring one variable when it remains constant while solving gas law problems.