The Gas Laws

The Kinetic Theory of gases assumes five things: Gas particles do not repel or attract each other, they are smaller than the distances between them, they are in constant, random motion, no kinetic energy is lost when gas particles collide, and all gases have the same average kinetic energy in a given temperature. Actual gases do not obey all of these assumptions, but their behavior does approximate them. The assumptions themselves are based on the temperature, volume and pressure of the gas sample. The interdependence of these three variables is the basis for the following gas laws. Boyle's Law relates pressure and volume, keeping temperature constant: P1V1=P2V2. Charles' Law relates volume and temperature, keeping the pressure constant: V1/T1 = V2/T2. Gay-Lussac's Law relates pressure and temperature, keeping volume constant: P1/T1=P2/T2. This quiz will cover basic gas law problems. You will need a calculator. Select the best answer from the choices.