• Gases?in a container exert a?pressure?as the gas molecule are constantly?colliding?with the wall of the container

Gas particles exert a pressure by constantly colliding with the walls of the container

Changing gas volume

• Decreasing?the?volume?(at constant temperature) of the container causes the molecules to be?squashed?together which results in more?frequent?collisions with the container wall
• The?pressure?of the gas?increases
• The?volume?is therefore?inversely proportional?to the?pressure?(at constant temperature)
  • A graph of?volume?of gas plotted against 1/pressure gives a straight line

Decreasing the volume of a gas causes an increased collision frequency of the gas particles with the container wall (a); volume is inversely proportional to the pressure (b)

Changing gas temperature

• Increasing?the?temperature?(at constant volume) of the gas causes the molecules to gain more?kinetic energy
• This means that the particles will move?faster?and?collide?with the container walls more?frequently
• The?pressure?of the gas?increases
• The?temperature?is therefore?directly proportional?to the?pressure?(at constant volume)
  • A graph of?temperature?of gas plotted against?pressure?gives a straight line

Increasing the temperature of a gas causes an increased collision frequency of the gas particles with the container wall (a); temperature is directly proportional to the pressure (b)