Pressure

Look at the animation on the left. Notice how the rate of collisions changes as we alter the temperature, volume and number of particles.

Increasing the temperature increases the average kinetic energy of the molecules. With a higher speed they reach the other side of the container in less time which increases the frequency of collisions.

Increasing the number of particles will obviously increase the rate at which collisions occur as there is now a greater number of molecules capable of colliding with the walls of the container.

Reducing the volume decreases the distance molecules have to travel before colliding with the wall.

 

Looking at the animation above, for a fixed amount of gas, think of how:
- a decrease in pressure, without changing the temperature, is to be achieved.
Solution
- an increase in pressure, without changing the temperature, is to be achieved.
Solution
- the temperature of the gas can be increased without changing the pressure.
Clue
- the temperature of the gas can be decreased without changing the pressure.
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