Why does increasing the temperature of a gas increase the pressure (when the volume is fixed)?

We can understand this using an idea called the Kinetic Model of Gases. Basically, let's assume that every molecule in the gas is a tiny, tiny snooker ball whizzing around the container. These 'snooker balls' can collide with one another and the walls of the container they are in.

Now, the speed of the gas molecules (snooker balls) depends on their kinetic energy. The more kinetic energy they have, the faster they are moving. And the faster they are moving the harder they must hit each other and the walls.

Increasing the temperature will mean that we supply more energy to the molecules of gas and therefore increase their kinetic energy and speed. They will collide off the walls of the container harder. This raises the pressure because the pressure on the walls is defined as the force exerted by the molecules on the container wall divided by area (the area bit isn't too important here). The pressure is getting bigger because the molecules are whacking the walls harder!

Answered by Andrew M. Physics tutor

18654 Views

See similar Physics GCSE tutors

Related Physics GCSE answers

All answers ▸

How Should I structure my experiment report?


What name is given to the phenomena which results in longer wavelengths of light being observed from distant galaxies and why does this occur?


Give an example of a transverse and longitudinal wave.


A 15kg cannonball and a 1kg football are dropped to the ground from a height of 10 metres. Calculate the speed of the cannonball and of the football just before they hit the ground (you may ignore air resistance).


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences