Use the kinetic theory of gases to explain why the pressure inside a container increases when the temperature of the air inside it rises. Assume that the volume of the container remains constant.

The kinetic theory of gases states that a gas consists of many molecules in constant motion. A rise in temperature increases the mean speed of these molecules, and therefore their momentum (=mv).

The increased momentum of these molecules results in more frequent and more forceful collisions with the walls of the container. Pressure is defined as force/area. As we are told that the volume, and therefore the area of the walls of the container remain the same, the increased force of the colliding gas molecules must result in an increased pressure within the container.

ET
Answered by Epen T. Physics tutor

7182 Views

See similar Physics A Level tutors

Related Physics A Level answers

All answers ▸

A stone is thrown horizontally at 5m/s from a platform 10m above ground. Find time till impact with ground.


One of the decays of potassium (A=40, Z=19) results in an excited argon atom with excess energy of 1.50 Mev. In order to be stable, it emits a gamma photon. What frequency and wavelength has this gamma photon?


Is F=ma Newton's 2nd Laws of Motion?


Calculate the threshold frequency for a metal with a work function of 3eV


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