Chemistry – States of matter - Solids, liquids and gases | e-Consult

When the temperature of a gas increases, the average kinetic energy of the gas particles also increases. Kinetic energy is directly proportional to temperature. This means the particles move faster and, consequently, possess more kinetic energy.

According to kinetic theory, gas particles are assumed to be in constant random motion and occupy a volume. As the particles move faster, they collide with the walls of the container more frequently and with greater force. This increased frequency and force of collisions effectively push the walls of the container outwards.

Therefore, the gas expands to occupy a larger volume to accommodate the faster-moving particles. This expansion is a direct consequence of the increased kinetic energy causing the particles to exert greater pressure on the container walls, leading to a greater overall volume. The volume increase is proportional to the increase in temperature, assuming pressure remains constant.