Explain how increasing the temperature of a gas affects its pressure when the volume is kept constant.

Increasing the temperature of a gas increases the average kinetic energy of its particles, causing them to move faster. As a result, the particles collide with the walls of the container more frequently and with greater force, which increases the pressure.

Boundary lens: Keep this separate from nearby specification points that use similar words but test a different idea. This question asks: Explain how increasing the temperature of a gas affects its pressure when the volume is kept constant. The correct response is Increasing the temperature of a gas increases the average kinetic energy of its particles, causing them to move faster. As a result, the particles collide with the walls of the container more frequently and with greater force, which increases the pressure., because density links mass and volume, so the answer must preserve which quantity is being calculated. In Pressure in gases (physics only), the marking point should connect directly to (Physics only) Interpret pressure-volume data for a fixed mass of gas at constant temperature. If the question includes values, the working must keep the appropriate unit and operation; if it is an explanation, it must name the relevant particle behaviour or energy change. This item belongs to Particle model and pressure, so avoid answers that switch to a different quantity, confuse heat with temperature, or describe gas pressure without collisions when collisions are the reason. Checkpoint 574 is distinct because it uses this exact question context and the boundary lens rather than a generic particle-model sentence.