Explain why increasing the temperature of a gas increases the pressure if 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, leading to an increase in pressure.

Graph lens: Read the trend, flat section, gradient, or axis labels before explaining the physical meaning. This question asks: Explain why increasing the temperature of a gas increases the pressure if 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, leading to an increase in pressure., because gas pressure comes from particle collisions with container walls. In Particle motion in gases, the marking point should connect directly to explain that gas particles collide with each other and with the walls of their container. 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 459 is distinct because it uses this exact question context and the graph lens rather than a generic particle-model sentence.