A rigid, sealed container holds a fixed mass of an ideal gas. When the temperature of the gas is increased, the pressure exerted by the gas on the walls of the container increases.
Which statement correctly explains this increase in pressure on a molecular level?
The average kinetic energy of the gas molecules increases, so they collide with the walls of the container more frequently and experience a greater change in momentum per collision.
The intermolecular forces of attraction between the gas molecules and the container walls increase.
The volume of individual gas molecules increases as they absorb heat, which forces them against the container walls.
The molecules lose more kinetic energy when they collide with the walls, transferring it to the container.
321 exam-style questions on CIE IGCSE Physics 2.1 Kinetic particle model of matter, covering 2.1.1 States of matter and changes of state, 2.1.2a Particle structure and motion in solids, liquids and gases, 2.1.2b Gas pressure and particle collisions, 2.1.2c Brownian motion, 2.1.3a The absolute scale of temperature, and 2.1.3b Pressure, volume and temperature of a gas. Each one has a worked solution and a mark scheme showing where the marks go.