Particle Motion In Gases (GCSE Physics)

At constant temperature, what happens to the pressure of a fixed mass of gas if the volume is halved?

A sealed syringe contains trapped air. The plunger is pushed slowly reducing volume; temperature is kept constant. What happens to the spacing between particles and the frequency of collisions?

If the temperature of a gas is increased while the container is allowed to expand so pressure stays constant, what happens to the average speed of the gas particles?

At constant pressure, which direct relationship describes how gas volume changes with temperature (in kelvin) for an ideal gas?

Which change will NOT increase gas pressure in a fixed container?

A gas in a container is warmed quickly (adiabatically to a good approximation). Which happens to internal energy and to average particle kinetic energy?

Which statement correctly links rms (root mean square) speed, temperature T (in kelvin), and particle mass m for an ideal gas (qualitative Year 10 form)?

Two containers contain the same gas. Container A has particles moving faster on average than Container B. Which is definitely true?

Which option explains why gas viscosity increases with molecular size and density?

Which process best describes diffusion of a gas?

Which description matches the Maxwell–Boltzmann idea used in particle theory of gases at school level?