Particle Motion In Gases (GCSE Physics)

Why does a pressure cooker cook food faster than an open pot at the same heat source?

When comparing two samples of the same gas, one at 300 K and one at 600 K, both at equal pressure, how do their average kinetic energies compare?

If two gases at the same temperature have different molecular masses, how do their root mean square speeds compare?

When a gas is compressed quickly, the temperature rises. What happens to the mean kinetic energy of the particles during this process?

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

If a sealed container contains gas at 20 °C and then gas is allowed to escape slowly until pressure halves while temperature constant, what happens to number of particles inside?

Why does a rising balloon balloon`s internal gas particles not instantly escape even though collisions happen at the surface?

What happens to the frequency of particle collisions with the walls when the density of a gas in a sealed container is increased?

Which quantity increases when the temperature of a fixed mass of gas increases at constant volume?

How does adding an inert gas (that does not react) to a container at constant volume affect the partial pressure of the original gas?

What is the main reason gas diffusion is faster in helium than in air at the same temperature?