Increasing The Pressure Of A Gas (physics Only) (ht Only) (GCSE Physics)

A syringe containing air is compressed slowly keeping temperature constant. According to the particle model, why does the measured pressure increase?

For a fixed mass of gas in a sealed container, which two independent changes would both increase the internal pressure?

Which expression (ideal-gas form) correctly links pressure P, volume V, number of moles n and absolute temperature T?

A fixed mass of gas is heated in a constant-volume steel container that can safely hold pressure up to 5.0 × 10^6 Pa. Initial pressure 1.0 × 10^5 Pa, initial temperature 290 K. Using ideal gas law, what maximum temperature T_max (in K) would cause pressure to reach 5.0 × 10^6 Pa (approximate)?

A sealed syringe initially at room temperature contains gas at pressure P0. The syringe is plunged quickly to half its initial volume so the process is near-adiabatic. If the mean kinetic energy per particle increases due to compression, which of these increases?

Which microscopic change best explains why adding more gas molecules (same T, same volume) increases pressure?

In the particle model, why does reducing the volume of a gas (with the same number of particles and same temperature) increase its pressure?

A sample of gas obeys PV = nRT. If you double n and double V while holding T constant, what happens to pressure P?

A sealed rigid container holds a fixed mass of an ideal gas. Which single change will increase the gas pressure inside the container?

A piston contains gas at 100 kPa and 300 K. If the number of gas moles is doubled rapidly while keeping volume constant and no heat exchange, which immediate effect will be observed?

Which statement describes why rapid compression (faster than thermal losses) produces a higher peak pressure than slow compression to the same final volume?