The Effect Of Pressure Changes On Equilibrium (ht Only) (GCSE Chemistry)

In the industrial Haber process for ammonia production, why is a high pressure used?

In a heterogeneous equilibrium involving a solid and a gas, e.g. CaCO3(s) ? CaO(s) + CO2(g), how does increasing the external pressure affect the equilibrium?

For PCl5(g) ? PCl3(g) + Cl2(g), increasing pressure has which effect on the equilibrium position?

For the reaction H2(g) + Cl2(g) ? 2HCl(g) (?n = 0), what is the effect of changing the total pressure?

For a gas equilibrium involving solids, why are solids not included in the Kp expression?

For N2(g) + 3H2(g) ? 2NH3(g), an inert gas is added at constant pressure (so the volume increases). What is the expected shift of equilibrium?

Which statement about adding an inert gas at constant pressure (by increasing volume) is correct for a gas-phase equilibrium?

If the volume of a container is halved at constant temperature for a mixture at equilibrium, this is equivalent to which immediate effect on the gases?

For a reaction 2A(g) ? 3B(g), what is the effect of increasing pressure by compressing the gas mixture?

In which industrial situation is raising pressure used despite higher cost because it increases yield of a gaseous product?

Does changing the pressure of a gas-phase equilibrium change the equilibrium constant Kp (at fixed temperature)?