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

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?

An inert gas is added at constant volume to a reacting gas mixture. Which of the following is correct immediately after addition?

If a gaseous reaction at equilibrium has ?n(g) = 0 (same number of moles on both sides), what is the effect of changing pressure?

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

If the total pressure of a reaction mixture is increased by adding more of a gaseous reactant (not an inert gas), what is the immediate effect on the equilibrium?

For 2NO2(g) ? N2O4(g) the equilibrium at constant temperature is a brown ? colourless system. What happens to the colour if pressure is increased by compression?

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

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

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

For the reaction 2H2(g) + O2(g) ? 2H2O(g) at a temperature where Kp is fixed, what is the effect of increasing pressure by compressing the mixture?

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