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

For the gas-phase equilibrium N2(g) + 3H2(g) ? 2NH3(g), what is the effect of increasing the total pressure (by compressing the container) at constant temperature?

Which of the following is true about changing pressure and the numerical value of Kp at constant temperature?

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?

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

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?

For the equilibrium 2SO2(g) + O2(g) ? 2SO3(g), what is the effect of increasing pressure?

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

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

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

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?