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

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

Write the expression for Kp for the reaction N2(g) + 3H2(g) ? 2NH3(g).

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

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 the equilibrium N2O4(g) ? 2NO2(g), at fixed temperature and initial total pressure P0, an additional amount of gas is added but it is chemically inert and the volume is held constant. What happens to the equilibrium?

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

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?

When the pressure of a gas-phase equilibrium is increased, what happens to the instantaneous rates of the forward and reverse reactions before a new equilibrium is reached?

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

Which of the following best describes what happens to a gas-phase equilibrium if the system is compressed (volume decreased) and the equilibrium then shifts to re-establish Kp?