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

Adding extra gaseous product to an equilibrium mixture (without changing volume) will have which effect?

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?

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

If the pressure of a system at equilibrium is increased and the position shifts so that more product forms, what happens to the rate at which the new equilibrium is established compared to before the pressure change?

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

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

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 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?

For the equilibrium 2NO2(g) ? N2O4(g) at a given temperature, the equilibrium constant Kp is 0.50. If initially only NO2 is present at total pressure 1.00 atm, which expression gives p(N2O4) at equilibrium (letting y = p(N2O4))?

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?

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