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

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

A gaseous equilibrium 2A(g) ? B(g) is at equilibrium. If the volume of the container is instantaneously halved (pressure doubles), which direction does the equilibrium shift?

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

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?

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

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?

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

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?