The Effect Of Changing Conditions On Equilibrium (ht Only) (GCSE Chemistry)

Which is true about Le Chatelier’s principle?

Which description correctly distinguishes rate and extent of reaction?

Which change will increase the extent of a reaction that is endothermic in the forward direction?

Which change is most effective to increase the yield of a gaseous product that is formed by a reaction producing fewer gas moles than it consumes?

Consider the equilibrium N2(g) + O2(g) ? 2NO(g) which is endothermic in forward direction. What happens to the position of equilibrium and the value of K if temperature is decreased?

Which change will both increase the rate and increase the extent (yield) of an endothermic forward reaction?

In an industrial reversible reaction carried out at temperature T, adding a catalyst will:

For the exothermic equilibrium A(g) ? B(g) + heat, which change increases the equilibrium constant K at the new temperature?

In a gaseous equilibrium with more moles of gas on the left, increasing pressure will:

Consider 2NO2(g) ? N2O4(g) (exothermic forward). What happens to the colour and position of equilibrium when pressure is increased?

For the gas equilibrium CO(g) + 2H2(g) ? CH3OH(g), what is the effect of increasing total pressure (by decreasing volume) on the position of equilibrium?