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

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?

Which experimental action would change the rate but not the equilibrium position for a closed heterogeneous system?

Which change would decrease the yield of product for an exothermic forward reaction at equilibrium?

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

A sealed container holds the equilibrium 2 A(g) ? B(g) + C(g). Initially brown B is present with colourless A and C. If B is removed continuously, what happens?

Which effect does doubling the concentration of a reactant have immediately on the rates at equilibrium?

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?

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

Which description correctly distinguishes rate and extent of reaction?

In the Haber process, removing liquid ammonia as it is formed has what effect on the gas-phase equilibrium?

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