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

Which statement about Le Chatelier’s principle and temperature is correct?

Which of the following is a correct industrial strategy when an equilibrium reaction is exothermic and the desired product has fewer gas moles than the reactants?

When a reaction is exothermic in the forward direction, which of these changes will increase K (equilibrium constant) for the forward reaction?

A reaction profile shows products at higher energy than reactants. If the system is at equilibrium and temperature is increased, Le Chatelier’s principle predicts:

When the temperature is increased for a reversible reaction that is exothermic in the forward direction, the equilibrium position will shift to:

For the heterogeneous equilibrium CaCO3(s) ? CaO(s) + CO2(g), increasing temperature will:

A system at equilibrium is exothermic in the forward direction. Which change would increase the equilibrium yield of products?

When designing an experiment to measure the effect of temperature on equilibrium position, which control is most essential?

For the reversible reaction A(g) ? B(g), ?H° forward = -120 kJ. If the temperature is reduced, the equilibrium constant K will:

For the equilibrium 2A(g) ? B(g) + C(g) with ?H° forward = +60 kJ (endothermic), increasing temperature will:

An endothermic forward reaction has activation energy Ea,f and reverse Ea,r. Adding heat (raising temperature) generally: