Which of the following best describes the effect of increasing the temperature on the equilibrium constant, K, for an exothermic reaction?

A. K remains unchanged

B. K increases

C. K decreases

D. K becomes zero

In the context of Le Chatelier's principle, what is the response of a system at equilibrium when stress is applied?

A. The system shifts to increase the stress

B. The system shifts to decrease the stress

C. The system remains unchanged

D. The system reaches a new equilibrium immediately

Which of the following is true regarding the relationship between Gibbs free energy change (Delta G) and the equilibrium constant (K)?

A. Delta G is positive when K > 1

B. Delta G is negative when K < 1

C. Delta G is zero when K = 1

D. Delta G and K are not related

For a given reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium position?

A. It will shift to the right

B. It will shift to the left

C. It will remain unchanged

D. It will depend on the temperature

How does an increase in pressure affect the equilibrium position of a gaseous reaction that produces fewer moles of gas?

A. Shifts to the right

B. Shifts to the left

C. No effect

D. The direction of shift cannot be determined

a) Explain the principle of Le Chatelier's principle and how it can be used to predict the effect of changes on the equilibrium position of a reaction. [3]

b) A system at equilibrium is subjected to an increase in pressure. Describe how this change would affect the position of equilibrium for a reaction that produces fewer moles of gas. [2]

a) Describe the relationship between Gibbs free energy change (ΔG) and the equilibrium constant (K) for a reaction. [3]

b) If ΔG for a reaction is positive, what can be inferred about the spontaneity of the reaction and the value of K? [2]

a) The Haber process is an industrial method for producing ammonia. Describe how the principles of equilibrium are utilised in this process to maximise the yield of ammonia. [3]

b) In the context of the Haber process, explain the effect of increasing the temperature on the equilibrium position and the rate of reaction. [2]

a) Describe the effect of a catalyst on the rate of a reaction and its impact on the position of equilibrium. [2]

b) Consider a reaction that is endothermic in the forward direction. Predict the effect of decreasing the temperature on the equilibrium position. [2]

c) How does the value of the equilibrium constant, K, change for the above reaction when the temperature is decreased? [2]

a) Explain the relationship between stress and response in equilibrium systems using Le Chatelier's principle. [3]

b) If the concentration of products in a system at equilibrium is increased, predict the direction in which the system will shift. [1]

c) How would the addition of an inert gas at constant volume affect the position of equilibrium? [2]

Which of the following industrial processes utilises the principles of equilibrium to increase product yield?

A. Electrolysis of water

B. Haber process

C. Distillation of ethanol

D. Fermentation of glucose

For a reaction at equilibrium, if the temperature is decreased and the reaction is exothermic, what will happen to the equilibrium position?

A. It will shift to the right

B. It will shift to the left

C. It will remain unchanged

D. It will depend on the concentration of reactants

Which of the following best describes the effect of a catalyst on the equilibrium position of a reaction?

A. Shifts the equilibrium to the right

B. Shifts the equilibrium to the left

C. Does not affect the equilibrium position but increases the rate at which equilibrium is achieved

D. Prevents the reaction from reaching equilibrium

If the equilibrium constant (K) for a reaction is much greater than 1, which of the following is true?

A. The reaction is not favourable

B. The concentration of reactants at equilibrium is much higher than that of products

C. The concentration of products at equilibrium is much higher than that of reactants

D. The reaction does not reach equilibrium

In the context of the equilibrium law, what does a K value of less than 1 indicate about a reaction?

A. The reaction is endothermic

B. The reaction is exothermic

C. The reactants are favoured at equilibrium

D. The products are favoured at equilibrium

a) Describe the significance of the equilibrium constant, K, in determining the extent of a reaction. [3]

b) For a reaction with a K value much greater than 1, what can be inferred about the concentrations of reactants and products at equilibrium? [2]

c) How does the value of K relate to the spontaneity of a reaction? [2]

a) The Gibbs free energy change (ΔG) is a useful parameter in predicting the direction of spontaneous change. Explain the conditions under which a reaction is spontaneous based on ΔG. [3]

b) How is the temperature dependence of equilibrium constants related to the Gibbs free energy change? [2]

c) Given that a reaction has a positive ΔG at a certain temperature, what can be inferred about the value of K for that reaction at that temperature? [2]

a) Describe the principle of Le Chatelier's principle in the context of changes in concentration and its effect on the position of equilibrium. [3]

b) A reaction at equilibrium is exothermic in the forward direction. If the system is cooled, predict the effect on the equilibrium position. [2]

c) Based on your answer to part b, how would the concentration of the reactants change? [2]

d) In the context of the reaction mentioned in part b, if a catalyst is introduced, how would the time taken to reach equilibrium be affected? [2]

a) Explain the significance of the equilibrium constant, K, in relation to the concentrations of reactants and products at equilibrium. [3]

b) Given a reaction with a K value of 0.01 at a certain temperature, what can be inferred about the extent of the reaction? [2]

c) How does the Gibbs free energy change (ΔG) relate to the value of K? [3]

d) For the reaction mentioned in part b, if the temperature is increased, predict the effect on the value of K, assuming the reaction is endothermic. [2]

a) Describe the effect of pressure changes on the position of equilibrium for gaseous reactions. [3]

b) Consider a gaseous reaction where the number of moles of reactants is greater than the number of moles of products. Predict the effect of increasing the pressure on the equilibrium position. [2]

c) How would the addition of an inert gas at constant pressure affect the position of equilibrium for the reaction mentioned in part b? [2]

d) In industrial processes, why might a compromise pressure be used instead of the highest possible pressure to maximise product yield? [3]