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5/58 MCQs for:

Chemical Equilibrium

The following equilibrium is exothermic for the left to right reaction:

2SO_2(g) + O_2(g) ⇌ 2SO_3(g).

K_P = K_C.

K_C = (RT)K_P.

K_C = -K_P/(RT).

K_P = (RT)K_C.

Which one of the following will change the value of an equilibrium constant?

Varying the initial concentrations of products

Changing temperature

Adding other substances that do not react with any of the species involved in the equilibrium

Varying the initial concentrations of reactants

Consider the following reaction system in equilibrium.

2SO_2(g) + O_2(g) ⇌ 2SO_3(g) ΔH = -197 KJ/mol

The forward reaction is ... while the backward reaction is:

Exothermic, exothermic.

Endothermic, endothermic.

Endothermic, exothermic.

Exothermic, endothermic.

Consider the following reaction system in equilibrium.
2SO_2(g) + O_2(g) ⇌ 2SO_3(g) ΔH = -197 KJmol⁻¹

The equilibrium position will shift to the right and then to the left i.e. the exothermic reaction will be favoured so as to replenish the heat removed from the system

The equilibrium position will shift to the right i.e. the exothermic reaction will be favoured so as to replenish the heat removed from the system

The equilibrium position will shift to the left i.e. the exothermic reaction will be favoured so as to replenish the heat removed from the system

The equilibrium position will shift to the left favouring the endothermic reaction so that the extra heat added is used up

How is the reaction quotient used to determine whether a system is at equilibrium?

At equilibrium, the reaction quotient is undefined.

The reaction is at equilibrium when Q = K_eq.

The reaction is at equilibrium when Q < Keq.

The reaction is at equilibrium when Q > K_eq.