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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_C = -K_P/(RT).

K_P = (RT)K_C.

K_P = K_C.

K_C = (RT)K_P.

Nitrogen and hydrogen are mixed in a molar ratio of 1:3 in the Haber process for the production of ammonia. The equilibrium is attained at 6000C and 10atm. Given that the percentage of ammonia in the mixture of gases at equilibrium is 15%, the value of K_p is:

1.4 x 10⁻³ atm⁻².

4.09 x 10⁻¹ atm⁻².

4.09 x 10⁻¹ atm².

1.4 x 10⁻³ atm².

The equilibrium attained by a chemical reaction is described as a dynamic equilibrium because at equilibrium

The forward and the backward reactions continue to take place but at the same rate, hence there is no net change in the concentrations of reactants and products

The forward and the backward reactions continue to take place but at different rates, hence there is no net change in the concentrations of reactants and products

The forward and the backward reactions continue to take place but at the same rate, hence there is no net change in the concentrations of reactants only

The forward and the backward reactions continue to take place but at the same rate, hence there is a net change in the concentrations of reactants and products

Consider the following systems in equilibrium:
N_{2 (g)} + 3H_{2 (g)} ⇌ 2NH_{3 (g)}

All are correct

4 moles of gas molecules on the LHS and 2 moles on the RHS

If pressure is reduced, the equilibrium will shift to the left to produce more gas molecules thereby increasing the pressure of the system in accordance with Le Chatelier’s principle

If pressure is increased, the equilibrium position will shift to the right to produce fewer gas molecules thereby reducing the pressure of the system according to Le Chatelier’s principle

At equilibrium:

The limiting reagent has been consumed.

The rate constants of the forward and reverse reactions are equal.

All chemical reactions have ceased.

The rates of the forward and reverse reactions are equal.