Question

Consider the exothermic reaction shown. To increase the amount of NH3, which of these tactics might not work, if the reaction is at equilibrium: N2(g) + 3H2(g) ⇌ 2NH3(g) Group of answer choices: A) Adding a catalyst derived from a transition metal. B) Removing NH3 as soon as it is formed. C) Adding more N2(g). D) Lowering the reaction temperature.

Answer 1

Ans. (A) adding a catalyst will not work to increase the amount of ammonia.

Explanation:

(A) catalyst doesn't effect the equilibrium. Because in presence of catalyst, both forward and backward reaction rate speed up equally , thus moving the system towards equilibrium faster but catalyst has no effect on final equilibrium position.

(B) according to Le Chatelier principle, if we remove the product as soon as it's formed, then the reaction will go in forward direction to produce the products .

C) adding more N2 means we are adding the reactant, so the reaction will go in forward direction fastly to decrease the added reactants. Means it will increase the amount of ammonia.

D) exothermic reaction gives off the energy. Thus decrease in temperature will decrease the energy released and so the reaction will go in product forming direction. So formation of ammonia will increase.