Question

Which of the following options will cause the equilibrium of the system below to shift?

NH4SHs)NH3(g)+H2S(g)
A) Increasing the volume of the container
B)Decreasing the temperature of the system
C) Adding NH3(g) Adding a catalyst
D) None of these

Answer 1

The equilibrium of the system NH4SH(s) ⇌ NH3(g) + H2S(g) will shift if the volume of the container is increased, which lowers pressure and favors the products. Adding NH3(g) will shift the equilibrium to the left. Adding a catalyst does not affect the position of equilibrium. Therefore, the correct answer is A) Increasing the volume of the container.

Step-by-step explanation:

The question relates to how changes in conditions will affect the equilibrium of the reaction NH4SH(s) ⇌ NH3(g) + H2S(g).

Increase in the volume of the container would cause a decrease in pressure and shift the equilibrium towards the side with more moles of gas, according to Le Chatelier’s principle. In this case, since NH3 and H2S are both gases and produced on the product side, increasing volume would shift the equilibrium to the right, favoring the production of NH3 and H2S.

Decreasing the temperature of the system will shift the equilibrium based on the exothermic or endothermic nature of the reaction, which isn't specified in the question. If the decomposition of NH4SH is exothermic, the equilibrium would shift towards the reactants. Otherwise, it would shift towards the products.

Adding NH3(g) to a system at equilibrium would lead to an increased concentration of one of the products, which would shift the equilibrium to the left to re-establish equilibrium according to Le Chatelier's principle.

Adding a catalyst will not shift the equilibrium, as it only speeds up the rate at which equilibrium is reached without affecting the position of equilibrium.