Question

Heating ammonium hydrogen sulfide leads to decomposition.

NH₄HS(s) ---> NH₃(g) + H₂S(g) ΔH > 0
Predict the effect on the equilibrium of raising the temperature. Answer by choosing:

A.) shift to right
B.) shift to left
C.) no change
D.) cannot tell

Answer 1

Raising the temperature of the endothermic reaction involving ammonium hydrogen sulfide decomposition causes the equilibrium to shift to the right, increasing the formation of ammonia and hydrogen sulfide gases. So, the correct option is A.) shift to right.

Step-by-step explanation:

When considering the effect of temperature change on a chemical equilibrium, we rely on Le Chatelier's Principle. This principle states that if a change is applied to a system at equilibrium, the system will adjust to counteract this change. In the case of the decomposition of ammonium hydrogen sulfide (NH4HS), which is an endothermic reaction with ΔH > 0, raising the temperature supplies heat to the system.

According to Le Chatelier's Principle, if we view heat as a reactant, adding heat to an endothermic reaction would shift the equilibrium to the right to consume the added heat. This means we would see an increase in the products, ammonia (NH3) and hydrogen sulfide (H2S). Hence, upon raising the temperature, the equilibrium would shift to the right, favoring the formation of more NH3 and H2S. Based on the given data and the principles of equilibrium, the mention the correct option in the final part of this response is: A.) shift to right.