Question

The following endothermic reaction is at equilibrium: 2NOBr(g) <----> 2NO(g) + Br2(g) Predict the effect of each of the following changes on the position of equilibrium. Explain your answer.

A) adding more Br₂(g)
B) removing NOBr(g)
C) decreasing the temperature

Answer 1

Adding more Br₂(g) and removing NOBr(g) will shift the equilibrium to the right, producing more NO(g) and Br2(g). Decreasing the temperature will shift the equilibrium to the left, favoring the formation of more NOBr(g).

Step-by-step explanation:

The addition of more Br₂(g) will shift the equilibrium to the right, favoring the formation of more NO(g) and Br2(g).

This is because the increase in the concentration of Br₂(g) will cause the reaction to consume more of it to restore equilibrium.

Removing NOBr(g) from the equilibrium will also shift the equilibrium to the right.

Since NOBr(g) is a reactant, its removal will cause the reaction to produce more NO(g) and Br2(g) to compensate.

Decreasing the temperature will favor the exothermic direction of the reaction, shifting the equilibrium to the left.

This means that more NOBr(g) will be formed and less NO(g) and Br2(g) will be produced.