Question

The following reversible reaction is at equilibrium. If the concentration of HCI is increased, how would

the system react?
NH4CI NH3 + HCI

A. Nothing would change.
B. The reaction would move to the right, producing more NH3.
C. The reaction would move to the left, producing more NH4CI.
D. There would only be HCI remaining.

Answer 1

C.) The reaction would move to the left, producing more NH₄CI.

Step-by-step explanation:

The chemical equation:

NH₄Cl ↔ NH₃ + HCl

If you were to increase the amount of HCl, the equilibrium would shift to the left. This is because the system is trying to go back to equilibrium. The equilibrium was disturbed when more product (HCl) was added. In order to restore equilibrium, you need to do the same thing that was done to the products to the reactants. In other words, since the products increased, the reactants need to increase.