Question

At a higher temperature, K = 1.8 × 105. Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will

Answer 1

The question is incomplete, the complete question is;

1. Given: 2A(g) <-> 2B(g) + C(g). At a particular temperature, K = 1.6x104.

At a higher temperature, K = 1.8x10-5. Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will...

cause [A] to increase

cause [B] to increase

gave no effect

cannot be determined

Answer:

cause [B] to increase

Explanation:

We have to have it behind our minds that;  for an exothermic reaction, when the temperature is increased, the value of the equilibrium constant decreases. On the other hand, for an endothermic reaction, increasing the temperature increases the value of the equilibrium constant.

In this particular case, increasing the temperature decreased the equilibrium constant from K = 1.6x104 to K = 1.8x10-5 meaning that the equilibrium constant decreased with increase in temperature. This means that the reaction is exothermic and a decrease in temperature will favour the forward reaction hence more B is produced.