Question

(Multiple choice) Consider the reaction at equilibrium. Which way would the equilibrium shift if the temperature were increased?

Answer 1

Step-by-step explanation:

We are given the following reaction at equilibrium:

2 A (g) + B (g) <---> C (g) + D (g) ΔH = -52 kJ/mol

Since the ΔH is negative we know that this reaction is exothermic, it is releasing heat. Since we are producing heat we can consider it a product.

2 A (g) + B (g) <---> C (g) + D (g) + HEAT

If we increase the temperature, the reaction will try to lower it. It will shift to the left to remove some heat and come back to the equilibrium.

Answer: Left