N2(g) + 3H2(g) ⇌ 2NH3(g) + energy : which direction does the reaction proceed if heat is addedA ReverseB ForwardC towards the products

Break Down the Problem

1. Identify the reaction and the conditions provided (addition of heat).
2. Analyze the effect of heat on the equilibrium of the reaction according to Le Chatelier's principle.

Relevant Concepts

1. Le Chatelier's Principle states that if an external change is applied to a system at equilibrium, the system will adjust to counteract that change and re-establish equilibrium.
2. In the reaction: $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \text{energy}$ Energy is on the product side, indicating that the reaction releases heat.

Analysis and Detail

1. Adding heat to the system is analogous to adding a product (in this case, energy).
2. According to Le Chatelier's Principle, the equilibrium will shift to the left (the reverse direction) to consume the extra "product" (heat).

Verify and Summarize

• When heat is added, the equilibrium shifts to the left, favoring the reactants to decrease the concentration of the added heat. Hence, the reaction moves in the reverse direction.

Final Answer

The reaction proceeds in the Reverse direction. (Option A)