𝑁2 (𝑔) + 3𝐻2 (𝑔) ⇌ 2𝑁𝐻3 (𝑔), is exothermic in the forward direction. At higher temperatures

𝑁2 (𝑔) + 3𝐻2 (𝑔) ⇌ 2𝑁𝐻3 (𝑔), is exothermic in the forward direction. At higher temperatures (assuming the same total pressure), the yield of NH3(g) produced from a given N2 and H2 gas mixture should be

A) Larger

B) The Same

C) Smaller

D) Not enough information is given

Explanation: The question states that the reaction is exothermic, which means heat is being released. Therefore we can put heat on the product side: 𝑁2 (𝑔) + 3𝐻2 (𝑔) ⇌ 2𝑁𝐻3 (𝑔) + heat

At higher temperatures, heat would increase. The equilibrium will shift to lower the heat, to the opposite side of where the heat is located. Therefore, equilibrium would should to the left, decreasing the yield of NH3

Answer: C