Question

ive #4 - chemical systems and equilibrium (part 1)
question 5 (1 point)
which change to the equilibrium system below will maximize the formation of ammonia, given it is an exothermic reaction?
n₂ + 3h₂ ⇌ 2nh₃
adding a catalyst
decreasing the temperature
increasing n₂ amount
decreasing pressure

Explanation:

To determine the change that maximizes $\ce{NH_{3}}$ formation in the exothermic equilibrium $\ce{N_{2} + 3H_{2}
ightleftharpoons 2NH_{3}}$:

• Adding a catalyst: Only speeds up equilibrium attainment, no effect on equilibrium position or $\ce{NH_{3}}$ yield.
• Decreasing temperature: For exothermic reactions (heat is a product), lowering temperature shifts equilibrium to the right (favors product formation) to release heat, increasing $\ce{NH_{3}}$.
• Increasing $\ce{N_{2}}$ amount: Shifts equilibrium right, but the question asks for the change that maximizes formation. While this helps, temperature change (for exothermic) has a more direct impact on equilibrium position for yield in such reactions (Le Chatelier’s principle: exothermic → lower temp favors products).
• Decreasing pressure: The reaction has 4 moles of gas on the left (1 $\ce{N_{2}}$ + 3 $\ce{H_{2}}$) and 2 moles on the right ($\ce{2NH_{3}}$). Lowering pressure shifts equilibrium to the side with more moles of gas (left), decreasing $\ce{NH_{3}}$.

Answer:

B. decreasing the temperature (assuming options are labeled as A. adding a catalyst, B. decreasing the temperature, C. increasing $\ce{N_{2}}$ amount, D. decreasing pressure)