QuestionJune 10, 2025

Given the Haber reaction at equilibrium: N_(2)(g)+3H_(2)(g)leftharpoons 2NH_(3)(g)+heat Which stress on the system at equilibrium favors the production of NH_(3)(g) A. decreasing the concentration of H_(2)(g) B. increasing the concentration of H_(2)(g) C. increasing the pressure on the system D. increasing the temperature of the system

Given the Haber reaction at equilibrium: N_(2)(g)+3H_(2)(g)leftharpoons 2NH_(3)(g)+heat Which stress on the system at equilibrium favors the production of NH_(3)(g) A. decreasing the concentration of H_(2)(g) B. increasing the concentration of H_(2)(g) C. increasing the pressure on the system D. increasing the temperature of the system
Given the Haber reaction at equilibrium: N_(2)(g)+3H_(2)(g)leftharpoons 2NH_(3)(g)+heat Which stress on the system at equilibrium favors the production of NH_(3)(g) A. decreasing the concentration of H_(2)(g) B. increasing the concentration of H_(2)(g) C. increasing the pressure on the system D. increasing the temperature of the system

Solution
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Answer

B. increasing the concentration of H_{2}(g) Explanation 1. Analyze Reaction Direction The reaction is exothermic. Increasing temperature shifts equilibrium to the left, favoring reactants. 2. Apply Le Chatelier's Principle Increasing H_{2}(g) concentration shifts equilibrium to the right, favoring NH_{3}(g) production. 3. Consider Pressure Effect Increasing pressure favors the side with fewer gas moles. Here, 4 moles (reactants) vs. 2 moles (products), so it favors NH_{3}(g). 4. Evaluate Options A. Decreasing H_{2}(g) shifts equilibrium left. B. Increasing H_{2}(g) shifts equilibrium right. C. Increasing pressure shifts equilibrium right. D. Increasing temperature shifts equilibrium left.

Explanation

1. Analyze Reaction Direction<br /> The reaction is exothermic. Increasing temperature shifts equilibrium to the left, favoring reactants.<br /><br />2. Apply Le Chatelier's Principle<br /> Increasing $H_{2}(g)$ concentration shifts equilibrium to the right, favoring $NH_{3}(g)$ production.<br /><br />3. Consider Pressure Effect<br /> Increasing pressure favors the side with fewer gas moles. Here, 4 moles (reactants) vs. 2 moles (products), so it favors $NH_{3}(g)$.<br /><br />4. Evaluate Options<br /> A. Decreasing $H_{2}(g)$ shifts equilibrium left.<br /> B. Increasing $H_{2}(g)$ shifts equilibrium right.<br /> C. Increasing pressure shifts equilibrium right.<br /> D. Increasing temperature shifts equilibrium left.
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