Question:
If the reaction \( \text{N}_2 + 3\text{H}_2 \rightarrow 2\text{NH}_3 \) occurs at 200°C and 1000 atm then the graph showing the correct equilibrium yield at 400°C is
If the reaction \( \text{N}_2 + 3\text{H}_2 \rightarrow 2\text{NH}_3 \) occurs at 200°C and 1000 atm then the graph showing the correct equilibrium yield at 400°C is
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For exothermic reactions, increasing temperature shifts the equilibrium to favor the reactants, decreasing the product concentration.
Updated On: Jan 12, 2026
- A
- B
- C
- D
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The Correct Option is B
Solution and Explanation
Step 1: Le Chatelier’s Principle.
According to Le Chatelier’s principle, increasing the temperature of an exothermic reaction (like the formation of ammonia) will shift the equilibrium to the left, decreasing the concentration of ammonia at higher temperatures.
Step 2: Conclusion.
The correct answer is (B), \( [NH_3] \) vs \( T \) (200°C to 400°C) is decreasing.
According to Le Chatelier’s principle, increasing the temperature of an exothermic reaction (like the formation of ammonia) will shift the equilibrium to the left, decreasing the concentration of ammonia at higher temperatures.
Step 2: Conclusion.
The correct answer is (B), \( [NH_3] \) vs \( T \) (200°C to 400°C) is decreasing.
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