Question:
For the reaction \( \mathrm{N_2 + 3H_2 \rightleftharpoons 2NH_3} \), \(\Delta H = -92\) kJ/mol. The equilibrium constant \(K_p\) will increase with:
For the reaction \( \mathrm{N_2 + 3H_2 \rightleftharpoons 2NH_3} \), \(\Delta H = -92\) kJ/mol. The equilibrium constant \(K_p\) will increase with:
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For exothermic reactions, decreasing temperature increases equilibrium constant.
Updated On: Jan 6, 2026
- Increase in temperature
- Decrease in temperature
- Increase in pressure
- Addition of catalyst
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The Correct Option is B
Solution and Explanation
The reaction is exothermic. Lowering temperature favors product formation, increasing \(K_p\).
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