Question:
Consider the equilibrium reaction, \(X(g) + Y(g) \rightleftharpoons W(g) + Z(g)\). The equilibrium constant \(K_C\) for the reaction is \(2.0 \times 10^2\) at 300 K and it decreases with increase in temperature. Which of the following is true for the reaction?
Consider the equilibrium reaction, \(X(g) + Y(g) \rightleftharpoons W(g) + Z(g)\). The equilibrium constant \(K_C\) for the reaction is \(2.0 \times 10^2\) at 300 K and it decreases with increase in temperature. Which of the following is true for the reaction?
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$K \propto 1/T$ for exothermic; $K \propto T$ for endothermic reactions.
Updated On: Apr 27, 2026
- $\Delta H<0$
- $\Delta G<0$
- $\Delta S<0$
- $\Delta H>0$
- $\Delta S>0$
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The Correct Option is A
Solution and Explanation
Step 1: Concept
Le Chatelier's Principle regarding temperature.
Step 2: Meaning
If $K$ decreases as $T$ increases, the equilibrium shifts toward the reactants.
Step 3: Analysis
A shift toward reactants with added heat implies the forward reaction is exothermic.
Step 4: Conclusion
For exothermic reactions, $\Delta H$ is negative ($\Delta H<0$). Correct answer is (A).
Final Answer: (A)
Le Chatelier's Principle regarding temperature.
Step 2: Meaning
If $K$ decreases as $T$ increases, the equilibrium shifts toward the reactants.
Step 3: Analysis
A shift toward reactants with added heat implies the forward reaction is exothermic.
Step 4: Conclusion
For exothermic reactions, $\Delta H$ is negative ($\Delta H<0$). Correct answer is (A).
Final Answer: (A)
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