Question:
Given the equilibrium system:
\[
\text{NH₄Cl(s)} \rightleftharpoons \text{NH₃(aq)} + \text{Cl⁻(aq)} \quad \Delta H = +3.5 \, \text{Kcal/mol}
\]
What change will shift the equilibrium to the right?
Given the equilibrium system:
\[
\text{NH₄Cl(s)} \rightleftharpoons \text{NH₃(aq)} + \text{Cl⁻(aq)} \quad \Delta H = +3.5 \, \text{Kcal/mol}
\]
What change will shift the equilibrium to the right?
Show Hint
For endothermic reactions, increasing temperature shifts the equilibrium to the right.
Updated On: Jan 6, 2026
- Decreasing the temperature
- Increasing the temperature
- Dissolving NaCl crystals in the equilibrium mixture
- Dissolving NH₄NO₃ crystals in the equilibrium mixture
Show Solution
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The Correct Option is B
Solution and Explanation
Step 1: Effect of temperature on equilibrium.
For an endothermic reaction (positive \( \Delta H \)), increasing the temperature shifts the equilibrium to the right, favoring the forward reaction.
Step 2: Conclusion.
Thus, the correct answer is option (B).
Final Answer: \[ \boxed{\text{(B) Increasing the temperature}} \]
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