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?

• A. Decreasing the temperature
• B. Increasing the temperature
• C. Dissolving NaCl crystals in the equilibrium mixture
• D. Dissolving NH₄NO₃ crystals in the equilibrium mixture

Hint:

For endothermic reactions, increasing temperature shifts the equilibrium to the right.

Answer 1

The Correct Option is B

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: \[ \boxed{\text{(B) Increasing the temperature}} \]