25° C তাপমাত্রায় নিম্নোক্ত সাম্যবস্থা দেওয়া আছে; \( NH_4Cl(s) \leftrightarrow NH_4^+(aq) + Cl^-(aq) \) (\( \Delta H = +3.5 \) Kcal mol\(^{-1}\))। কোন পরিবর্তনটি সাম্যবস্থানটিকে ডান দিকে স্থানান্তরিত করবে?

Explanation of the Effect of Temperature Increase on the Equilibrium

Given the reaction:

\( NH_4Cl(s) \leftrightarrow NH_4^+(aq) + Cl^-(aq) \)

with an enthalpy change \( \Delta H = +3.5 \) Kcal/mol, indicating that the reaction is endothermic.

Effect of Increasing Temperature:

• According to Le Châtelier's principle, if the temperature of an endothermic reaction is increased, the equilibrium will shift to favor the formation of products to absorb the excess heat.
• Since \(\Delta H\) is positive, increasing temperature supplies more heat, thus shifting the equilibrium to the right (products side).
• This shift results in more \(\mathrm{NH_4^+}\) and \(\mathrm{Cl^-}\) ions in solution.

Conclusion:

Therefore, increasing the temperature to 35°C will shift the equilibrium towards the right, favoring the dissociation of \(\mathrm{NH_4Cl}\).