Q. Given the equilibrium system $NH_{4}Cl(s) \rightleftharpoons NH_{4}^{+}(aq) + Cl^{-}(aq)\ \ \ \ \ \$ $\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ (\mathrm{\Delta}H = + 3.5$ 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 $NH_{4}NO_{3}$ crystals in the equilibrium mixture
Explanation
(b)
$H_{4}Cl(s) \rightleftharpoons NH_{4}^{+}(aq) + Cl^{-}(aq);\ \ \ \ \ \ \ \mathrm{\Delta}H = + 3.5$ kcal/mol
This is the endothermic reaction hence, increasing the temperature will shift the equilibrium to the right.
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.