Question

If a solute dissolves in an endothermic process Question 10 options: a) the solute must be a gas. b) the entropy of the solution must be greater than that of its pure components. c) H bonds must exist between solvent and solute. d) the entropy of the solution is immaterial. e) strong ion-dipole forces must exist in the solution.

Answer 1

Answer: If a solute dissolves in an endothermic process the entropy of the solution must be greater than that of its pure components.

Explanation:

An endothermic process is defined as the process in which heat is absorbed by the reactant molecules taking part in a chemical reaction.

But in an endothermic process it is not possible to determine the type of bond present in the chemical atoms.

Also, we know that a spontaneous reaction between the solute and solvent leads to dissolution of solute particles. For such type of reactions, $\Delta G < 0$.

We know that,

         $\Delta G = \Delta H - T \Delta S$ .......... (1)

For this, heat at constant pressure, $\Delta H > 0$ (for an endothermic process).

According to equation (1), more is the entropy of solution ($\Delta S > 0$) more will be the negative value of $\Delta G$.

Thus, we can conclude that if a solute dissolves in an endothermic process the entropy of the solution must be greater than that of its pure components.