Choose the situation below that would result in a ?_solutionH near 0. A)when $\left| \Delta _ { \text {solvent } } H \right|$ $\Delta _ { \text {solute } } H \mid$ B)when $\Delta _ { \text {solute } } H \mid$ $\Delta \text { hydration } H \mid$ C)when $|\Delta _ { \text {solute } } H \mid$

Question

Choose the situation below that would result in a ?_solutionH near 0. A)when $\left| \Delta _ { \text {solvent } } H \right|$ >$\Delta _ { \text {solute } } H \mid$ B)when $\Delta _ { \text {solute } } H \mid$ >$\Delta \text { hydration } H \mid$ C)when $|\Delta _ { \text {solute } } H \mid$ <$|\Delta \text { hydration } H \mid$ D)when $|\Delta _ { \text {solute } } H \mid$ is close to$|\Delta \text { hydration } H \mid$ E)There isn't enough information to determine the answer.

Quizplus · Accepted Answer

Δ_solutionH is the change in standard molar entropy when a solute is dissolved in a solvent to form a solution. It depends on the enthalpy changes during the process, such as ΔsoluteH and ΔhydrationH. When these two values are close to each other, there will not be a significant change in the standard molar entropy of the solution, resulting in a Δ_solutionH near 0. Therefore, option D is the best choice.

Choose the Situation Below That Would Result in a ?solutionH ∣Δsolvent H∣\left| \Delta _ { \text {solvent } } H \right|∣Δsolvent ​H∣

Choose the Situation Below That Would Result in a ?_solutionH $\left| \Delta _ { \text {solvent } } H \right|$