Choose the situation below that would result in an endothermic ?_solutionH. A)when $|\Delta _ { \text {solute } } H \mid$ $|\Delta \text { hydration } H \mid$ B)when$\left| \Delta _ { \text {solute } } H \right| \left| \Delta _ { \text {solute } } H \right|$ E)There isn't enough information to determine the answer.

Question

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

Quizplus · Accepted Answer

If $|\Delta_{solute}H|$ is greater than $|\Delta_{hydration}H|$, then the solute will require more energy to break the intermolecular forces holding it together than it will release when new intermolecular forces form between the solute and solvent molecules. This means that the process of dissolving the solute in the solvent will require a net input of energy, resulting in an endothermic process ($\Delta S_{solution}>0$ and $\Delta H_{solution}>0$).

Choose the Situation Below That Would Result in an Endothermic ∣Δsolute H∣|\Delta _ { \text {solute } } H \mid∣Δsolute ​H∣

Choose the Situation Below That Would Result in an Endothermic $|\Delta _ { \text {solute } } H \mid$