Review I Constants I Periodic Table ${?}_{(})$

Part A

A solution is made by dissolving $9\mathrm{.}7gKBr$ in $135mL$ of $H_{2}O.$ Once the mixing is complete, no solid $KBr$ remains, and the temperature of the solution drops by $4C$ from the temperature before mixing. If we define the system as the $KBr$ plus the $H_{2}O,$ the enthalpy of the system and the entropy of the system upon forming the solution.

increases, increases

increases, decreases

decreases, decreases

decreases, increases

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Incorrect; Try Again

Dissolving an ionic solid like $KBr$ in a solvent provides more degrees of freedom for the $K^{+}$and $B{r}^{-}$ions to move around, which leads to an increase, not a decrease, in the entropy of the system.