Consider the reaction for the dissolution of ammonium nitrate:
`NH_(4)NO_(3)(s) rarr NH_(4)^(o+)(aq) +NO_(3)^(Theta) (aq)`
`DeltaH =+29.8 KJ mol^(-1), DeltaS = 108.0 J K^(-1) mol^(-1)`.
Calculate the change in entropy of the surroundings and predict whether the reaction is spontaneous or not at `25^(@)C`?

Explanation

To solve the problem, we need to calculate the change in entropy of the surroundings and then determine whether the reaction is spontaneous at 25°C.

### Step 1: Calculate the change in entropy of the surroundings (ΔS_surroundings)

The formula for the change in entropy of the surroundings is given by:

\[
\Delta S_{\text{surroundings}} = -\frac{\Delta H}{T}
...