Answer
$\Delta S_{univ}=-649\,J/K$, nonspontaneous.
Work Step by Step
For a spontaneous process, $\Delta S_{univ}$ is positive.
$\Delta S_{univ}=\Delta S_{sys}+\Delta S_{surr}$
$\Delta S_{surr}=\frac{-\Delta H_{sys}}{T}=\frac{-(115\,kJ)}{298\,K}=\frac{-115\times10^{3}\,J}{298\,K}=-386\,J/K$
$\Delta S_{sys}=-263\,J/K$
Therefore,
$\Delta S_{univ}=(-263\,J/K)+(-386\,J/K)=-649\,J/K$
As $\Delta S_{univ}$ is negative, the reaction is nonspontaneous.
