Answer
$\Delta S_{univ}=-476\,J/K$
The reaction is non-spontaneous.
Work Step by Step
For a spontaneous process, $\Delta S_{univ}$ is positive.
$\Delta S_{univ}=\Delta S_{sys}+\Delta S_{surr}$
$\Delta S_{surr}=\frac{-\Delta H_{sys}}{T}=\frac{-(95\,kJ)}{298\,K}=\frac{-95\times10^{3}\,J}{298\,K}=-319\,J/K$
$\Delta S_{sys}=-157\,J/K$
Therefore,
$\Delta S_{univ}=(-157\,J/K)+(-319\,J/K)=-476\,J/K$
As $\Delta S_{univ}$ is negative, the reaction is non-spontaneous.
