Answer
$\Delta S_{univ}=-46\,J/K$, the reaction is non-spontaneous.
Work Step by Step
For a spontaneous process, $\Delta S_{univ}$ is positive.
$\Delta S_{univ}=\Delta S_{sys}+\Delta S_{surr}$
$\Delta S_{surr}=\frac{-\Delta H_{sys}}{T}=\frac{-(-95\,kJ)}{855\,K}=\frac{95\times10^{3}\,J}{855\,K}=111\,J/K$
$\Delta S_{sys}=-157\,J/K$
Therefore,
$\Delta S_{univ}=(-157\,J/K)+(111\,J/K)=-46\,J/K$
As $\Delta S_{univ}$ is negative, the reaction is non-spontaneous.
