Answer
$\Delta S_{univ}=-76\,J/K$
The reaction is nonspontaneous.
Work Step by Step
For a spontaneous process, $\Delta S_{univ}$ is positive.
$\Delta S_{univ}=\Delta S_{sys}+\Delta S_{surr}$
$\Delta S_{surr}=\frac{-\Delta H_{sys}}{T}=\frac{-(-115\,kJ)}{615\,K}=\frac{115\times10^{3}\,J}{615\,K}=187\,J/K$
$\Delta S_{sys}=-263\,J/K$
Therefore,
$\Delta S_{univ}=(-263\,J/K)+(187\,J/K)=-76\,J/K$
As $\Delta S_{univ}$ is negative, the reaction is non-spontaneous.
