Answer
$-198.7\,J\,mol^{-1}K^{-1}$
Work Step by Step
We find:
$\Delta S^{\circ}=\Sigma n_{p}S^{\circ}(products)-\Sigma n_{r}S^{\circ}(reactants)$
$=[2S^{\circ}(NH_{3},g)]-[S^{\circ}(N_{2},g)+3S^{\circ}(H_{2},g)]$
$=[2(192.5\,J\,mol^{-1}K^{-1})]-[(191.6\,J\,mol^{-1}K^{-1})+3(130.7\,J\,mol^{-1}K^{-1})]$
$=-198.7\,J\,mol^{-1}K^{-1}$