Calculate the entropy change when $36\;g$ of liquid water evaporates at $373\;K(\Delta _{vap} H=40.63\;kJ\;mol^{-1})$

Question

$\begin{array}{1 1} (a)\;218\;JK^{-1} \\ (b)\;318\;JK^{-1}\\ (c)\;418\;JK^{-1} \\ (d)\;118\;JK^{-1} \end{array}$