Calculate the entropy change when 36 g of liquid water evaporates at $373\: K( \Delta H_{vap} = 40.63\: kJ/mol)$

Question

$\begin {array} {1 1} (A)\;109 \: J/K-mol & \quad (B)\;-109\: J/K-mol \\ (C)\;-218\: J/K-mol & \quad (D)\;218\: J/K-mol \end {array}$