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Questions  >>  JEEMAIN and NEET  >>  Physics  >>  Class11  >>  Thermodynamics
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Calculate the entropy change when 36 g of liquid water evaporates at $373\: K( \Delta H_{vap} = 40.63\: kJ/mol)$

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

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