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Gibbs Free Energy & Spontaneity

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Question

Calculate the entropy change when 36 g of liquid water evapourates at 373 K .Change in Enthalpy of vapourisation =40.63KJ/mol

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Solution

$∆ S_{V a p} = \frac{∆ H_{V a p}}{T_{b}} = \frac{40.63 \times 1000}{373} = 109 J K^{- 1} m o l^{- 1} E n t r o p y c h a n g e f o r t h e e v a p o r a t i o n o f 36 g o f w a t e r = \frac{109}{18} \times 36 = 218 J K^{- 1}$

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