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JEE Main levelNumerical answerDifficulty 2 of 3td045

$150 g$ of liquid water ( $c_{P} = 4.18 J g^{- 1} K^{- 1}$ , assumed constant) is heated reversibly from $293 K$ to $353 K$ . The entropy change of the water in $J K^{- 1}$ (one decimal) is

Numerical answer type, answer in J/K, tolerance 0.2.

Answer: 116.8 J/K

Δ S = m c_{P} ln (T_{2} / T_{1}) = 150 (4.18) ln (353/293) = 627 \times 0.18630 = 116.81 J K^{- 1}

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