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JEE Main levelSingle correct optionDifficulty 2 of 3td140

Three moles of liquid water ( $C_{P} = 75.3 J mo l^{- 1} K^{- 1}$ , assumed constant) are heated reversibly at constant pressure from $300 K$ to $350 K$ . The entropy change of the water is

A $32.3 J K^{- 1}$
B $37.6 J K^{- 1}$
C $15.1 J K^{- 1}$
D $34.8 J K^{- 1}$

Answer: D

Δ S = n C_{P} ln (T_{2} / T_{1}) = 3 \times 75.3 \times ln (350/300) = 34.8 J K^{- 1}

. Dividing the heat by only the final or the initial temperature gives

32.3

or

37.6

, and using

lo g_{10}

gives

15.1

.

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