The entropy change involved in the isothermal reversible expansion of 2 moles of

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Question
The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10 dm3 at 27�C is to a volume of 100 dm3
Options
A. 42.3 J/ mole / K
B. 38.3 J/ mole / K
C. 35.8 J/ mole / K
D. 32.3 J/ mole / K

Correct Answer

38.3 J/ mole / K

Explanation

$? s = n R \ln \frac{v 2}{v 1}$

$= 2.303 n R \log \frac{v 2}{v 1}$ = $2.303 � 2 � 8.314 � \log (\frac{100}{10})$ = $38.3 J$ $m o l^{- 1}$ $k^{- 1}$

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