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What will be the value of change in entropy in JK^-1 mol^-1 when 0.1 mole of an ideal gas expanded reversibly two times of its initial volume at 25⁰C. $(\ln 2 = 0.69)$

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0.57

1.38

1.14

2.68

answer is A.

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Detailed Solution

$ΔS = \frac{q}{T} = \frac{nRTln \frac{V_{2}}{V_{1}}}{T} = 0 .1 \times 8 .314 \times \ln (2) = 0 .5736 {JK}^{- 1} {mol}^{- 1}$

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