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JEE Main levelSingle correct optionDifficulty 2 of 3td040

Two moles of an ideal gas expand isothermally from $5.0 L$ to $20 L$ . With $R = 8.314 J mo l^{- 1} K^{- 1}$ , the entropy change of the gas is

A $11.53 J K^{- 1}$
B $23.05 J K^{- 1}$
C $10.01 J K^{- 1}$
D $66.5 J K^{- 1}$

Answer: B

Δ S = n R ln (V_{2} / V_{1}) = 2 (8.314) ln 4 = 23.05 J K^{- 1}

. This holds for any path between the two states because

S

is a state function.

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