For a reversible isothermal expansion of an ideal gas

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$\begin{aligned} Δ S_{sys} = Δ S_{surr} = 0 \end{aligned}$

$\begin{aligned} Δ S_{sys} = - Δ S_{surr} \end{aligned}$

$\begin{aligned} Δ S_{sys} = Δ S_{surr} = negative \end{aligned}$

$\begin{aligned} Δ S_{sys} = Δ S_{surr} = positive \end{aligned}$

answer is B.

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Detailed Solution

In the reversible isothermal expansion, temperature of the system and surroundings are taken to be identical. Since heat absorbed by the system is equal to the heat lost by the surroundings, $Δ S_{sys}$ and $Δ S_{sum}$ will have equal value but carry opposite sign.

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