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1 mol of an ideal gas at 25°C is subjected to expand reversibly 10 times of its initial volume. Calculate the change in entropy of expansions.

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Detailed Solution

$We have, Δ S = \frac{q_{1}}{T} = \frac{2.303 n R T \log_{10} \frac{V_{2}}{V_{1}}}{T}$

$\begin{array}{l} Given, n = 1, R = 8.314 J, T = 298 K, V_{1} = V, V_{2} = 10 V \\ ∴ Δ S = 2.303 \times 1 \times 8.314 \times 298 \log_{10} \frac{10 V}{V} \\ = 19.15 {JK}^{- 1} {mol}^{- 1} . \end{array}$

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