The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10 dm^3 to a volume of 100 dm^3 at 27^ - Chemistry MCQ FIITJEE AIEEE 2011 (Set Q) 2026 | ExamTest.live

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The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10 dm^{3} to a volume of 100 dm^{3} at 2 7^{\circ} C is:

Solution & Step-by-step Explanation

For isothermal reversible expansion: Δ S = n R ln \frac{V _{2}}{V _{1}} . Δ S = 2 \times 8.314 \times 2.303 \times lo g_{10} \frac{100}{10} Δ S = 2 \times 8.314 \times 2.303 \times 1 \approx 38.3 J/K .Per mole value calculation varies with question intent; usually n is included. Δ S = 38.29 J/K .

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The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10 dm^{3} to a volume of 100 dm^{3} at 2 7^{\circ} C is:

35.8 J mol^{- 1} K^{- 1}

32.3 J mol^{- 1} K^{- 1}

42.3 J mol^{- 1} K^{- 1}

38.3 J mol^{- 1} K^{- 1}

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