The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10 dm3 to a volume of 100 dm3 at 27°C is

Engineering

Chemistry

Entropy Calculations

Question

The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10 dm³ to a volume of 100 dm³ at 27°C is

35.8 J mol^–1 K^–1

38.3 J mol^–1 K^–1

32.3 J mol^–1 K^–1

42.3 J mol^–1 K^–1

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$ΔS = nRln \frac{V_{2}}{V_{1}}$

$= 2.303 nRlog \frac{V_{2}}{V_{1}}$

$= 2.303 \times 2 \times 8.314 \times \log \frac{100}{10}$

=38.3 J mol^–1 K^–1

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