Question

The entropy change involved in the isothermal reversible expansion of $2$ moles of an ideal gas from a volume of $10\, dm ^{3}$ at $27^{\circ} C$ is to a volume of $100\, dm ^{3}$

• A. $42.3\, J\, mol ^{-1} K ^{-1}$
• B. $38.3\, J\, mol ^{-1} K ^{-1}$
• C. $35.8\, J\, mol ^{-1} K ^{-1}$
• D. $32.3\, J\, mol ^{-1} K ^{-1}$

Answer 1

Answer: (B)

$38.3\, J\, mol ^{-1} K ^{-1}$

Answer 2

$\Delta S=2.303\, n\,\log \frac{V_{2}}{V_{1}}$ $\Delta S=2.303 \times 2 \times 8.314 \times \log \frac{100}{10}$ $\Lambda S=38.3\, J\, mol ^{-1} K ^{-1}$