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° C is to a volume of 100 dm 3

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° 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

Tardigrade Admin · Accepted Answer

Δ S=2.303 n log (V2/V1) Δ S=2.303 × 2 × 8.314 × log (100/10) Lambda S=38.3 J mol -1 K -1

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

$42.3 J m o l^{- 1} K^{- 1}$

$38.3 J m o l^{- 1} K^{- 1}$

$35.8 J m o l^{- 1} K^{- 1}$

$32.3 J m o l^{- 1} K^{- 1}$

$Δ S = 2.303 n lo g \frac{V _{2}}{V _{1}}$
$Δ S = 2.303 \times 2 \times 8.314 \times lo g \frac{100}{10}$
$Λ S = 38.3 J m o l^{- 1} K^{- 1}$

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

42.3Jmol−1K−1

38.3Jmol−1K−1

35.8Jmol−1K−1

32.3Jmol−1K−1