Five moles of an ideal gas expands reversibly from a volume of 8 dm3 to 80 dm3 at a temperature of 27°C. Calculate the change in entropy.

Question

Five moles of an ideal gas expands reversibly from a volume of 8 dm3 to 80 dm3 at a temperature of 27°C. Calculate the change in entropy. (A) 70.26 JK-1 (B) 82.55 JK-1 (C) 95.73 JK-1 (D) 107.11 JK-1

Tardigrade Admin · Accepted Answer

Entropy change (Δ S)=2.303 nRT log (V2/V1) =2.303×5×8.314× log (80/8)=95.73 JK-1

Q. Five moles of an ideal gas expands reversibly from a volume of $8 d m^{3}$ to $80 d m^{3}$ at a temperature of $2 7^{\circ} C$ . Calculate the change in entropy.

$70.26 J K^{- 1}$

$82.55 J K^{- 1}$

$95.73 J K^{- 1}$

$107.11 J K^{- 1}$

Entropy change $(Δ S) = 2.303 n RTl o g \frac{V _{2}}{V _{1}}$
$= 2.303 \times 5 \times 8.314 \times l o g \frac{80}{8} = 95.73 J K^{- 1}$

Q. Five moles of an ideal gas expands reversibly from a volume of 8dm3 to 80dm3 at a temperature of 27∘C. Calculate the change in entropy.

70.26JK−1

82.55JK−1

95.73JK−1

107.11JK−1