Calculate entropy change when 5 moles of an ideal gas expands reversibly and isothermally from an initial volume of 5 litre to 50 litre at 27° C

Question

Calculate entropy change when 5 moles of an ideal gas expands reversibly and isothermally from an initial volume of 5 litre to 50 litre at 27° C (A) 190.15 J K -1 (B) 95.74 J K -1 (C) 87.25 J K -1 (D) 90.13 J K -1

Tardigrade Admin · Accepted Answer

Δ S =2.303 n R log (V2/V1) = 2.303 × 5 × 8.314 log (50/5)=95.74 JK -1

Q. Calculate entropy change when $5$ moles of an ideal gas expands reversibly and isothermally from an initial volume of $5$ litre to $50$ litre at $2 7^{\circ} C$

$190.15 J K^{- 1}$

$95.74 J K^{- 1}$

$87.25 J K^{- 1}$

$90.13 J K^{- 1}$

$Δ S = 2.303 n R lo g \frac{V _{2}}{V _{1}}$

$= 2.303 \times 5 \times 8.314 lo g \frac{50}{5} = 95.74 J K^{- 1}$

Q. Calculate entropy change when 5 moles of an ideal gas expands reversibly and isothermally from an initial volume of 5 litre to 50 litre at 27∘C

190.15JK−1

95.74JK−1

87.25JK−1

90.13JK−1