Calculate the change in entropy when 1 mole nitrogen gas expands isothermally and reversibly from an initial volume of 1 litre to a final volume of 10 litre at 27° C.

Question

Calculate the change in entropy when 1 mole nitrogen gas expands isothermally and reversibly from an initial volume of 1 litre to a final volume of 10 litre at 27° C. (A) 19.15 J K -1 (B) 20.18 J K -1 (C) 16.15 J K -1 (D) 17.16 J K -1

Tardigrade Admin · Accepted Answer

Δ S =2.303 n R log ((V2/V1)) =2.303 × 1 × 8.314 log ((10/1))=19.15 J K -1

Q. Calculate the change in entropy when $1$ mole nitrogen gas expands isothermally and reversibly from an initial volume of $1$ litre to a final volume of $10$ litre at $2 7^{\circ} C$ .

$19.15 J K^{- 1}$

$20.18 J K^{- 1}$

$16.15 J K^{- 1}$

$17.16 J K^{- 1}$

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

$= 2.303 \times 1 \times 8.314 lo g (\frac{10}{1}) = 19.15 J K^{- 1}$

Q. Calculate the change in entropy when 1 mole nitrogen gas expands isothermally and reversibly from an initial volume of 1 litre to a final volume of 10 litre at 27∘C.

19.15JK−1

20.18JK−1

16.15JK−1

17.16JK−1