What is the entropy change when 1 mole oxygen gas expands isothermally and reversibly from an initial volume of 10 L to 100 L at 300 K?

Question

What is the entropy change when 1 mole oxygen gas expands isothermally and reversibly from an initial volume of 10 L to 100 L at 300 K? (A) 19.14 J K-1 (B) 109.12 J K-1 (C) 29.12 J K-1 (D) 10 J K-1

Tardigrade Admin · Accepted Answer

Δ S = 2.303nR log (V2/V1) = 2.303 × 1 × 8.314 log (100/10) = 19.14 J K-1

Q. What is the entropy change when $1$ mole oxygen gas expands isothermally and reversibly from an initial volume of $10 L$ to $100 L$ at $300 K$ ?

$19.14 J K^{- 1}$

$109.12 J K^{- 1}$

$29.12 J K^{- 1}$

$10 J K^{- 1}$

$Δ S = 2.303 n R l o g \frac{V _{2}}{V _{1}}$
$= 2.303 \times 1 \times 8.314 l o g \frac{100}{10}$
$= 19.14 J K^{- 1}$

Q. What is the entropy change when 1 mole oxygen gas expands isothermally and reversibly from an initial volume of 10L to 100L at 300K?

19.14JK−1

109.12JK−1

29.12JK−1

10JK−1