Two moles of an ideal gas are allowed to expand reversibly and isothermally at 300 K from a pressure of 1 atm to a pressure of 0.1 atm. The change in Gibbs free energy is

Question

Two moles of an ideal gas are allowed to expand reversibly and isothermally at 300 K from a pressure of 1 atm to a pressure of 0.1 atm. The change in Gibbs free energy is (A) -11.488 J (B) +11.488 J (C) -11.488 kJ (D) zero

Tardigrade Admin · Accepted Answer

Use the following equation, Δ G=2303 n R T log ((p2/p1)) ∴ Δ G=2.303 × 2 ×(8.314 J K-1 mol -1) ×(300 K) × log ((0.1 atm /1 atm )) =-11488 J =-11.488 kJ

Q. Two moles of an ideal gas are allowed to expand reversibly and isothermally at $300 K$ from a pressure of $1 a t m$ to a pressure of $0.1 a t m$ . The change in Gibbs free energy is

-11.488 J

+11.488 J

-11.488 kJ

zero

Use the following equation,
$Δ G = 2303 n RT lo g (\frac{p _{2}}{p _{1}})$
$∴ Δ G = 2.303 \times 2 \times (8.314 J K^{- 1} m o l^{- 1})$
$\times (300 K) \times lo g (\frac{0.1 a t m}{1 a t m})$
$= - 11488 J = - 11.488 k J$

Q. Two moles of an ideal gas are allowed to expand reversibly and isothermally at 300K from a pressure of 1atm to a pressure of 0.1atm. The change in Gibbs free energy is