Which of the following statements is correct for a reversible process in a state of equilibrium?

Question

Which of the following statements is correct for a reversible process in a state of equilibrium? (A) Δ G° = - 2.30 RT log K (B) Δ G° = 2.30 RT log K (C) Δ G = - 2.30 RT log K (D) Δ G = 2.30 RT log K

Tardigrade Admin · Accepted Answer

The relationship between the Gibbs free energy change

Δ G

, the standard Gibbs free energy change

Δ G^{\circ}

and the equilibrium constant

K

is

Δ G = Δ G^{o} + 2.303 RT lo g K

For a reversible process in a state of equilibrium

Δ G = 0

Hence,

0 = Δ G^{0} + 2.303 RT lo g K

Δ G^{o} = - 2.303 RT lo g K

Q. Which of the following statements is correct for a reversible process in a state of equilibrium?

$ΔG X^{\circ} = - 2.30 RT log K$

$ΔG X^{\circ} = 2.30 RT log K$

$ΔG = - 2.30 RT log K$

$ΔG = 2.30 RT log K$

Q. Which of the following statements is correct for a reversible process in a state of equilibrium?

ΔGX∘=−2.30RT log K

ΔGX∘=2.30RT log K

ΔG=−2.30RT log K

ΔG=2.30RT log K

The relationship between the Gibbs free energy change ΔG, the standard Gibbs free energy change ΔG∘ and the equilibrium constant K is ΔG=ΔGo+2.303RTlogK For a reversible process in a state of equilibrium ΔG=0 Hence, 0=ΔG0+2.303RTlogK ΔGo=−2.303RTlogK

$ΔG X^{\circ} = - 2.30 RT log K$

$ΔG X^{\circ} = 2.30 RT log K$

$ΔG = - 2.30 RT log K$

$ΔG = 2.30 RT log K$