Question

Which of the following statements is correct for a reversible
process in a state of equilibrium ?
(a) ∆G = 2.30 RT log K [2015]
(b) ∆Gº = –2.30 RT log K
(c) ∆Gº = 2.30 RT log K
(d) ∆G = –2.30 RT log K

Answer 1

Answer:

options a is correct ....

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Answer 2

Correct statement for a reversible

process in a state of equilibrium is :

• Thermodynamic equation for Gibbs free energy is given by

• ΔG = ΔG° + 2.30RTlogQr .... (1)

• where, ΔG = Gibbs free energy change per mole of reaction,

ΔG° = Gibbs free energy change per mole of reaction for unmixed reactants and products at standard condition

R = gas constant

T = absolute temperature

Qr = reaction quotient

• In equilibrium, ∆G = 0 and Qr = K

• Therefore equation (1) will be

0 = ∆G° + 2.30RTlogK

• where, K = equilibrium constant

• Hence correct statement is :

∆G° = -2.30RTlogK