Statement 1: Δ G=Δ G0+2.303 R T log Q where Q is reaction quotient. Statement 2: Q may be greater or lesser than Kc or equal to Kc.

Question

Statement 1: Δ G=Δ G0+2.303 R T log Q where Q is reaction quotient. Statement 2: Q may be greater or lesser than Kc or equal to Kc. (A) Statement 1 is True, Statement 2 is True; Statement 2 is correct explanation for Statement 1 (B) Statement 1 is True, Statement 2 is True; Statement 2 is not correct explanation for Statement 1 (C) Statement 1 is True, Statement 2 is False (D) Statement 1 is False, Statement 2 is True

Tardigrade Admin · Accepted Answer

Q < Kc forward reaction Q>Kc backward reaction Q=Kc if Δ G=0

Q. Statement 1 : $Δ G = Δ G^{0} + 2.303 RT lo g Q$ where $Q$ is reaction quotient.
Statement 2 : $Q$ may be greater or lesser than $K_{c}$ or equal to $K_{c}$ .

Statement 1 is True, Statement 2 is True; Statement 2 is correct explanation for Statement 1

Statement 1 is True, Statement 2 is True; Statement 2 is not correct explanation for Statement 1

Statement 1 is True, Statement 2 is False

Statement 1 is False, Statement 2 is True

$Q < K_{c}$ forward reaction
$Q > K_{c}$ backward reaction
$Q = K_{c}$ if $Δ G = 0$

Q. Statement 1 : ΔG=ΔG0+2.303RTlogQ where Q is reaction quotient. Statement 2 : Q may be greater or lesser than Kc​ or equal to Kc​.