If the E°cell for a given reaction has a negative value, which of the following gives the correct relationships for the values of Δ G° and Keq ?

Question

If the E°cell for a given reaction has a negative value, which of the following gives the correct relationships for the values of Δ G° and Keq ? (A) Δ G° > 0 ; Keq < 1 (B) Δ G° > 0 ; Keq > 1 (C) Δ G° < 0 ; Keq > 1 (D) Δ G° < 0 ; Keq < 1

Tardigrade Admin · Accepted Answer

Δ G °=- nFE ° E o is negative So Δ G°=+v e Δ G °=-2.303 RT log K ∴ K eq < 1

Q. If the $E_{ce ll}^{\circ}$ for a given reaction has a negative value, which of the following gives the correct relationships for the values of $Δ G^{\circ}$ and $K_{e q}$ ?

$Δ G^{\circ} > 0; K_{e q} < 1$

$Δ G^{\circ} > 0; K_{e q} > 1$

$Δ G^{\circ} < 0; K_{e q} > 1$

$Δ G^{\circ} < 0; K_{e q} < 1$

$Δ G^{\circ} = - n F E^{\circ}$
$E^{o}$ is negative
So $Δ G^{\circ} = + v e$
$Δ G^{\circ} = - 2.303 RT lo g K$
$∴ K_{e q} < 1$

Q. If the Ecell∘​ for a given reaction has a negative value, which of the following gives the correct relationships for the values of ΔG∘ and Keq​ ?

ΔG∘>0;Keq​<1

ΔG∘>0;Keq​>1

ΔG∘<0;Keq​>1

ΔG∘<0;Keq​<1