Δ G 0 for the reaction, Cu 2++ Fe arrow Fe 2++ Cu is: [given: . E Cu 2+ / Cu 0=+0.34 V , E Fe 2+ / Fe 0=-0.44 V ]

Question

Δ G 0 for the reaction, Cu 2++ Fe arrow Fe 2++ Cu is: [given: . E Cu 2+ / Cu 0=+0.34 V , E Fe 2+ / Fe 0=-0.44 V ] (A) 11.44 KJ (B) 180.8 KJ (C) -150.5 KJ (D) 28.5 KJ

Tardigrade Admin · Accepted Answer

E text cell 0= E Cu 2+ / Cu 0- E Fe 2+ / Fe 0 =0.34-(-0.44)=0.78 Δ G 0=- n FE text cell 0 =-2 × 96500 × 0.78 =150540 J =-150.5 KJ

Q. $Δ G^{0}$ for the reaction, $C u^{2 +} + F e \to F e^{2 +} + C u$ is: [given: $E_{C u^{2 +} / C u}^{0} = + 0.34 V, E_{F e^{2 +} / F e}^{0} = - 0.44 V]$

11.44 KJ

180.8 KJ

-150.5 KJ

28.5 KJ

$E_{cell}^{0} = E_{C u^{2 +} / C u}^{0} - E_{F e^{2 +} / F e}^{0}$
$= 0.34 - (- 0.44) = 0.78$
$Δ G^{0} = - n F E_{cell}^{0}$
$= - 2 \times 96500 \times 0.78$
$= 150540 J$
$= - 150.5 K J$

Q. ΔG0 for the reaction, Cu2++Fe→Fe2++Cu is: [given: ECu2+/Cu0​=+0.34V,EFe2+/Fe0​=−0.44V]