The standard electrode potential for the half-cell reactions are Zn 2++2 e- longrightarrow Zn ; E°=-0.76 V Fe 2++2 e- longrightarrow Fe ; E°=-0.44 V The emf of the cell reaction, Fe 2++ Zn longrightarrow Zn 2++ Fe is

Question

The standard electrode potential for the half-cell reactions are Zn 2++2 e- longrightarrow Zn ; E°=-0.76 V Fe 2++2 e- longrightarrow Fe ; E°=-0.44 V The emf of the cell reaction, Fe 2++ Zn longrightarrow Zn 2++ Fe is (A) 0.32 V (B) -0.32 V (C) +1.20 V (D) -1.20 V

Tardigrade Admin · Accepted Answer

beginaligned E text cell 0 &=( E Fe 2+ Fe 0+ E ZnZnh 2+0) &=(-0.44 V +0.76) E 0 &=+0.32 V text olt endaligned

Q. The standard electrode potential for the half-cell reactions are
$Z n^{2 +} + 2 e^{-} ⟶ Z n; E^{\circ} = - 0.76 V$
$F e^{2 +} + 2 e^{-} ⟶ F e; E^{\circ} = - 0.44 V$
The emf of the cell reaction,
$F e^{2 +} + Z n ⟶ Z n^{2 +} + F e$ is

0.32 V

-0.32 V

+1.20 V

-1.20 V

$E_{cell}^{0} E^{0} = (E_{F e^{2 +} F e}^{0} + E_{Z n Z n h^{2 +}}^{0}) = (- 0.44 V + 0.76) = + 0.32 V olt$

Q. The standard electrode potential for the half-cell reactions are Zn2++2e−⟶Zn;E∘=−0.76V Fe2++2e−⟶Fe;E∘=−0.44V The emf of the cell reaction, Fe2++Zn⟶Zn2++Fe is