The standard reduction potential Eo for half reations are Zn = Zn2+ + 2e- ; Eo = +0.76 V Fe = Fe2+ + 2e-; Eo = + 0.41 V The EMF of the cell reaction Fe2+ + Zn = Zn2+ + Fe is

Question

The standard reduction potential Eo for half reations are Zn = Zn2+ + 2e- ; Eo = +0.76 V Fe = Fe2+ + 2e-; Eo = + 0.41 V The EMF of the cell reaction Fe2+ + Zn = Zn2+ + Fe is (A) -0.35 V (B) + 0.35 V (C) +1.17 V (D) -1.17 V

Tardigrade Admin · Accepted Answer

Zn longrightarrow Zn 2++2 e- ; E oxi °=+0.76 V or E text red °=-0.76 V Fe longrightarrow Fe 2++2 e- ; E oxi °=+0.41 V or E red °=-0.41 V ∴ E text cell °=E text cathode °(R P)-E text anode °(R P) =-0.41-(0.76) =+0.35 V

Q. The standard reduction potential $E^{o}$ for half reations are
$Z n = Z n^{2 +} + 2 e^{-}; E^{o} = + 0.76 V$
$F e = F e^{2 +} + 2 e^{-}; E^{o} = + 0.41 V$
The EMF of the cell reaction
$F e^{2 +} + Z n = Z n^{2 +} + F e$ is

$- 0.35 V$

$+ 0.35 V$

$+ 1.17 V$

$- 1.17 V$

$Z n ⟶ Z n^{2 +} + 2 e^{-}; E_{o x i}^{\circ} = + 0.76 V$
or $E_{red}^{\circ} = - 0.76 V$
$F e ⟶ F e^{2 +} + 2 e^{-}; E_{o x i}^{\circ} = + 0.41 V$
or $E_{re d}^{\circ} = - 0.41 V$
$∴ E_{cell}^{\circ} = E_{cathode}^{\circ} (RP) - E_{anode}^{\circ} (RP)$
$= - 0.41 - (0.76)$
$= + 0.35 V$

Q. The standard reduction potential Eo for half reations are Zn=Zn2++2e−;Eo=+0.76V Fe=Fe2++2e−;Eo=+0.41V The EMF of the cell reaction Fe2++Zn=Zn2++Fe is

−0.35V

+0.35V

+1.17V

−1.17V