Consider the following Eo values. EoFe3+/Fe2+ =+0.77V Eo sn2+ /sn =-0.14 V. the Eo cellfor the reaction; Sn(s) +2Fe3+ (aq.) →2Fe2(aq) +Sn2+ (aq) is.

Question

Consider the following Eo values. EoFe3+/Fe2+ =+0.77V Eo sn2+ /sn =-0.14 V. the Eo cellfor the reaction; Sn(s) +2Fe3+ (aq.) →2Fe2(aq) +Sn2+ (aq) is. (A) 0.63 V (B) 1.40 V (C) 0.91 V (D) 1.68 V

Tardigrade Admin · Accepted Answer

Eo cell=Eo opsn/sn2++Eo RPFe3+ /fe2+ = 0.14 + 0.77 = 0.91 V

Q. Consider the following $E^{o}$ values. $E_{F e^{3 +} / F e^{2 +}}^{o} = + 0.77 V$
$E_{s n^{2 +} / s n}^{o} = - 0.14 V .$ the $E_{ce ll}^{o}$ for the reaction;
$S n (s) + 2 F e^{3 +} (a q .) \to 2 F e^{2} (a q) + S n^{2 +} (a q)$ is.

$0.63 V$

$1.40 V$

$0.91 V$

$1.68 V$

$E_{ce ll}^{o} = E_{o p s n / s n^{2 +}}^{o} + E_{RPF e^{3 +} / f e^{2 +}}^{o}$
$= 0.14 + 0.77 = 0.91 V$

Q. Consider the following Eo values. EFe3+/Fe2+o​=+0.77V Esn2+/sno​=−0.14V. the Ecello​for the reaction; Sn(s)+2Fe3+(aq.)→2Fe2(aq)+Sn2+(aq) is.

0.63V

1.40V

0.91V

1.68V