1. Tardigrade
  2. Question
  3. Chemistry
  4. 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.

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Q. Consider the following $E^{o}$ values. $E^{o}_{Fe^{3+}/Fe^{2+}} =+0.77V$
$E^{o} _{sn^{2+} /sn} =-0.14 V.$ the $E^{o} _{cell}$for the reaction;
$Sn(s) +2Fe^{3+} (aq.) \to2Fe^{2}(aq) +Sn^{2+} (aq)$ is.

Electrochemistry

Solution:

$E^{o} _{cell}=E^{o} _{opsn/sn^{2+}}+E^{o} _{RPFe^{3+} /fe^{2+}}$
$= 0.14 + 0.77 = 0.91 V$