# Question fb84b

Jul 22, 2017

Good catch,the book should have included the solution species ${\text{Sn}}^{2 +}$.

#### Explanation:

The iron metal is not in solution and thus should still be left out. Thus, properly,

$E = {E}^{0} - \frac{R T}{6 F} \ln \left(\left\{{\left[{\text{Sn"^{4+}]^3}/{["Sn"^{2+}]^3["Fe}}^{3 +}\right]}^{2}\right\}\right)$

Note that the tin ion concentrations can be rendered as a ratio between oxidized and reduced solution species:

E=E^0-{RT}/{6F}ln[ { ( (["Sn"^{4+}])/(["Sn"^{2+}]))^3}/{["Fe"^{3+}]^2}]#