Problem: Consider this reaction.Sn2+ (aq) + 2 Fe3+ (aq) → Sn4+ (aq) + 2 Fe2+ (aq)     E° = 0.617 VWhat is the value of E when [Sn2+] and {Fe3+] are equal to 0.50 M and [Sn4+] and [Fe2+] are equal to 0.10 M?(A) 0.069V(B) 0.679 V(C) 0.658 V(D) 0.576

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We are asked to find the cell potential of the given reaction. We will use the Nernst Equation to calculate for the cell potential with the given conditions. The Nernst Equation relates the concentrations of compounds and cell potential.

Ecell = cell potential under non-standard conditions
cell = standard cell potential
n = number of e- transferred
Q= reaction quotient = [products]/[reactants] 


Let’s first determine how many electrons were transferred in the reaction by separating the two half-reactions:

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Problem Details

Consider this reaction.

Sn2+ (aq) + 2 Fe3+ (aq) → Sn4+ (aq) + 2 Fe2+ (aq)     E° = 0.617 V

What is the value of E when [Sn2+] and {Fe3+] are equal to 0.50 M and [Sn4+] and [Fe2+] are equal to 0.10 M?

(A) 0.069V

(B) 0.679 V

(C) 0.658 V

(D) 0.576

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