The standard cell potential (e°cell) for the voltaic cell based on the reaction below is v. sn2+ (aq) + 2fe3+ (aq) → 2fe2+ (aq) + sn4+ (aq) the standard cell potential (e°cell) for the voltaic cell based on the reaction below is v. sn2+ (aq) + 2fe3+ (aq) 2fe2+ (aq) + sn4+ (aq) +1.39 +1.21 +0.46 -0.46 +0.617

The standard cell potential (E°cell) for the voltaic cell based on the reaction below is 0.64 V.

Explanation:

Let's consider the following redox reaction.

Sn²⁺(aq) + 2 Fe³⁺(aq) → 2 Fe²⁺(aq) + Sn⁴⁺(aq)

We can recognize the following half-reactions.

Cathode (reduction): 2 Fe³⁺(aq) + 2 e⁻ → 2 Fe²⁺(aq)    E°red = 0.77 V

Anode (oxidation): Sn²⁺(aq) → Sn⁴⁺(aq) + 2 e⁻              E°red = 0.13 V

The standard cell potential (E°cell) is the difference between the standard reduction potential of the cathode and the standard reduction potential of the anode.

E°cell = E°red, cat - E°red, an = 0.77 V - 0.13 V = 0.64 V