Agalvanic cell is powered by the following redox reaction: 2fe+3(aq) + h2 (g) + 2oh−(aq) → 2fe+2 (aq) + 2h2o (l)answer the following questions about this cell. if you need any electrochemical data, be sure you get it from the aleks data tab. write a balanced equation for the half-reaction that takes place at the cathode. write a balanced equation for the half-reaction that takes place at the anode. calculate the cell voltage under standard conditions. =e0v

Anode: H₂(g) + 2 OH⁻(aq) → 2 H₂O(l) + 2 e⁻

Cathode: 2 Fe⁺³(aq) + 2 e⁻ → 2 Fe⁺²(aq)

E° = 1.60 V

Explanation:

Let's consider the reaction taking place in a galvanic cell.

2 Fe⁺³(aq) + H₂(g) + 2 OH⁻(aq) → 2 Fe⁺²(aq) + 2 H₂O(l)

The corresponding half-reactions are:

Anode (oxidation): H₂(g) + 2 OH⁻(aq) → 2 H₂O(l) + 2 e⁻   E°red = - 0.83 V

Cathode (reduction): 2 Fe⁺³(aq) + 2 e⁻ → 2 Fe⁺²(aq)        E°red = 0.77 V

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

E° = E°red, cat - E°red, an = 0.77 V - (-0.83 V) = 1.60 V