What is the balanced redox equation for the voltaic cell? Answer is A) 2 Fe2+(aq) + Cl2(g) \rightarrow → 2 Fe3+(aq) + 2 Cl−(aq)B) 2 Fe3+(aq) + 2 Cl−(aq) \rightarrow → 2 Fe2+(aq) + Cl2(g)C) Fe2+(aq) + Cl2(g) \rightarrow → Fe3+(aq) + Cl−(aq)D) Fe3+(aq) + Cl−(aq) \rightarrow → Fe2+(aq) + Cl2(g)E) None of the above is correct, because neither C(s) not Pt(s) appears in any of them.

Option (A) is the correct answer.

Explanation:

Balanced redox reaction for the given reaction is as follows.

At anode, oxidation reaction will take place as follows.

Oxidation:

Multiplying this equation with 2, in order to balance it.

At cathode, reduction will take place as follows.

Therefore, the correct balanced redox equation for the voltaic cell is as follows.

the answer is b & c i believe : )