Question

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.

Answer 1

Answer: 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: $Fe^{2+}(aq) \rightarrow Fe^{3+}(aq) + 1e^{-}$

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

    $2Fe^{2+}(aq) \rightarrow 2Fe^{3+}(aq) + 2e^{-}$

At cathode, reduction will take place as follows.

   $Cl_{2}(g) + 2e^{-} \rightarrow 2Cl^{-}(aq)$

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

     $2Fe^{2+}(aq) + Cl_{2}(g) \rightarrow 2Fe^{3+}(aq) + 2Cl^{-}(aq)$