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slega [8]
4 years ago
13

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.
Chemistry
1 answer:
kicyunya [14]4 years ago
8 0

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)

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