Write a balanced chemical equation for the overall reaction represented by the cell notation below.Mn(s)| Mn²⁺(aq)|| Zn²⁺(aq)| Zn(s) A) 2Mn(s)+ Zn²⁺(aq)$\to$ Zn(s)+ 2Mn²⁺(aq) B) Mn(s)+ Mn²⁺(aq)$\to$ Zn(s)+ Zn²⁺(aq) C) Mn(s)+ Zn²⁺(aq)$\to$ Zn(s)+ Mn²⁺(aq) D) 2Zn(s)+ Mn²⁺(aq)$\to$Mn(s)+ 2Zn²⁺(aq) E) Zn(s)+ Mn²⁺(aq)$\to$Mn(s)+ Zn²⁺(aq)

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The notation consists of two half-reactions, one at each electrode separated by ||. The half-reactions can be written as: Mn(s) → Mn²⁺(aq) + 2e- (oxidation at anode) Zn²⁺(aq) + 2e- → Zn(s) (reduction at cathode) To get the overall reaction, these two half-reactions are added together after multiplying the oxidation half-reaction by 1 and the reduction half-reaction by 2: Mn(s) + Zn²⁺(aq) → Zn(s) + Mn²⁺(aq)

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