Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s)| Cu²⁺(aq)|| Mn²⁺(aq)| Mn(s) A) 2 Cu(s)+ Mn²⁺(aq)→ Mn(s)+ 2 Cu²⁺(aq) B) Cu(s)+ Cu²⁺(aq)→ Mn(s)+ Mn²⁺(aq) C) Cu(s)+ Mn²⁺(aq)→ Mn(s)+ Cu²⁺(aq) D) 2 Mn(s)+ Cu²⁺(aq)→ Cu(s)+ 2Mn²⁺(aq) E) Mn(s)+ Cu²⁺(aq)→ Cu(s)+ Mn²⁺(aq)

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Quizplus · Accepted Answer

The cell notation shows the reactants and products in the half-cells. The left half-cell has copper metal and copper sulfate solution, while the right half-cell has manganese metal and manganese sulfate solution. The anode reaction (left half-cell) is oxidation of copper metal to Cu2+ ions, which react with sulfate ions to form CuSO4 solution. The cathode reaction (right half-cell) is reduction of Mn2+ ions to manganese metal. The net ionic equation for the entire reaction is Cu(s) + Mn2+(aq) → Cu2+(aq) + Mn(s). However, the given answer choices have different combinations of reactants and products. Among them, choice C represents the net ionic equation after cancelling out the spectator ions (SO42- and Na+ if present) and putting the remaining ions in the correct products and reactants. Therefore, choice C is the best choice.

Write a Balanced Net Ionic Equation for the Overall Reaction