Which of the following is the correct net ionic equation for the redox reaction between zinc and the copper(II) ion and the correct direction that is favored? The half-reactions are:
Cu²⁺ + 2 e^- Cu(s)
Zn²⁺ + 2 e^- Zn(s)
Cu²⁺ is a stronger oxidizing agent than Zn²⁺.

Question

Which of the following is the correct net ionic equation for the redox reaction between zinc and the copper(II) ion and the correct direction that is favored? The half-reactions are:
Cu²⁺ + 2 e^-

Cu(s)
Zn²⁺ + 2 e^-

Zn(s)
Cu²⁺ is a stronger oxidizing agent than Zn²⁺.

Quizplus · Accepted Answer

The correct net ionic equation is Cu2+(aq) + Zn(s) --> Cu(s) + Zn2+(aq). This is because copper(II) ion acts as the oxidizing agent and zinc acts as the reducing agent. In other words, copper(II) ion gains electrons (is reduced) and zinc loses electrons (is oxidized). Choice B is the correct one because it shows the correct products and direction of the reaction, with copper(II) ion being reduced and zinc being oxidized.

Which of the Following Is the Correct Net Ionic Equation