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 can be broken down into the following half-reactions:

Cu2+(aq) + 2e- → Cu(s)         Reduction (Gain of Electrons)
Zn(s) → Zn2+(aq) + 2e-         Oxidation (Loss of Electrons)

In this reaction, zinc is oxidized (loses electrons) and copper(II) ion is reduced (gains electrons).

Since copper(II) ion is a stronger oxidizing agent than zinc, it tends to gain electrons more readily and is therefore reduced more easily. As a result, the direction favored is the forward reaction:

Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq)

Which of the Following Is the Correct Net Ionic Equation