Chapter 17: Problem 56

Using half-reactions, balance the redox equation of \(\mathrm{Zn}(s)\) and \(\mathrm{Fe}^{3+}(a q)\) reacting to form \(\mathrm{Zn}^{2+}(a q)\) and \(\mathrm{Fe}^{2+}(a q) .\)

Short Answer

Expert verified

The balanced redox equation for the reaction of zinc with iron (III) to form zinc ions and iron (II) is \(\text{Zn}(s) + 2\text{Fe}^{3+}(aq) \rightarrow \text{Zn}^{2+}(aq) + 2\text{Fe}^{2+}(aq)\)

Step by step solution

Writing down the Half-Reactions

The given redox reaction should be divided into two half-reactions, one for reduction and one for oxidation: \[ \text{Zn}(s)\rightarrow \text{Zn}^{2+}(aq)+2e^- \]\[ \text{Fe}^{3+}(aq)+e^- \rightarrow \text{Fe}^{2+}(aq) \]

Balancing Half-Reactions

In order to balance the redox equation, the number of electrons in the half reactions must be equal. The oxidation half-reaction already has 2 electrons and the reduction half-reaction has 1 electron, therefore the reduction half-reaction must be multiplied by 2 to balance the electrons: \[ 2\left[\text{Fe}^{3+}(aq)+e^- \rightarrow \text{Fe}^{2+}(aq)\right] \] Now both half reactions involve the transfer of 2 electrons.

Combining the Half-Reactions

Put the two half-reactions together and confirm that electrons will cancel out to make the overall balanced equation: \[\text{Zn}(s) + 2\text{Fe}^{3+}(aq) \rightarrow \text{Zn}^{2+}(aq) + 2\text{Fe}^{2+}(aq)\]

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Using half-reactions, balance the redox equation of \(\mathrm{Zn}(s)\) and \(\mathrm{Fe}^{3+}(a q)\) reacting to form \(\mathrm{Zn}^{2+}(a q)\) and \(\mathrm{Fe}^{2+}(a q) .\)

Short Answer

Step by step solution

Writing down the Half-Reactions

Balancing Half-Reactions

Combining the Half-Reactions

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