The unbalanced reaction is:
This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Here's how to balance the redox reaction in acidic medium:
The unbalanced reaction is:
$$\text{Fe} + \text{ClO}_3^- \rightarrow \text{Fe}^{3+} + \text{Cl}^-$$
Step 1: Separate the reaction into half-reactions.
Oxidation half-reaction:
$$\text{Fe} \rightarrow \text{Fe}^{3+}$$
Reduction half-reaction:
$$\text{ClO}_3^- \rightarrow \text{Cl}^-$$
Step 2: Balance atoms other than oxygen and hydrogen.
Both Fe and Cl atoms are already balanced in their respective half-reactions.
Step 3: Balance oxygen atoms by adding $\text{H}_2\text{O}$.
Oxidation:
$$\text{Fe} \rightarrow \text{Fe}^{3+}$$
Reduction:
$$\text{ClO}_3^- \rightarrow \text{Cl}^- + 3\text{H}_2\text{O}$$
Step 4: Balance hydrogen atoms by adding $\text{H}^+$ (since it's an acidic medium).
Oxidation:
$$\text{Fe} \rightarrow \text{Fe}^{3+}$$
Reduction:
$$6\text{H}^+ + \text{ClO}_3^- \rightarrow \text{Cl}^- + 3\text{H}_2\text{O}$$
Step 5: Balance the charge by adding electrons ($\text{e}^-$).
Oxidation:
$$\text{Fe} \rightarrow \text{Fe}^{3+} + 3\text{e}^-$$
Reduction:
$$6\text{H}^+ + \text{ClO}_3^- + 6\text{e}^- \rightarrow \text{Cl}^- + 3\text{H}_2\text{O}$$
Step 6: Make the number of electrons equal in both half-reactions.
Multiply the oxidation half-reaction by 2 to get 6 electrons:
$$2(\text{Fe} \rightarrow \text{Fe}^{3+} + 3\text{e}^-)$$
$$2\text{Fe} \rightarrow 2\text{Fe}^{3+} + 6\text{e}^-$$
The reduction half-reaction remains:
$$6\text{H}^+ + \text{ClO}_3^- + 6\text{e}^- \rightarrow \text{Cl}^- + 3\text{H}_2\text{O}$$
Step 7: Add the two balanced half-reactions and cancel out common species (electrons).
$$2\text{Fe} + 6\text{H}^+ + \text{ClO}_3^- + 6\text{e}^- \rightarrow 2\text{Fe}^{3+} + 6\text{e}^- + \text{Cl}^- + 3\text{H}_2\text{O}$$
Step 8: Write the final balanced equation.
$$2\text{Fe} + \text{ClO}_3^- + 6\text{H}^+ \rightarrow 2\text{Fe}^{3+} + \text{Cl}^- + 3\text{H}_2\text{O}$$
The balanced equation is:
$$\boxed{2\text{Fe} + \text{ClO}_3^- + 6\text{H}^+ \rightarrow 2\text{Fe}^{3+} + \text{Cl}^- + 3\text{H}_2\text{O}}$$
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