---
title: "In an experiment, permanganate ions react with oxalate ions in an acidic aqueous solution according to the unbalanced skeleton equation below.  \\[ \\text{MnO}_4^-\\text{(aq)} + \\text{C}_2\\text{O}_4^{2-}\\text{(aq)} + \\text{H}^+\\text{(aq)} \\rightarrow \\text{Mn}^{2+}\\text{(aq)} + \\text{CO}_2\\text{(g)} + \\text{H}_2\\text{O(l)} \\]  When this oxidation-reduction reaction is balanced using the smallest whole-number coefficients, what is the total number of electrons transferred in the balanced equation?"
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url: "https://nerd-notes.com/ubq/119855/"
date_modified: "2026-08-21T08:16:22+00:00"
---

# In an experiment, permanganate ions react with oxalate ions in an acidic aqueous solution according to the unbalanced skeleton equation below.

\[ \text{MnO}_4^-\text{(aq)} + \text{C}_2\text{O}_4^{2-}\text{(aq)} + \text{H}^+\text{(aq)} \rightarrow \text{Mn}^{2+}\text{(aq)} + \text{CO}_2\text{(g)} + \text{H}_2\text{O(l)} \]

When this oxidation-reduction reaction is balanced using the smallest whole-number coefficients, what is the total number of electrons transferred in the balanced equation?

In an experiment, permanganate ions react with oxalate ions in an acidic aqueous solution according to the unbalanced skeleton equation below.

\[ \text{MnO}_4^-\text{(aq)} + \text{C}_2\text{O}_4^{2-}\text{(aq)} + \text{H}^+\text{(aq)} \rightarrow \text{Mn}^{2+}\text{(aq)} + \text{CO}_2\text{(g)} + \text{H}_2\text{O(l)} \]

When this oxidation-reduction reaction is balanced using the smallest whole-number coefficients, what is the total number of electrons transferred in the balanced equation?

- **A.** \(2\)
- **B.** \(5\)
- **C.** \(10\)
- **D.** \(20\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119855/*