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title: "A water-treatment chemist evaluates several reactions involving manganese species. In a comproportionation reaction, reactant species containing the same element at different oxidation states form a product in which that element has a common intermediate oxidation state. Which of the following balanced net ionic equations represents comproportionation of manganese?"
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url: "https://nerd-notes.com/ubq/120047/"
date_modified: "2026-08-21T08:40:56+00:00"
---

# A water-treatment chemist evaluates several reactions involving manganese species. In a comproportionation reaction, reactant species containing the same element at different oxidation states form a product in which that element has a common intermediate oxidation state. Which of the following balanced net ionic equations represents comproportionation of manganese?

A water-treatment chemist evaluates several reactions involving manganese species. In a comproportionation reaction, reactant species containing the same element at different oxidation states form a product in which that element has a common intermediate oxidation state. Which of the following balanced net ionic equations represents comproportionation of manganese?

- **A.** \[3\text{MnO}_4^{2-}\text{(aq)}+4\text{H}^{+}\text{(aq)}\rightarrow2\text{MnO}_4^{-}\text{(aq)}+\text{MnO}_2\text{(s)}+2\text{H}_2\text{O(l)}\]
- **B.** \[2\text{MnO}_4^{-}\text{(aq)}+5\text{H}_2\text{O}_2\text{(aq)}+6\text{H}^{+}\text{(aq)}\rightarrow2\text{Mn}^{2+}\text{(aq)}+5\text{O}_2\text{(g)}+8\text{H}_2\text{O(l)}\]
- **C.** \[2\text{MnO}_4^{-}\text{(aq)}+3\text{Mn}^{2+}\text{(aq)}+2\text{H}_2\text{O(l)}\rightarrow5\text{MnO}_2\text{(s)}+4\text{H}^{+}\text{(aq)}\]
- **D.** \[\text{Mn}^{2+}\text{(aq)}+2\text{OH}^{-}\text{(aq)}\rightarrow\text{Mn(OH)}_2\text{(s)}\]

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