AP Chemistry
4.9 Oxidation-Reduction (Redox) Reactions
4.2 Net Ionic Equations
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?
\[ \text{MnO}_4^-\text{(aq)} + \text{C}_2\text{O}_4^{2-}\text{(aq)} + \text{H}^+\text{(aq)} \rightarrow \text{Mn}^{2+}\text{(aq)} + \text{CO}_2\text{(g)} + \text{H}_2\text{O(l)} \]
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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