What is the total number of moles (n) of electrons exchanged between the oxidizing agent and the reducing agent in the overall redox equation: 3C₂O₄^2-(aq) + Cr₂O₇^2-(aq) + 14H⁺(aq) $\rarr$ 6CO₂(g) + 2Cr³⁺(aq) + 7H₂O(l)

Question

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In the balanced redox reaction, each C2O4^2- loses 2 electrons, and there are 3 C2O4^2- ions, totaling 6 electrons lost. The Cr2O7^2- gains 6 electrons to form 2 Cr^3+. Thus, 6 moles of electrons are exchanged.

What Is the Total Number of Moles (N) of Electrons →\rarr→

What Is the Total Number of Moles (N) of Electrons $\rarr$