What is the total number of moles (n) of electrons exchanged between the oxidizing agent and the reducing agent in the overall redox equation: Cr₂O₇^2-(aq) + 6Fe²⁺(aq) + 14H⁺(aq) $\rarr$ 2Cr³⁺(aq) + 6Fe³⁺(aq) + 7H₂O(l)

Question

Quizplus · Accepted Answer

In the given redox reaction, each Cr in Cr2O7^2- is reduced from +6 to +3, gaining 3 electrons per Cr atom. Since there are 2 Cr atoms, a total of 6 electrons are gained. Each Fe^2+ is oxidized to Fe^3+, losing 1 electron per Fe atom. With 6 Fe^2+ ions, a total of 6 electrons are lost. Therefore, 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 $\rarr$