What is the total number of moles (n) of electrons exchanged between the oxidizing agent and the reducing agent in the reaction below to obtain vanadium metal
V₂O₅(s) + 5Ca(l) $\rarr$ 2V(l) + 5CaO(s)

Question

What is the total number of moles (n) of electrons exchanged between the oxidizing agent and the reducing agent in the reaction below to obtain vanadium metal
V₂O₅(s) + 5Ca(l)

\rarr

2V(l) + 5CaO(s)

Quizplus · Accepted Answer

In the given reaction, vanadium is reduced from an oxidation state of +5 in $V_2O_5$ to 0 in $V$, and calcium is oxidized from 0 in $Ca$ to +2 in $CaO$. Each vanadium atom gains 5 electrons to reduce, and there are 2 vanadium atoms, so a total of $2 \times 5 = 10$ electrons are exchanged.

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

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