Iven the balanced equation representing a reaction: mg(s) + ni2+(aq) → mg2+(aq) + ni(s) what is the total number of moles of electrons lost by mg(s) when 2.0 moles of electrons are gained by ni2+(aq)?
This is a redox reaction where oxidation and reduction take place. Here, Mg(s) oxidizes into Mg²⁺(aq) by increasing oxidation number from 0 to +2 while Ni²⁺(aq) reduces into Ni(s) by decreasing oxidation number from +2 to 0.
Oxidation Mg(s) → Mg²⁺(aq) + 2 e
Reduction Ni²⁺(aq) + 2 e → Ni(s)
Hence, 2.0 moles of electrons lost by Mg(s) when 2.0 moles of electrons are gained by Ni²⁺(aq).
