Balancing Equations
Cu (s) + Ag+ (aq) ? Cu2+ (aq) + Ag (s)
Step 3: Multiply each half-reaction by a factor that makes the reducing agent supply as many electrons as the oxidizing agent requires - ELECTRON TRANSFER NUMBER (2 here)
Oxidation (Reducing agent) Cu ? Cu2+ + 2e-
Reduction (Oxidizing agent) 2 Ag+ + 2 e- ? 2 Ag
Step 4: Add half-reactions to give the overall equation.
Cu (s) + 2 Ag+ (aq) ? Cu2+ (aq) + 2Ag (s)
How to balance for both charge and mass ?
Step 1: Identify the oxidation and reduction HALF-REACTIONS:
Step 2: Balance each HALF-REACTION for charge and mass (done)