Balancing Redox Equations
Assign oxidation numbers (o.n.) to atoms and write a net ionic equation for each half
reaction. Work on each half
2. Balance atoms being oxidized or reduced.
3. From the change in oxidation numbers, determine the number of electrons involved and add them to the high oxidation number side of the equation.
4. Balance the charge, using either H+ (if in ACID solution) or OH- (if in BASE solution).
5. Now balance the OXYGEN by adding H2O to the appropriate side of the equation.
Check that everything balances - it will!
6. Equalize the number of electrons in each half reaction by multiplying by the appropriate factor and then add.
|In acid solution, potassium
permanganate can oxidize chloride ions to chlorine gas. The
manganese-containing product in this reaction is
Mn2+(aq). Balance the equation for this reaction.
2Cl-(aq) -----> Cl2(aq)
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