Question

Balancing Oxidation-Reduction Reactions 1. Assign oxidation numbers. 2. Separate into oxidation and reduction half reactions. 3. Balance each half reaction using the following steps: a. Balance all elements except oxygen or hydrogen. b. Balance oxygen by adding H20. c. Balance hydrogen by adding H*. d. Balance charge by adding electrons: Electrons go on the RIGHT (product side) for OXIDATION reactions. Electrons go on the LEFT (reactant side) for REDUCTION reactions. e. In BASIC solution, do this additional step: For every H", add OH to BOTH sides of the reaction. Combine H* + OH into H20. Cancel out any waters that appear on both sides. You should now have a balanced half reaction. 4. Multiply balanced half reactions so an equal number of electrons are consumed and produced. 5. Add together half reactions. 6. Clean up. Combine identical substances and reduce coefficients to the lowest terms. 7. CHECK! Atom and charge must balance.

1. 2. 3.

Answer 1

2 Both - 2a Bry by 0 à oxidised 2 Gray 3 MOH) 2 Gr (1) y 3 Mno Cro?- oxidising agent. 24g + 12th 2A + 2 Hgo Hgo is reduced