For the redox reaction

The correct coefficients of the reactants for the balanced equation are
| | | | |
| :--- | :--- | :--- | :--- |
| (1) |16 | 5 | 2 |
| (2) | 2 | 5 | 16 |
| (3) | 5 | 16 | 2 |

Question

For the redox reaction

The correct coefficients of the reactants for the balanced equation are
| |  |  |  |
| :--- | :--- | :--- | :--- |
| (1) |16 | 5 | 2 |
| (2) | 2 | 5 | 16 |
| (3) | 5 | 16 | 2 |
| (4) | 2 | 16 | 5 |

Canvas Classes · Accepted Answer

🧠 The Ion-Electron Balance
Balancing a redox reaction is like bookkeeping. The total number of electrons "lost" by the reducer must exactly match the electrons "gained" by the oxidizer.

🗺️ The Quantitative Balancing
1. Reduction Half-Reaction:
    (+7) goes to  (+2).
   Change  per .
2. Oxidation Half-Reaction:
    (each C is +3) goes to  (each C is +4).
   Change  per oxalate ion.
3. Equalizing Electrons: 
   To match  and , we use a common multiple of .
   - Multiply  by 2.
   - Multiply  b

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