`Cr_(2) O_(7)^(2-) + C_(2) O_(4)^(2-) + H^(+) = Cr^(3+) + CO_(2) + H_(2) O`

Explanation

To balance the given redox reaction in acidic medium, we will follow these steps:

### Step 1: Identify the oxidation and reduction half-reactions.
In the reaction:
\[ \text{Cr}_2\text{O}_7^{2-} + \text{C}_2\text{O}_4^{2-} + \text{H}^+ \rightarrow \text{Cr}^{3+} + \text{CO}_2 + \text{H}_2\text{O} \]

- **Oxidation half-reaction**: The oxidation state of carbon in oxalate (\( \text{C}_2\text{O}_4^{2-} \)) is +3, and it is oxidized to carbon dioxide (\( \text{CO}_2 \)), where the oxidation state of carbon is +4.

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