Describe the oxidizing action of with the following. `K_(2) Cr_(2) O_(7)`Write ionic equations for its reaction (acidic medium) with :
`H_(2) S`

Explanation

To describe the oxidizing action of \( K_2Cr_2O_7 \) (potassium dichromate) in an acidic medium with \( H_2S \) (hydrogen sulfide), we will follow these steps to derive the balanced ionic equation.

### Step 1: Identify the Oxidation States
In \( K_2Cr_2O_7 \), the oxidation state of chromium (Cr) is +6, and in \( H_2S \), the oxidation state of sulfur (S) is -2. During the reaction, chromium will be reduced, and sulfur will be oxidized.

### Step 2: Write the Half-Reactions
1. **Reduction Half-Reaction**:
\[
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