In the reaction `MnO_(2)+4 HCIrarr MnCI_(2) +CI_(2)+2H_(2)O` which species is oxidised

Explanation

To determine which species is oxidized in the reaction \( \text{MnO}_2 + 4 \text{HCl} \rightarrow \text{MnCl}_2 + \text{Cl}_2 + 2 \text{H}_2\text{O} \), we will analyze the oxidation states of the elements involved in the reaction.

### Step-by-Step Solution:

1. **Identify the oxidation states of manganese (Mn) in MnO2 and MnCl2:**
- In \( \text{MnO}_2 \), oxygen has an oxidation state of -2. Since there are two oxygen atoms, the total contribution from oxygen is \( 2 \times (-2) = -4 \). Therefore, to balance this, manganese must have an oxidation state of +4.
- In \( \text{MnCl}_2 \), chlorine has an oxidation state of -1. With two chlorine atoms, the total contribution from chlorine is \( 2 \times (-1) = -2 \). Therefore, manganese must have an oxidation state of +2 to balance this, as \( +2 + (-2) = 0 \).

...