In the reaction
`MnO_(2) + 4HC1 to MnC1_(2) + C1_(2) + 2H_(2)O`
the substance getting reduced is

Options

A. `MnO_(2)`
B. HC1
C. `MnC1_(2)`
D. `C1_(2)`

Answer

To determine which substance is getting reduced in the reaction:

\[ \text{MnO}_2 + 4\text{HCl} \rightarrow \text{MnCl}_2 + \text{Cl}_2 + 2\text{H}_2\text{O} \]

we will follow these steps:

### Step 1: Identify the oxidation states of the elements in the reactants and products.
- In **MnO₂**:
- Oxygen (O) has an oxidation state of -2.
- Let the oxidation state of manganese (Mn) be \( x \).
- The equation becomes: \( x + 2(-2) = 0 \) → \( x - 4 = 0 \) → \( x = +4 \).

- In **HCl**:
- Hydrogen (H) has an oxidation state of +1 and Chlorine (Cl) has an oxidation state of -1.

- In **MnCl₂**:
- Let the oxidation state of manganese (Mn) be \( y \).
- The equation becomes: \( y + 2(-1) = 0 \) → \( y - 2 = 0 \) → \( y = +2 \).

- In **Cl₂**:
- Chlorine (Cl) in its elemental form has an oxidation state of 0.

- In **H₂O**:
- Hydrogen (H) has an oxidation state of +1 and Oxygen (O) has an oxidation state of -2.

### Step 2: Compare the oxidation states before and after the reaction.
- For **Mn**:
- In MnO₂, Mn is +4.
- In MnCl₂, Mn is +2.
- The oxidation state of Mn decreases from +4 to +2, indicating that Mn is being reduced.

- For **Cl**:
- In HCl, Cl is -1.
- In Cl₂, Cl is 0.
- The oxidation state of Cl increases from -1 to 0, indicating that Cl is being oxidized.

### Step 3: Conclusion
Since the oxidation state of manganese decreases from +4 to +2, manganese is the substance that is getting reduced in this reaction.

### Final Answer:
The substance getting reduced is **MnO₂** (Manganese).

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