Justify that the reaction
`2Cu_(2)O_(s)+Cu_(2)S(s)rarr6Cu(s)+SO_(2)(g)` a redox reaction. Identify the species oxidised`//`reduced. Which acts as an oxidanat and which acts as a reductant?

Options

A. If both assertion and reason are true and reason is the correct explanation of assertion.
B. If both assertion and reason are true but reason is not the correct explanation of assertion.
C. If assertion is true but reason is false.
D. If both assertion and reason are false.

Explanation

To determine whether the reaction

\[ 2 \text{Cu}_2\text{O (s)} + \text{Cu}_2\text{S (s)} \rightarrow 6 \text{Cu (s)} + \text{SO}_2 \text{(g)} \]

is a redox reaction, we need to analyze the oxidation states of the elements involved.

### Step 1: Identify the oxidation states of each element in the reactants and products.

1. **Copper in Cu2O:**
- Let the oxidation state of Cu be \( x \).
- The equation for Cu2O is: \( 2x + (-2) = 0 \) (since the compound is neutral).
- Solving gives \( 2x = 2 \) → \( x = +1 \).
- Therefore, the oxidation state of Cu in Cu2O is \( +1 \).

2. **Sulfur in Cu2S:**
- Let the oxidation state of S be \( y \).
- The equation for Cu2S is: \( 2(+1) + y = 0 \).
- Solving gives \( 2 + y = 0 \) → \( y = -2 \).
- Therefore, the oxidation state of S in Cu2S is \( -2 \).

3. **Copper in the product (Cu):**
- In elemental form, the oxidation state of Cu is \( 0 \).

4. **Sulfur in SO2:**
- Let the oxidation state of S in SO2 be \( z \).
- The equation for SO2 is: \( z + 2(-2) = 0 \).
- Solving gives \( z - 4 = 0 \) → \( z = +4 \).
- Therefore, the oxidation state of S in SO2 is \( +4 \).

### Step 2: Determine changes in oxidation states.

- **Sulfur:**
- Changes from \( -2 \) (in Cu2S) to \( +4 \) (in SO2).
- This is an increase in oxidation state, indicating that sulfur is **oxidized**.

- **Copper:**
- Remains \( +1 \) (in Cu2O) and goes to \( 0 \) (in elemental Cu).
- This is a decrease in oxidation state, indicating that copper is **reduced**.

### Step 3: Identify the oxidizing and reducing agents.

- **Oxidizing Agent:** The species that is reduced (gains electrons) is the oxidizing agent. Here, copper (Cu) is reduced from \( +1 \) to \( 0 \), so it acts as the **oxidizing agent**.

- **Reducing Agent:** The species that is oxidized (loses electrons) is the reducing agent. Here, sulfur (S) is oxidized from \( -2 \) to \( +4 \), so it acts as the **reducing agent**.

### Conclusion

The reaction is a redox reaction because:
- Sulfur is oxidized (loses electrons) and acts as a reducing agent.
- Copper is reduced (gains electrons) and acts as an oxidizing agent.

### Summary:
- **Oxidized Species:** Sulfur (S)
- **Reduced Species:** Copper (Cu)
- **Oxidizing Agent:** Copper (Cu)
- **Reducing Agent:** Sulfur (S)