The reaction `2PbS + 3O_(2) rarr 2PbO + 2SO_(2)` used is the extractive metallurgy of lead is called

Options

A. Roasting
B. Cupellation
C. Smelting
D. Calcination

Explanation

To solve the question regarding the reaction `2PbS + 3O_(2) → 2PbO + 2SO_(2)` and to identify the process used in the extractive metallurgy of lead, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reaction**: The given reaction is `2PbS + 3O_(2) → 2PbO + 2SO_(2)`. Here, lead sulfide (PbS) reacts with oxygen (O₂) to produce lead oxide (PbO) and sulfur dioxide (SO₂).

2. **Understand the Process**: The reaction involves the conversion of a sulfide ore (PbS) into an oxide (PbO) by heating it in the presence of oxygen. This is a key characteristic of a specific metallurgical process.

3. **Define Roasting**: In metallurgy, the process of converting sulfide ores into oxides by heating in the presence of oxygen is known as roasting. This process is commonly used for sulfide ores such as lead sulfide (PbS) and zinc sulfide (ZnS).

4. **Differentiate from Other Processes**:
- **Calcination**: This process involves the thermal decomposition of carbonates, not sulfides.
- **Smelting**: This is the reduction of metal oxides to metals, typically using carbon, and does not apply here as we are not reducing an oxide.
- **Cupellation**: This is a refining process used for precious metals and is not relevant to the conversion of sulfides to oxides.

5. **Conclusion**: Since the reaction involves the conversion of lead sulfide to lead oxide through heating in the presence of oxygen, it is classified as roasting.

### Final Answer:
The process used in the extractive metallurgy of lead for the reaction `2PbS + 3O_(2) → 2PbO + 2SO_(2)` is called **Roasting**.

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