If 5 ml of methane is completely burnt the volume of oxygen required and the volume of `CO_(2)` formed under the same conditions are

Options

A. 5 ml, 10 ml
B. 10 ml, 5 ml
C. 5 ml, 15 ml
D. 10 ml, 10 ml

Explanation

To solve the problem of determining the volume of oxygen required and the volume of carbon dioxide formed when 5 ml of methane is completely burnt, we can follow these steps:

### Step-by-Step Solution:

1. **Write the Balanced Chemical Equation**:
The combustion of methane (CH₄) in the presence of oxygen (O₂) can be represented by the following balanced equation:
\[ \text{CH}_4 + 2 \text{O}_2 \rightarrow \text{CO}_2 + 2 \text{H}_2\text{O} \]
This equation shows that 1 mole of methane reacts with 2 moles of oxygen to produce 1 mole of carbon dioxide and 2 moles of water.

2. **Determine the Volume of Oxygen Required**:
According to the balanced equation, for every 1 mole of methane, 2 moles of oxygen are required. Since the volumes of gases at the same temperature and pressure are directly proportional to the number of moles, we can say:
- Volume of O₂ required = 2 × Volume of CH₄
- Given that the volume of CH₄ is 5 ml:
\[ \text{Volume of O}_2 = 2 \times 5 \, \text{ml} = 10 \, \text{ml} \]

3. **Determine the Volume of Carbon Dioxide Formed**:
From the balanced equation, we see that for every 1 mole of methane burned, 1 mole of carbon dioxide is produced. Therefore:
- Volume of CO₂ produced = Volume of CH₄
- Given that the volume of CH₄ is 5 ml:
\[ \text{Volume of CO}_2 = 5 \, \text{ml} \]

### Final Answer:
- Volume of Oxygen required = 10 ml
- Volume of Carbon Dioxide formed = 5 ml