5.6 litres of methane gas (`CH_(4)`) is ignited in oxygen gas. Calculate the number of moles of `CO_(2)` formed.

Options

A. 25
B. 0.25
C. 0.30
D. 50

Explanation

To solve the problem of calculating the number of moles of carbon dioxide (CO₂) formed from the combustion of 5.6 liters of methane (CH₄), we can follow these steps:

### Step-by-Step Solution:

1. **Write the Balanced Chemical Equation:**
The combustion of methane in oxygen can be represented by the following balanced equation:
\[ \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \]
From this equation, we see that 1 mole of CH₄ produces 1 mole of CO₂.

2. **Determine the Volume of 1 Mole of Gas:**
At standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 liters.

3. **Calculate the Moles of CH₄:**
To find out how many moles of CH₄ are present in 5.6 liters, we use the relationship:
\[ \text{Moles of CH}_4 = \frac{\text{Volume of CH}_4}{\text{Volume of 1 mole of gas}} = \frac{5.6 \text{ L}}{22.4 \text{ L/mol}} = 0.25 \text{ moles} \]

4. **Calculate the Moles of CO₂ Produced:**
From the balanced equation, we know that 1 mole of CH₄ produces 1 mole of CO₂. Therefore, the moles of CO₂ produced will be equal to the moles of CH₄ consumed:
\[ \text{Moles of CO}_2 = \text{Moles of CH}_4 = 0.25 \text{ moles} \]

### Final Answer:
The number of moles of CO₂ formed is **0.25 moles**.

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