1.0 lit of `CO_(2)` is passed over hot coke. The volume becomes 1.4 lit. The composition of products is

Options

A. 0.6 lit CO
B. 0.8 lit `CO_(2)`
C. 0.6 lit `CO_(2)` and 0.8 lit `CO`
D. 1.2 lit `CO_(2)`

Explanation

To solve the problem, we need to analyze the reaction between carbon dioxide (CO₂) and coke (which is primarily carbon, C) when heated. The reaction can be represented as follows:

1. **Identify the Reaction**:
The reaction between carbon dioxide and carbon (coke) produces carbon monoxide (CO):
\[ \text{CO}_2 + \text{C} \rightarrow 2\text{CO} \]

2. **Set Up the Initial and Final Volumes**:
- Initial volume of CO₂ = 1.0 L
- Final volume after the reaction = 1.4 L

3. **Define Variables**:
Let \( A \) be the volume of CO₂ that reacts. After the reaction:
- Volume of CO₂ remaining = \( 1 - A \)
- Volume of CO produced = \( 2A \)

4. **Write the Volume Balance Equation**:
The total volume after the reaction can be expressed as:
\[ \text{Final Volume} = \text{Volume of remaining CO}_2 + \text{Volume of CO produced} \]
So, we have:
\[ 1 - A + 2A = 1.4 \]

5. **Simplify the Equation**:
Combine like terms:
\[ 1 + A = 1.4 \]

6. **Solve for A**:
Subtract 1 from both sides:
\[ A = 1.4 - 1 = 0.4 \]

7. **Calculate the Volumes of Products**:
- Volume of CO₂ remaining = \( 1 - A = 1 - 0.4 = 0.6 \) L
- Volume of CO produced = \( 2A = 2 \times 0.4 = 0.8 \) L

8. **Conclusion**:
The composition of the products is:
- Volume of CO₂ = 0.6 L
- Volume of CO = 0.8 L

Thus, the final answer is:
- CO₂: 0.6 L
- CO: 0.8 L