1.2 L of hydrogen and 1.12 L of chlorine are reacted. The composition by volume of mixture is

Options

A. 0.08 L of `H_2` and 2.24 L of HCl
B. 2.24 L of `H_2` and 2.24 L of HCl
C. 0.08 L of `Cl_2` and 20.8 L of HCl
D. 22.4 L of `Cl_2` and 20.8 L of HCl

Answer

To solve the problem, we need to analyze the reaction between hydrogen (H₂) and chlorine (Cl₂) to form hydrogen chloride (HCl). The balanced chemical equation for the reaction is:

\[ \text{H}_2 + \text{Cl}_2 \rightarrow 2 \text{HCl} \]

### Step-by-Step Solution:

1. **Identify Initial Volumes:**
- Volume of hydrogen (H₂) = 1.2 L
- Volume of chlorine (Cl₂) = 1.12 L

2. **Determine the Limiting Reagent:**
- From the balanced equation, we see that 1 volume of H₂ reacts with 1 volume of Cl₂ to produce 2 volumes of HCl.
- Since we have 1.2 L of H₂ and 1.12 L of Cl₂, we need to determine which reactant will be consumed first.
- Here, Cl₂ is the limiting reagent because we have less of it compared to H₂.

3. **Calculate the Amount of Reactants Consumed:**
- Since Cl₂ is the limiting reagent, it will be completely consumed.
- Therefore, the amount of Cl₂ consumed = 1.12 L.
- According to the stoichiometry of the reaction, for every 1 L of Cl₂ consumed, 1 L of H₂ is also consumed.
- Thus, the amount of H₂ consumed = 1.12 L.

4. **Calculate Remaining Reactants:**
- Remaining H₂ = Initial H₂ - H₂ consumed
- Remaining H₂ = 1.2 L - 1.12 L = 0.08 L

5. **Calculate the Amount of Product Formed:**
- According to the reaction, 1 L of Cl₂ produces 2 L of HCl.
- Therefore, the amount of HCl produced from 1.12 L of Cl₂ = 2 × 1.12 L = 2.24 L.

6. **Final Composition of the Mixture:**
- After the reaction, we have:
- Remaining H₂ = 0.08 L
- HCl produced = 2.24 L

### Summary of Final Composition:
- Volume of H₂ = 0.08 L
- Volume of HCl = 2.24 L

### Final Answer:
The composition by volume of the mixture is:
- 0.08 L of H₂ and 2.24 L of HCl.