If the weight of `5.6` litres of a gas at `N.T.P.` is 11 gram. The gas may be `:`

Options

A. `PH_(3)`
B. `COCl_(2)`
C. `NO`
D. `N_(2)O`

Explanation

To solve the problem of identifying the gas based on its weight and volume at NTP (Normal Temperature and Pressure), we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Given Information**:
- Volume of gas = 5.6 liters
- Weight of gas = 11 grams
- At NTP, 1 mole of gas occupies 22.4 liters.

2. **Calculate the Weight of 1 Mole of Gas**:
- We know that 5.6 liters of gas weighs 11 grams.
- To find the weight of 22.4 liters (which is 1 mole), we can set up a proportion:
\[ \text{Weight of 22.4 liters} = \left(\frac{11 \text{ grams}}{5.6 \text{ liters}}\right) \times 22.4 \text{ liters} \]

3. **Perform the Calculation**:
- Calculate the weight:
\[ \text{Weight of 22.4 liters} = \frac{11}{5.6} \times 22.4 \]
- First, calculate \( \frac{11}{5.6} \):
\[ \frac{11}{5.6} = 1.9643 \text{ grams/liter} \]
- Now multiply by 22.4:
\[ 1.9643 \times 22.4 = 44 \text{ grams} \]

4. **Identify the Molecular Weight of the Gas**:
- The weight of 22.4 liters of the gas is 44 grams, which means the molecular weight of the gas is 44 g/mol.

5. **Determine the Gas**:
- Now we need to identify which gas has a molecular weight of 44 g/mol.
- Check the options:
- Option A: NO (Molecular weight = 30 g/mol)
- Option B: N2O (Molecular weight = 44 g/mol)
- Option C: CO (Molecular weight = 28 g/mol)
- Option D: CO2 (Molecular weight = 44 g/mol)

6. **Select the Correct Option**:
- The gas with a molecular weight of 44 g/mol is N2O (D) and CO2 (D). Since the question asks for the gas, we can conclude that both are valid answers, but typically, N2O is the one referred to in such problems.

### Final Answer:
The gas may be **N2O (Nitrous oxide)** or **CO2 (Carbon dioxide)**.