A container of volume V, contains `0*28` g of `N_(2)` gas. If same volume of an unknown gas under similar conditions of temperature and pressure weighs `0*44` g, the molecular mass of the gas is

Options

A. `22`
B. `44`
C. `66`
D. `88`

Explanation

To find the molecular mass of the unknown gas, we can use the relationship between the masses of gases under the same conditions of temperature and pressure. According to the law of equal volumes of gases, the ratio of the masses of two gases in the same volume is equal to the ratio of their molecular masses.

### Step-by-Step Solution:

1. **Identify the Given Data:**
- Mass of \( N_2 \) (Nitrogen gas) = \( 0.28 \, \text{g} \)
- Mass of unknown gas = \( 0.44 \, \text{g} \)
- Molecular mass of \( N_2 \) = \( 28 \, \text{g/mol} \)

2. **Set Up the Ratio:**
The ratio of the masses of the unknown gas (let's denote its molecular mass as \( M_g \)) to the mass of \( N_2 \) can be expressed as:
\[ \frac{M_g}{M_{N_2}} = \frac{\text{mass of unknown gas}}{\text{mass of } N_2} \]
Substituting the known values:
\[ \frac{M_g}{28} = \frac{0.44}{0.28} \]

3. **Calculate the Ratio:**
Now, calculate \( \frac{0.44}{0.28} \):
\[ \frac{0.44}{0.28} = 1.5714 \quad (\text{approximately}) \]

4. **Solve for \( M_g \):**
Now, we can rearrange the equation to find \( M_g \):
\[ M_g = 28 \times \frac{0.44}{0.28} \]
Substitute the calculated ratio:
\[ M_g = 28 \times 1.5714 \]
\[ M_g \approx 44 \, \text{g/mol} \]

5. **Conclusion:**
The molecular mass of the unknown gas is approximately \( 44 \, \text{g/mol} \).

### Final Answer:
The molecular mass of the unknown gas is \( 44 \, \text{g/mol} \).