11.35L of a gas at STP weighs 14g. The gas could be :

Options

A. `N_(2)O`
B. `N_(2)`
C. CO
D. Both (b) and (C )

Answer

To solve the problem of identifying the gas based on its volume and weight at STP, we can follow these steps:

### Step 1: Understand the given data
- Volume of the gas at STP = 11.35 L
- Weight of the gas = 14 g

### Step 2: Use the molar volume of a gas at STP
At STP (Standard Temperature and Pressure), 1 mole of any ideal gas occupies 22.4 liters. We can use this information to find the number of moles of the gas.

### Step 3: Calculate the number of moles of the gas
Using the formula:
\[ \text{Number of moles} = \frac{\text{Volume at STP}}{22.4 \text{ L}} \]
Substituting the given volume:
\[ \text{Number of moles} = \frac{11.35 \text{ L}}{22.4 \text{ L}} \approx 0.506 \text{ moles} \]

### Step 4: Relate moles to mass
We know that:
\[ \text{Number of moles} = \frac{\text{mass}}{\text{molar mass}} \]
Rearranging this gives us:
\[ \text{molar mass} = \frac{\text{mass}}{\text{number of moles}} \]

### Step 5: Calculate the molar mass of the gas
Substituting the known values:
\[ \text{molar mass} = \frac{14 \text{ g}}{0.506 \text{ moles}} \approx 27.6 \text{ g/mol} \]

### Step 6: Identify the gas based on molar mass
Now we need to compare the calculated molar mass with known gases:
- Molar mass of \(N_2\) (Nitrogen) = 28 g/mol
- Molar mass of \(O_2\) (Oxygen) = 32 g/mol
- Molar mass of \(CO_2\) (Carbon Dioxide) = 44 g/mol
- Molar mass of \(CH_4\) (Methane) = 16 g/mol

From our calculation, the molar mass of approximately 27.6 g/mol suggests that the gas could be Nitrogen (\(N_2\)) or any gas with a similar molar mass.

### Step 7: Conclusion
The gas could be either Nitrogen (\(N_2\)) or another gas with a molar mass close to 28 g/mol.