0.132g of an organic compound gave 50 ml of `N_(2)` of STP. The weight percentage of nitrogen in the compound is close to

Options

A. 15
B. 20
C. 48.9
D. 47.34

Explanation

To find the weight percentage of nitrogen in the organic compound, we will follow these steps:

### Step 1: Calculate the number of moles of \(N_2\)
We are given that 50 mL of nitrogen gas is produced at STP (Standard Temperature and Pressure). At STP, 1 mole of any gas occupies 22.4 liters (or 22400 mL).

\[ \text{Number of moles of } N_2 = \frac{\text{Volume of } N_2}{\text{Molar volume at STP}} = \frac{50 \, \text{mL}}{22400 \, \text{mL/mol}} = 2.23 \times 10^{-3} \, \text{moles} \]

### Step 2: Calculate the mass of nitrogen in grams
The molar mass of \(N_2\) (nitrogen gas) is 28 g/mol. We can find the mass of nitrogen produced using the number of moles calculated in the previous step.

\[ \text{Mass of } N_2 = \text{Number of moles} \times \text{Molar mass} = 2.23 \times 10^{-3} \, \text{moles} \times 28 \, \text{g/mol} = 0.0624 \, \text{g} \]

### Step 3: Calculate the weight percentage of nitrogen in the compound
The weight percentage of nitrogen in the compound is calculated using the formula:

\[ \text{Weight percentage of } N = \left( \frac{\text{Mass of } N_2}{\text{Total mass of compound}} \right) \times 100 \]

Substituting the values we have:

\[ \text{Weight percentage of } N = \left( \frac{0.0624 \, \text{g}}{0.132 \, \text{g}} \right) \times 100 \approx 47.27\% \]

### Conclusion
Therefore, the weight percentage of nitrogen in the organic compound is approximately **47.3%**.

---