0.132 g of an organic compound gave 50 ml of `N_(2)` at NTP. 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 can follow these steps:

### Step 1: Calculate moles of nitrogen gas (N₂) produced
At NTP (Normal Temperature and Pressure), 1 mole of gas occupies 22.4 liters (or 22400 mL). Given that 50 mL of N₂ was produced, we can calculate the number of moles of N₂:

\[ \text{Moles of } N_2 = \frac{\text{Volume of } N_2}{22400 \, \text{mL}} = \frac{50 \, \text{mL}}{22400 \, \text{mL/mol}} \approx 0.002232 \, \text{mol} \]

### Step 2: Calculate the mass of nitrogen in the produced N₂
The molar mass of nitrogen gas (N₂) is 28 g/mol (since the atomic mass of nitrogen is 14 g/mol). Therefore, the mass of nitrogen in the produced N₂ can be calculated as follows:

\[ \text{Mass of } N = \text{Moles of } N_2 \times \text{Molar mass of } N_2 = 0.002232 \, \text{mol} \times 28 \, \text{g/mol} \approx 0.062496 \, \text{g} \]

### Step 3: Calculate the weight percentage of nitrogen in the organic compound
The weight percentage of nitrogen in the compound is given by the formula:

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

Substituting the values we have:

\[ \text{Weight percentage of } N = \left( \frac{0.062496 \, \text{g}}{0.132 \, \text{g}} \right) \times 100 \approx 47.34\% \]

### Final Answer
Thus, the weight percentage of nitrogen in the organic compound is approximately **47.34%**.

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