6 g of the organic compound on heating with NaOH gave `NH_(3)` which is neutralised by 200 mL of 1(N) HCl. Percentage of nitrogen is ?

Options

A. 0.12
B. 0.6
C. 0.4667
D. 0.2667

Answer

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

### Step 1: Determine the moles of HCl used
Given that 200 mL of 1 N HCl is used, we can calculate the number of equivalents of HCl.

\[ \text{Normality (N)} = \frac{\text{Number of equivalents}}{\text{Volume in liters}} \]

Here, the volume of HCl is 200 mL, which is 0.2 L. Therefore, the number of equivalents of HCl is:

\[ \text{Number of equivalents} = \text{Normality} \times \text{Volume in liters} = 1 \times 0.2 = 0.2 \text{ equivalents} \]

### Step 2: Relate equivalents of HCl to moles of nitrogen
Since each mole of NH₃ (ammonia) contains one mole of nitrogen, the number of moles of nitrogen produced from the reaction is equal to the number of equivalents of HCl used:

\[ \text{Moles of nitrogen} = 0.2 \text{ moles} \]

### Step 3: Calculate the mass of nitrogen
The molar mass of nitrogen (N) is 14 g/mol. Therefore, the mass of nitrogen can be calculated as follows:

\[ \text{Mass of nitrogen} = \text{Moles of nitrogen} \times \text{Molar mass of nitrogen} = 0.2 \times 14 = 2.8 \text{ grams} \]

### Step 4: Calculate the percentage of nitrogen in the organic compound
To find the percentage of nitrogen in the organic compound, we use the formula:

\[ \text{Percentage of nitrogen} = \left( \frac{\text{Mass of nitrogen}}{\text{Mass of organic compound}} \right) \times 100 \]

Substituting the values we have:

\[ \text{Percentage of nitrogen} = \left( \frac{2.8}{6} \right) \times 100 \approx 46.67\% \]

### Conclusion
The percentage of nitrogen in the organic compound is approximately **46.67%**.

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