1.2 g of an organic compound on Kjeldahlization liberates ammonia which consumes 30 `cm^3` of 1 N HCI. The percentage of nitrogen in the organic compound is

Options

A. 30
B. 35
C. 46.67
D. 20.8

Answer

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

### Step-by-Step Solution:

1. **Identify the Given Data:**
- Mass of the organic compound = 1.2 g
- Volume of HCl consumed = 30 cm³ (which is equivalent to 30 mL)
- Normality of HCl = 1 N

2. **Use the Formula for Percentage of Nitrogen:**
The formula to calculate the percentage of nitrogen in the organic compound is:
\[ \text{Percentage of Nitrogen} = \frac{1.4 \times \text{Normality of HCl} \times \text{Volume of HCl (mL)}}{\text{Mass of organic compound (g)}} \]

3. **Substitute the Values into the Formula:**
- Normality of HCl = 1 N
- Volume of HCl = 30 mL
- Mass of organic compound = 1.2 g

Plugging these values into the formula:
\[ \text{Percentage of Nitrogen} = \frac{1.4 \times 1 \times 30}{1.2} \]

4. **Calculate the Numerator:**
\[ 1.4 \times 1 \times 30 = 42 \]

5. **Calculate the Percentage of Nitrogen:**
\[ \text{Percentage of Nitrogen} = \frac{42}{1.2} = 35 \]

6. **Final Result:**
The percentage of nitrogen in the organic compound is **35%**.