0.28 g of nitrogenous compound was subjected to Kjeldahl's process to produce 0.17 g of `NH_(3)` . The percentage of nitrogen in the organic compound is

Options

A. 5
B. 2
C. 50
D. 80

Explanation

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

### Step 1: Calculate the mass of nitrogen from the ammonia produced
We know that 1 mole of ammonia (NH₃) has a mass of 17 grams, and it contains 14 grams of nitrogen.

Using the mass of ammonia produced (0.17 g), we can set up a proportion to find the mass of nitrogen:

\[ \text{Mass of nitrogen} = \left(\frac{14 \text{ g N}}{17 \text{ g NH}_3}\right) \times 0.17 \text{ g NH}_3 \]

### Step 2: Perform the calculation
Now, we can calculate the mass of nitrogen:

\[ \text{Mass of nitrogen} = \left(\frac{14}{17}\right) \times 0.17 \approx 0.14 \text{ g} \]

### Step 3: Calculate the percentage of nitrogen in the organic compound
Now that we have the mass of nitrogen, we can calculate the percentage of nitrogen in the nitrogenous compound using the formula:

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

Substituting the values we have:

\[ \text{Percentage of nitrogen} = \left(\frac{0.14 \text{ g}}{0.28 \text{ g}}\right) \times 100 \]

### Step 4: Perform the final calculation
Now we can calculate the percentage:

\[ \text{Percentage of nitrogen} = \left(0.5\right) \times 100 = 50\% \]

### Final Answer
The percentage of nitrogen in the organic compound is **50%**.

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