To solve the problem, we need to determine the percentage of nitrogen in the organic compound based on the information provided. Here’s a step-by-step breakdown of the solution:
### Step 1: Understand the Reaction
The ammonia evolved from the organic compound neutralizes sulfuric acid (H₂SO₄). The amount of H₂SO₄ used is given as 10 mL of 1 M solution.
### Step 2: Calculate Moles of H₂SO₄
Using the molarity and volume of H₂SO₄, we can calculate the number of moles of H₂SO₄:
\[
\text{Moles of H₂SO₄} = \text{Molarity} \times \text{Volume (L)} = 1 \, \text{mol/L} \times 0.010 \, \text{L} = 0.010 \, \text{mol}
\]
### Step 3: Determine Moles of Ammonia (NH₃)
The reaction between ammonia and sulfuric acid is:
\[
2 \, \text{NH₃} + \text{H₂SO₄} \rightarrow \text{(NH₄)₂SO₄}
\]
From the stoichiometry of the reaction, 1 mole of H₂SO₄ reacts with 2 moles of NH₃. Therefore, the moles of NH₃ produced can be calculated as:
\[
\text{Moles of NH₃} = 2 \times \text{Moles of H₂SO₄} = 2 \times 0.010 \, \text{mol} = 0.020 \, \text{mol}
\]
### Step 4: Calculate Mass of Nitrogen in Ammonia
The molar mass of ammonia (NH₃) is approximately 17 g/mol, and since each mole of NH₃ contains 1 mole of nitrogen (N), we can find the mass of nitrogen:
\[
\text{Mass of NH₃} = \text{Moles of NH₃} \times \text{Molar Mass of NH₃} = 0.020 \, \text{mol} \times 17 \, \text{g/mol} = 0.34 \, \text{g}
\]
Since nitrogen has a molar mass of approximately 14 g/mol, the mass of nitrogen in the ammonia is:
\[
\text{Mass of Nitrogen} = \text{Moles of NH₃} \times 14 \, \text{g/mol} = 0.020 \, \text{mol} \times 14 \, \text{g/mol} = 0.28 \, \text{g}
\]
### Step 5: Calculate Percentage of Nitrogen in the Organic Compound
Now, we can find the percentage of nitrogen in the original organic compound:
\[
\text{Percentage of Nitrogen} = \left( \frac{\text{Mass of Nitrogen}}{\text{Mass of Organic Compound}} \right) \times 100 = \left( \frac{0.28 \, \text{g}}{0.5 \, \text{g}} \right) \times 100 = 56\%
\]
### Conclusion
The percentage of nitrogen in the organic compound is 56%. Therefore, the correct statement is that the percentage of nitrogen in the organic compound is 56%.
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