QuestionJune 5, 2025

5. What is the percent composition by mass of nitrogen (N) in ammonium nitrate (NH4NO3)

5. What is the percent composition by mass of nitrogen (N) in ammonium nitrate (NH4NO3)
5. What is the percent composition by mass of nitrogen (N) in ammonium nitrate (NH4NO3)

Solution
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Answer

35.00% Explanation 1. Calculate Molar Mass of NH_4NO_3 Molar mass of N = 14.01 \, \text{g/mol}, H = 1.01 \, \text{g/mol}, O = 16.00 \, \text{g/mol}. Total molar mass of NH_4NO_3 = (2 \times 14.01) + (4 \times 1.01) + (3 \times 16.00) = 80.05 \, \text{g/mol}. 2. Calculate Mass of Nitrogen in NH_4NO_3 Mass of nitrogen = 2 \times 14.01 = 28.02 \, \text{g}. 3. Calculate Percent Composition **Percent composition** = \left(\frac{\text{Mass of N}}{\text{Molar mass of } NH_4NO_3}\right) \times 100 = \left(\frac{28.02}{80.05}\right) \times 100.

Explanation

1. Calculate Molar Mass of $NH_4NO_3$<br /> Molar mass of $N = 14.01 \, \text{g/mol}$, $H = 1.01 \, \text{g/mol}$, $O = 16.00 \, \text{g/mol}$. Total molar mass of $NH_4NO_3 = (2 \times 14.01) + (4 \times 1.01) + (3 \times 16.00) = 80.05 \, \text{g/mol}$.<br />2. Calculate Mass of Nitrogen in $NH_4NO_3$<br /> Mass of nitrogen = $2 \times 14.01 = 28.02 \, \text{g}$.<br />3. Calculate Percent Composition<br /> **Percent composition** = $\left(\frac{\text{Mass of N}}{\text{Molar mass of } NH_4NO_3}\right) \times 100 = \left(\frac{28.02}{80.05}\right) \times 100$.
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