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A compound was found by analysis to contain 65.45 percent of Carbone 9.09 percent of hydrogen and 25.45 percent of nitrogen.calculate it's empirical formula (carbon is equal 12, hydrogen 1, nitrogen 14)
Accepted Answer
Here's how to calculate the empirical formula:
1. Assume a 100g sample: This makes the percentages equal to grams. So we have 65.45g C, 9.09g H, and 25.45g N.
2. Convert grams to moles: Divide each mass by the element's molar mass:
C: 65.45g / 12 g/mol = 5.45 mol C
H: 9.09g / 1 g/mol = 9.09 mol H
N: 25.45g / 14 g/mol = 1.82 mol N
3. Find the simplest whole-number ratio: Divide each mole value by the smallest one (1.82 mol):
C: 5.45 mol / 1.82 mol = 3
H: 9.09 mol / 1.82 mol = 5
N: 1.82 mol / 1.82 mol = 1
4. Write the empirical formula: The ratio of C:H:N is 3:5:1, so the empirical formula is C₃H₅N.
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