A compound is found to contain 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. Determine the empirical formula of this compound.
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To determine the empirical formula, we need to find the ratios of the different elements in the compound.
1. Assume we have a 100g sample of the compound.
2. Convert the mass of each element to moles using their molar masses.
The molar masses of carbon (C), hydrogen (H), and oxygen (O) are approximately:
C: 12.01 g/mol
H: 1.01 g/mol
O: 16.00 g/mol
3. Convert the mass of each element to moles:
Carbon (C):
0.40 * 100 g = 40 g
moles of C = 40 g / 12.01 g/mol ≈ 3.330 moles
Hydrogen (H):
0.067 * 100 g = 6.7 g
moles of H = 6.7 g / 1.01 g/mol ≈ 6.634 moles
Oxygen (O):
0.533 * 100 g = 53.3 g
moles of O = 53.3 g / 16.00 g/mol ≈ 3.331 moles
4. Find the simplest ratio by dividing the number of moles of each element by the smallest number of moles (approximately 3.330 moles):
Carbon (C): 3.330 moles / 3.330 moles = 1 mole
Hydrogen (H): 6.634 moles / 3.330 moles ≈ 1.994 moles ≈ 2 moles
Oxygen (O): 3.331 moles / 3.330 moles ≈ 1 mole
Therefore, the empirical formula of the compound is CH2O.
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