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Sagot :
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Get the mass of each element by assuming a certain overall mass for the sample (100 g is a good mass to assume when working with percentages).
- (.7546) (100 g) = 75.46 g C
- (.0443) (100 g) = 4.43 g H
- (.2010) (100 g) = 20.10 g O
Convert the mass of each element to moles.
- (75.46 g C) (1 mol/ 12.00 g C) = 6.289 mol C
- (4.43 g H) (1 mol/ 1.008 g H) = 4.39 mol H
- (20.10 g O) (1 mol/ 16.00 g O) = 1.256 mol O
Find the ratio of the moles of each element.
- (1.256 mol O)/ (1.256) = 1 mol O
- (6.289 mol C)/ (1.256) = 5.007 mol C
- (4.39 mol H)/ (1.256) = 3.50 mol H
Use the mole ratio to write the empirical fomula.
Multiplying the mole ratios by two to get whole number, the empirical formula becomes:
- C10H7O2
Find the mass of the empirical unit.
- 10(12.00) + 7(1.008) + 2(16.00) = 159.06 g/mol
Figure out how many empirical units are in a molecular unit.
- (318.31 g/mol) / (159.06 g/mol) = 2.001 empirical units per molecular unit
Write the molecular formula.
Since there are two empirical units in a molecular unit, the molecular formula is:
- C20H14O4
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