Determine the correct empirical formula of a compound containing 26.68% carbon, 2.24% hydrogen, and 71.08% oxygen give the following molar masses: C: 12.01 g/mole; H: 1.01 g/mole; O:16.00 g/mole.Group of answer choicesCHOCHO2CH2OC2H2O4
Question
Determine the correct empirical formula of a compound containing 26.68% carbon, 2.24% hydrogen, and 71.08% oxygen give the following molar masses: C: 12.01 g/mole; H: 1.01 g/mole; O:16.00 g/mole.Group of answer choicesCHOCHO2CH2OC2H2O4
Solution
To determine the empirical formula, we first assume that we have 100g of the compound. This means that the percentages given can be viewed as grams.
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Convert the percentages to grams:
- Carbon (C): 26.68g
- Hydrogen (H): 2.24g
- Oxygen (O): 71.08g
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Convert the grams to moles using the molar masses given:
- Carbon (C): 26.68g / 12.01g/mole = 2.22 moles
- Hydrogen (H): 2.24g / 1.01g/mole = 2.22 moles
- Oxygen (O): 71.08g / 16.00g/mole = 4.44 moles
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Divide each mole quantity by the smallest number of moles calculated to get the mole ratio:
- Carbon (C): 2.22 moles / 2.22 = 1
- Hydrogen (H): 2.22 moles / 2.22 = 1
- Oxygen (O): 4.44 moles / 2.22 = 2
So, the empirical formula of the compound is CHO2.
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