An unknown compound was decomposed into 316 g carbon, 26.3 g hydrogen, and 208 g oxygen. What is its empirical formula?
Question
An unknown compound was decomposed into 316 g carbon, 26.3 g hydrogen, and 208 g oxygen. What is its empirical formula?
Solution
To find the empirical formula, follow these steps:
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Convert the mass of each element to moles.
For Carbon: 316 g / 12.01 g/mol = 26.31 mol For Hydrogen: 26.3 g / 1.008 g/mol = 26.09 mol For Oxygen: 208 g / 16.00 g/mol = 13 mol
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Divide each mole quantity by the smallest number of moles calculated.
For Carbon: 26.31 mol / 13 = 2.02 ≈ 2 For Hydrogen: 26.09 mol / 13 = 2.01 ≈ 2 For Oxygen: 13 mol / 13 = 1
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Round to the nearest whole number.
For Carbon: 2 For Hydrogen: 2 For Oxygen: 1
So, the empirical formula of the compound is C2H2O.
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