What is the empirical formula of a compound that contains 40% carbon, 6.7% hydrogen, and 53.3% oxygen?

C H_{2} O

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C H O

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C_{2} H O

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C H_{2} O_{2}

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Solution

The correct option is A $C H_{2} O$
A compound contains $40 %$ carbon, $6.7 %$ hydrogen, and $53.3 %$ oxygen.
100 g of the compound will contain 40 g C, 6.7 g H and 53.3 g O.
The atomic masses of C, H and O are 12 g/mol, 1 g/mol and 16 g/mol respectively.
The number of moles of $C = \frac{40 g}{12 g} = 3.33 m o l$
The number of moles of $H = \frac{6.7 g}{1 g} = 6.7 m o l$ .
The number of moles of $O = \frac{53.3 g}{16 g} = 3.33 m o l$ .
The mole ratio $C : H : O = 3.33 : 6.7 : 3.33 = 1 : 2 : 1$
The empirical formula of compound is $C H_{2} O$ .

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