Combustion of 5.000 g of a hydrocarbon produces 15.40 g of CO2 and 7.886 g of H2O. What is the empirical formula?

C2H5 Mol C = 15.40/44.01 = 0.3499. Mol H = 2 \cdot 7.886/18.02 = 0.8753. Ratio H:C = 0.8753/0.3499 = 2.50, i.e. C:H = 2:5. The empirical formula is C2H5.

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Elemental Composition of Pure Substances

AP Chemistry· difficulty 4/5

CO_2

A
$C_2H_5$
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B
$C_4H_9$
C
$C_3H_7$
D
$CH_3$

Explanation

15.40/44.01 = 0.3499

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