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3 May, 14:15

Complete combustion of 4.20 g of a hydrocarbon produced 13.4 g of CO2 and 4.81 g of H2O. What is the empirical formula for the hydrocarbon?

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  1. 3 May, 15:05
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    There is a complete combustion of the hydrocarbon.

    13.4 g CO2 is produced

    The number of moles of carbon is

    13.4 g CO2 (1 mol CO2 / 44 g CO2) (1 mol C/1 mol CO2) = 0.3045 mol C

    4.81 g of H2O is produced

    The number of moles of H is

    4.81 g H2O (1 mol H2O/18 g H2O) (2 mol H/1 mol H2O) = 0.2672 mol H

    Dividing greater number by the smaller number

    0.3045 / 0.2672 = 1.14

    The empirical formula is

    CH
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