Acompound contains only carbon, hydrogen, and oxygen. combustion of 9.612 mg of the compound yields 14.41 mg co2 and 3.93 mg h2o. the molar mass of the compound is 176.1 g/mol. what are the empirical and molecular formulas of the compound? (type your answer using the format co2 for co2.)

Formula used for determining the number of moles:

number of moles = -(1)

Mass of = 14.41 mg (given)

Mass of = 3.93 mg (given)

Number of moles of from =

=

Number of moles of from =

=

Mass of carbon  =

=

Mass of hydrogen =

=

Mass of oxygen = total mass of the compound - mass of carbon- mass of hydrogen

=

=

Now, number of moles of oxygen =

=

To identify the empirical formula; divide the number of moles of carbon, hydrogen and oxygen with least number of moles.

Thus,

Now, multiply the numbers with 3 to get the hydrogen number in whole number, we get

The empirical formula =

The empirical weight =

=

Divide the molecular weight with empirical weight to find the factor between empirical formula and molecular formula  , we get

=

=

Now, multiply the numbers of carbon, hydrogen and oxygen with 2 to get molecular formula, we get

Number of carbon = 6

Number of hydrogen = 8

Number of oxygen = 6

Thus, molecular formula is .

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