Acompound contains only carbon, hydrogen, and oxygen. combustion of 11.75 mg of the compound yields 17.61 mg co2 and 4.81 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.)

Number of moles is defined as the ratio of given  mass in g to the molar mass.

First, convert the given mass of carbon dioxide in mg to g:

1 mg = 0.001 g

17.61 mg = 0.01761 g

Number of moles of carbon dioxide =

=

Mass of carbon  = number of moles of carbon dioxide \times molar mass of carbon

=

=

Number of moles of water=

=

Since, water contains two hydrogen atoms. Thus,

Moles of hydrogen =

=

Mass of hydrogen =

=

Mass of oxygen =

=

Number of moles of oxygen =

=

Now,

Divide the smallest number to get the whole number,

we get,

Now, multiply all the subscript by 3 to get the whole number,

  (empirical fomula)

Molar mass of the compound  =

=

Divide given molar mass of the compound with the molar mass of the compound.

=

=

Thus, multiply the subscripts of empirical formula by 2 to get the molecular formula, we get:

Hence, empirical formula is and molecular formula is

fr8t7iot7o87oglgt87ot79p0[90

the answers would be

the first one and the second one