Verified answer

It is probably should be 2mg of CO2 and 1mg of H2O, otherwise the solution is CH10 that does not make sense.

1. Divide masses of produced CO2 and H2O by their respective molar masses to find the amount of moles of CO2 and H2O:

0.002/44=4.5454x10^-5 moles of CO2 which equals the number of moles of C

0.001/18=5.5555x10^-5 moles of H2O which means 1.1111x10^-4 moles of H

2. Take the ratio of n(H) to n(C): 1.1111x10^-4/4.5454x10^-5=2.44

So, you have something close to CH2.5 or closest compound that makes sense is C4H10, butane

You need to find moles of C from 1.00mg of CO2 and the same goes for H from 2.00mg of H2O.

mols C - 1.00mg CO2 *(1mol CO2/44.01mg CO2)*(1mol C/1Mol CO2)= 0.022722 Mol C

Mols H - 2.00mg H2O*(1mol H2O/18.016g H2O)*(2mol H/1mol H2O)= 0.222025 Mol H

To find Empirical Formula Divide the smallest mol into each mol.

0.022722 Mol C/ 0.022722Mol C = 1

0.222025 Mol H/ 0.022722 Mol C = 9.77131

Our Empirical Formula So far is C1H9.77131

Now you have to multiply by the smallest whole number that will get 9.77 close to a whole number and multiply C by that as well. This number should be 4.

So the Empirical Formula Is

C4H39

The carbon in the CO2 comes from the carbon in the compound

so : 1.00 mg = .000100 g C / 44.01 = moles CO2 = moles of Carbon (because there is only one Carbon atom per molecule of CO2)

the hydrogen from the H2O comes from the compound also

so

2.00mg = .000200 grams H / 18.02 = moles of H2O x 2 = moles of H because there are two atoms of H per molecule of H20

Moles of C: about .0227

Moles of H: about .229

since there are the least number of moles of C, divide both numbers by .0227 to get the mole ratio. this will give you the empirical formula, but there is no way to get the molecular formula without the mass of the compound.