emperical formula?

Question

An unknown compound contains C, H and N. When 0.574 g was burned in a combustion apparatus 0.4187 g of H 2O and 1.1364 g CO 2 were produced. What is the empirical formula of the compound?
just tell me the procedure

Answer 1

From the weight of CO2, calculate the weight of C produced and then the number of moles of C atoms produced.

From the weight of H2O, calculate the weight of H produced and the the moles of H atoms produced.

From the weight of the sample, and the weight of C and the weight of H, you can calculate the weight of N by difference and then the moles of N atoms in the sample..

You will now have the moles of C, H, and N
You need to divide all of these values by the smallest. (That will give you 1.00 mole for the smallest.)
Your goal is to multiply all of these values by a number that will make them whole numbers (or very close to whole numbers) because the subscripts of the empirical formula must be whole numbers.

For example if the ratio of N : C : H was 1 : 1.49 : 2.34 (I made these numbers up to illustrate the method)
You could multiply by 6 to get 6 :8.94 : 14.04
I would call that 6 : 9 : 14 and the formula would be-
C9H14N6

Answer 2

Work out the moles of C in the CO2, and the moles of H in H2O, and this gives you the ratio of C:H. Work out the actual masses of C and H, and subtract from 0.574. This gives the mass of N, and dividing by 14 gives the moles. Now you can work out the C:H:N ratio.