a compound was analyzed and found to contain C,H,N,O, and Cl. When o.150g sample of this compound was burned, it produced 0.138 g of CO2 and 0.0566 g of H2O. All of the Nitrogen in another sample of mass 0.200 g was converted to 0.0238 g of NH3. Finally, the chlorine in a 0.500 g sample of the compound was converted to Cl- an precipitated as AgCl. the precipitate had a mass of 1..004 g. Find the empirical formula of the compound.

Question

when going from CO2 to C or from H20 to H and so on. Will we have to balance the equation or just 1 mole of co2 = 1 mole of C?!! Help plz

Answer 1

1 mole of CO2 = 1 mole C.
2 moles H = 1 mole H2O
etc.

Answer 2

ok i got the answer but seem different i get C3H6Cl2 N O