A certain compound contains only C, H, and N. Combustion of 0.125 g of this compound produces 0.172 g of H2O and 0.279 g of CO2. Calculate the number of moles of CO2 and H2O.
The compound contains only carbon C, hydrogen H and nitrogen N. When 0.125 g of the compound undergoes combustion 0.172 g of H2O and 0.279 g of CO2 are produced.
The atomic mass of hydrogen is 1 and that of oxygen is 16. H2O has a molecular mass of 2 + 16 = 18 g/ mole. 0.172 g of water (H2O) is equivalent to 0.172/18 = 9.55*10^-3 moles of H2O
The molecular mass of carbon is 12 and that of oxygen is 16. The molecular mass of CO2 is 12 + 16*2 = 44 g/mole. 0.279 g of CO2 is equivalent to 6.34*10^-3 moles of CO2.