Answer:
There were 0.20 moles Carbon in the original sample
There were 0.40 moles hydrogen in the original sample
Explanation:
Step 1: The balanced equation
CxHyOz + O2 → CO2 + H2O
Step 2: Data given
mass of the unknown compound = 6.00 g
mass of carbon dioxide produced = 8.80 g
mass of water produced = 3.60 g
Molar mass of Carbon = 12.01 g/mole
Molar mass of Hydrygen = 1.01 g/mole ; 2.02 for H2
Molar mass of Oxygen = 16 g/mole
Molar mass of CO2 = 44.01 g/mole
Molar mass of H2O = 18.02 g/mole
Step 3: Calculate mass
8.80 g CO2 * 12.01 g/mole / 44.01 g/mole = 2.40 g carbon
3.60 g H2O * 2.02 g/mole / 18.02 g/mole = 0.404 g hydrogen
6.00 g total - 2.40 g carbon - 0.404 g hydrogen = 3.196 g oxygen
Step 4: Calculate number of moles
moles = mass / Molar mass
Mass of Carbon = 2.40g / 12.01 g/mole = 0.20 mole Carbon
Mass of hydrogen = 0.40 g / 1.01 g/mole = 0.40 mole Hydrogen
