posted by Franklin on .
0.717 g of a compound containing carbon, hydrogen, and oxygen is burned and found to produce 1.02 g CO2 and 0.624 g H2O. The molar mass of the compound is 124 g/mol.
(a) Write a chemical equation for the combustion of this unknown hydrocarbon.
(b) Determine the # of g and moles of carbon, hydrogen, and oxygen in the unknown hydrocarbon.
(c) Calculate the empirical formula.
(d) Calculate the molecular formula.
(e) Write the balanced equation for the combustion reaction.
You must know SOMETHING about this problem. Tell me what you know and I can help you through the remainder of it.
You know the mass of the hydrocarbon and the what mass of the products produced are as well as the mass of the compound.
part b. Convert g CO2 to g C, convert g H2O to g hydrogen, add the two and subtract from 0.717 to find g oxygen. Then I would find %C, %H, and %O. Take a 100 g sample and find moles. moles = grams/molar mass.