Hey I've attempted this problem twice and only get three attempts on it so I was wondering if I could get some help with answering this problem.
An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOz). Combustion of 2.50 g of this compound produced 3.67 g of carbon dioxide and 1.50 g of water.
How many Mols of C and H were in the original sample?
So I started like this:
(.083 mol C)x(12.0 g C)/(1 mol C)x(3.67gCO2)x(1 mol CO2)/(44.01gCO2) = .083 moles CO2 which I thought would equal 1 mol of C because there is only one mol of C in the compound.
I did the same thing for H but I divided by two because there are 2 mols of H in H2O.
I got the wrong answer apparently, I'm just confused as to what I'm doing wrong. Then they gave me a hint saying, How many mols of C are in 8.33x10^-2 mol CO2. still not sure what I'm doing wrong.