I have a simple yet puzzling question which is as following.

"A hydrocarbon was subjected to combustion analysis. A sample of the compound gave 0.314g CO2 and 0.129g H2O"

a) Calculate the masses of carbon and Hydrogen on the sample
b) Find the number of moles of carbon in the sample of the compound.
c) What is the empirical formula of the compund?
d) if its relative mass is 84 what is its molecular formula
e) draw a posssible skeletal mass

I really need help as I do not know where to begin. Ive calculated that 0.129g of h2o is equal to 7x10(power)-3 moles and that 0.314g of CO2 is also equal to 7x10(power)-3 moles

Thank you all in advance
i... hated... chemistry. i feel for you man, unless you like the class
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Post this in the appropriate thread and I'll help you.
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k dude i haven't done this in awhile, but i'll try to help

you've gotta find the molar mass of h2o and co2 (the mass per mole of that)
to do this, you add up the atomic numbers on the periodic table

and then, use that to calculate how many molecules of C and H there were.. that's for the first part anyway... post again if you need help and i might still be on?
have you done molar ratios?
you can use the ratios to find the number of moles for the reactants.

i dunno if that helps its hard to explain without seeing it, but yeah i had that course last semester, ****ty for you bro
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