posted by ALAN
A 8.408 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 12.53 grams of CO2 and 3.849 grams of H2O are produced.
In a separate experiment, the molar mass is found to be 118.1 g/mol. Determine the empirical formula and the molecular formula of the organic compound.
Find empirical formula and molecular formula.
Put in order of C,H,O.
JILLIAN, Alan. We prefer to keep the same screen name. Refer to your other problem. It a little simpler with just CxHy. This one is CxHyOz. The only difference is this.
Convert 12.53 g CO2 to g C.
Convert 3.849 g H2O to g H.
To find g O, it is
g O = 8.408 g - g C - g H
Then convert g C to mols C, g H to mols H, and g O to mols O.
Then convert these to ratios of whole numbers the same was as the other problem. The molecular formula is done the same way, also.
i literally have no idea how to do these and your explanations are not helping..... like i have no example and i need you to work one out and i can do the other but they are do soon and i have no clue what you are saying.
See my response to your earlier CxHy question below. I've worked it in detail. I hope things work out for you very well.