Combustion of 27.44 g of a compound containing only carbon, hydrogen, and oxygen produces 53.60 gCO2 and 27.43 gH2O. What is the empirical formula of the compound?
I know that the answer will be some variation of C_a H_b O_c.
I have determined the mols of O (0.7894), H (0.1808), and C (1.218) in the products through calculation but I do not know what to do with them now.
I know that the answer will be some variation of C_a H_b O_c.
I have determined the mols of O (0.7894), H (0.1808), and C (1.218) in the products through calculation but I do not know what to do with them now.
1 Answer
Well, let us see...I make in
Explanation:
We got
Combustion yields
What mass is unaccounted? That of oxygen in the initial sample...there are few ways to analyze for oxygen content... On the other hand, carbon, as carbon dioxide, and hydrogen, as WATER, may be routinely and accurately analyzed on a gas chromatograph; and these are the unspoken premises of the question.
And so we get a trial empirical formula of
This is probably a first year problem....but all I have done is to assume COMPLETE combustion of a hydrocarbon...i.e.
The rest is arithmetic....which is quite laborious...and I think you get this....anyway if you are unclear as to the steps ask for qualification and someone will help.