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A 0.4647-g sample of a compound known to contain only carbon, hydrogen, and oxygen was burned in dioxygen to yield 0.01962 mol of CO2 and 0.01961 mol of H2O. What is the empirical formula of the compound? A) CHO B) C3H3O2C) C2H2O D) C3H6O2E) C6H3O2I'm pretty sure this a combustion analysis problem. I found moles of C and H and then converted them to grams to find the mass of O. But for some reason I cannot get the empirical formula.
A 0.4647-g sample of a compound known to contain only carbon, hydrogen, and oxygen was burned in dioxygen to yield 0.01962 mol of CO2 and 0.01961 mol of H2O. What is the empirical formula of the compound? A) CHO B) C3H3O2C) C2H2O D) C3H6O2E) C6H3O2I'm pretty sure this a combustion analysis problem. I found moles of C and H and then converted them to grams to find the mass of O. But for some reason I cannot get the empirical formula.
Bunny GreenfelderLv2
17 Dec 2019
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