In: Chemistry
when 4.027 grams hydrocarbon, CxHy, we're burned in a combustion analysis apparatus, 12.64 grams of CO2 and 5.174 grams H2O we're produced.
I need empirical and molecular formulas
C% = 12*wt of CO2*100/44*wt of hydrocarbon
= 12*12.64*100/44*4.027 = 85.6%
H% = 2*wt of H2O*100/18*wt of hydrocarbon
= 2*5.174*100/18*4.027 = 14.4%
element % A.wt relative number simple ratio
C 85.6 12 85.6/12 = 7.13 7.13/7.13 = 1
H 14.4 1 14.4/1 = 14.4 14.4/7.13 = 2
Empirical formula = CH2