An unknown hydrocarbon gave 0.07484 g of CO2 and 0.03063 g of
H2O on combustion. What...
An unknown hydrocarbon gave 0.07484 g of CO2 and 0.03063 g of
H2O on combustion. What is the empirical formula of this unknown
hydrocarbon? a.C2H b.CH c.CH3 d.CH2
Complete combustion of 7.60 g of a hydrocarbon produced 23.0 g
of CO2 and 11.8 g of H2O. What is the empirical formula for the
hydrocarbon? I got C4H10 but was incorrect.
Complete combustion of 7.70 g of a hydrocarbon produced 23.6 g
of CO2 and 11.3 g of H2O. What is the empirical formula for the
hydrocarbon? Insert the subscripts:
CH
Combustion of 135.2 g of a compound produces 440.0 g CO2 and
135.0 g H2O. The molar mass of the compound is 270 g/mol. Determine
the empirical and molecular formula of the hydrocarbon (show all
work)
Combustion of 8.732 mg of an unknown organic compound gave
16.432 mg of CO2 and 2.840 mg of H2O. (a) find the wt% of C and H
in the substance. (b) Find the smallest reasonable integer mole
ration of C:H in the compound.