Question

. A certain hydrocarbon on complete combustion at s.t.p produced 89.6dm3 of CO2

and 54g of water. The hydrocarbon should be

Answer 1

moles of CO2 =$\frac{V}{V_m}=\frac{89.6}{22.4} = 4 mole$

$n(C) = n(CO_2)=4 mole$

moleas of H2O =$\frac{m}{M} =\frac{54}{18} = 3 mole$

$n(H) = 2\times n(H_2O)=2\times 3 = 6 mole$

mole ratio $n(C);n(H) = 4:6= 2:3$

the empirical formula of hydrocarbon is C2H3. the molecular formulas could be:

C4H6