A compound contains 4.07% hydrogen,24.27% carbon and 71.65% chlorine. Its molar mass is 98.96g Determine its empirical and molecular formulas
Answers
Explanation:
In 100g of sample of the compound, 4.07g of hydrogen, 24.27g of carbon and 71.65g of chlorine are present. Moles of hydrogen= 4.07g/ 1g = 4.0 Moles of carbon= 24.27g/ 12g = 2.0 Moles of chlorine= 71.65g/ 35g= 2.0 Since 2.0 is the smallest value, so by dividing each of the mole values obtained by this smallest value we will get a ratio of 2:1:1 for H:C:Cl. Thus, the empirical formula of the compound is CH2Cl. For CH2Cl, empirical formula mass= 12+ (2×1) +35 = 49g. Molar mass/ empirical formula = 98.96g/ 49g = 2=n Therefore, Empirical formula = CH2Cl n=2 Hence, molecular
Answer:
Explanation:
% mass ratio1 ratio2
4.07 1 4 2
24.27 12 2 1
71.65 35.5 2 1
CH2Cl = 49.5 emperical formula
(CH2Cl = 49.5)*2 = C2H4Cl2 = molecular formula