Respuesta :
Answer:
[tex]C_4H_6[/tex]
Explanation:
[tex]Moles =Given\ mass \times {Molar\ mass}[/tex]
Mass of water obtained = 27.0 g
Moles of [tex]H_2O[/tex] = 27.0 / 18 = 1.5 moles
2 moles of hydrogen atoms are present in 1 mole of water. So,
Moles of H = 2 x 1.5 = 3 moles
Molar mass of H atom = 1.008 g/mol
Mass of H in molecule = 3 x 1.008 = 3.024
Given that the compound is hydrocarbon. So it only contains hydrogen and carbon. So,
Mass of C in the sample = Total mass - Mass of H
Mass of the sample = 27 g
Mass of C in sample = 27 - 3.024 = 23.976 g
Molar mass of C = 12 g/mol
Moles of C = 23.976 / 12 = 1.998 moles
Taking the simplest ratio for H and C as:
3.024 : 1.998 = 3 : 2
The empirical formula is = [tex]C_2H_3[/tex]
Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.
Thus,
Molecular mass = n × Empirical mass
Where, n is any positive number from 1, 2, 3...
Since, the hydrogen is present in odd number in the empirical formula.So, possible molecular formula is:
Molecular mass = 2 × Empirical mass
The least possible formula of hydrocarbon = [tex]C_4H_6[/tex]
The molecular formula shows all the atoms that are present in a molecule. The molecular formula here is C4H6.
What is empirical formula?
Mass of water = 27.0 g
Number of moles of water Moles of = 27.0 / 18 = 1.5 moles
Number of moles of hydrogen = 2 x 1.5 = 3 moles
Mass of Hydrogen atom in the molecule = 3 x 1.008 = 3.024g
Mass of carbon = Total mass - Mass of H
Mass of carbon in the sample = 27 - 3.024 = 23.976 g
Number of moles of carbon= 23.976 / 12 = 1.998 moles
Divide through by the lowest ratio;
3.024 : 1.998 = 3 : 2
Emperical formula = C2H3
Hence the molecular formula of the compound must be C4H6.
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