Asked by Sinachi
Assuming the relative molecular mass of a compound with empirical formula C2H4NO is 116. What is the molecular formula
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To find the molecular formula, we need to first calculate the empirical formula's mass.
Empirical formula mass = (2 x atomic mass of C) + (4 x atomic mass of H) + (atomic mass of N) + (atomic mass of O)
Empirical formula mass = (2 x 12.01) + (4 x 1.01) + 14.01 + 16.00 = 42.03 g/mol
Now, we can use the given relative molecular mass to determine the molecular formula:
Relative molecular mass (M) = n x empirical formula mass
where n is the number of empirical formula units in the molecular formula.
n = M / empirical formula mass = 116 / 42.03 = 2.76
Since we cannot have a fraction of a molecule, we round n to the nearest whole number. Therefore, the molecular formula is:
Molecular formula = n x empirical formula
Molecular formula = 3 x C2H4NO
Molecular formula = C6H12N2O3
Empirical formula mass = (2 x atomic mass of C) + (4 x atomic mass of H) + (atomic mass of N) + (atomic mass of O)
Empirical formula mass = (2 x 12.01) + (4 x 1.01) + 14.01 + 16.00 = 42.03 g/mol
Now, we can use the given relative molecular mass to determine the molecular formula:
Relative molecular mass (M) = n x empirical formula mass
where n is the number of empirical formula units in the molecular formula.
n = M / empirical formula mass = 116 / 42.03 = 2.76
Since we cannot have a fraction of a molecule, we round n to the nearest whole number. Therefore, the molecular formula is:
Molecular formula = n x empirical formula
Molecular formula = 3 x C2H4NO
Molecular formula = C6H12N2O3