Answer:
C6H12O3
Explanation:
Data obtained from the question include:
C (carbon) = 54.5%
H (hydrogen) = 9.1%
O (oxygen) = 36.4%
To obtain the molecular formula, first, let us obtain the empirical formula. This is illustrated below
C = 54.5%
H = 9.1%
O = 36.4%
Divide by their individual molar mass.
C = 54.5/12 = 4.542
H = 9.1/1 = 9.1
O = 36.4/16 = 2.275
Divide by the smallest
C = 4.542/2.275 = 2
H = 9.1/2.275 = 4
O = 2.275/2.275 = 1
The empirical formula is C2H4O
The molecular formula is simply a multiple of the empirical formula. This is illustrated below:
Molecular formula => [C2H4O]n
The molar mass of the compound as obtained from the question is 135g/mol
Now, with the above information, we can simply calculate the value of n in order to obtain the molecular formula. This is illustrated below:
[C2H4O]n = 135
[(12x2) + (4x1) + 16]n = 135
[24 + 4+ 16]n = 135
44n = 135
Divide both side by the coefficient of n i.e 44
n = 135/44
n = 3
The molecular formula
=> [C2H4O]n
=> [C2H4O]3
=> C6H12O3
