Answer:
C4H8O4
Explanation:
To determine the molecular formula, first, let us obtain the empirical formula. This is illustrated below:
From the question given, we obtained the following information:
C = 45.45%
H = 6.12%
O = 48.44%
Divide the above by their molar mass
C = 45.45/12 = 3.7875
H = 6.12/1 = 6.12
O = 48.44/16 = 3.0275
Divide by the smallest
C = 3.7875/3.0275 = 1
H = 6.12/3.0275 = 2
O = 3.0275/3.0275 = 1
The empirical formula is CH2O
The molecular formula is given by [CH2O]n
[CH2O]n = 132.12
[12 + (2x1) + 16]n = 132.12
30n = 132.12
Divide both side by the coefficient of n i.e 30
n = 132.12/30 = 4
The molecular formula is [CH2O]n = [CH2O]4 = C4H8O4
Answer:
The molecular formula is C5H8O4
Explanation:
Step 1: Data given
Suppose the mass of the compound is 100 grams
The compound contains:
45.45 % Carbon = 45.45 grams
6.12 % hydrogen = 6.12 grams
48.44 % oxygen = 48.44 grams
Molar mass of C = 12.01 g/mol
Molar mass of H = 1.01 g/mol
Molar mass of O = 16.0 g/mol
Step 2: Calculate moles
Moles = mass / molar mass
Moles C = 45.45 grams / 12.01 g/mol
Moles C = 3.784 moles
Moles H = 6.12 grams / 1.01 g/mol
Moles H = 6.059 moles
Moles O = 48.44 grams / 16.0 g/mol
Moles O = 3.028 moles
Step 4: Calculate mol ratio
We divide by the smallest amount of moles
C: 3.784 / 3.028 = 1.25
H: 6.059 / 3.028 = 2
O: 3.028 / 3.028 = 1
The empirical formula is C5H8O4
The molar mass of this empirical formula is 132.12 g/mol
This means the empirical formula is also the molecular formula
The molecular formula is C5H8O4
