Answer:
1. The empirical formula is CH2O
2. The molecular formula is C6H12O6
Explanation:
Data obtained from the question include:
Carbon (C) = 48.38g
Hydrogen (H) = 8.12g
Oxygen (O) = 53.5g
Molar Mass of the compound = 180.15 g/mol
1. The empirical formula can be obtained as follow:
C = 48.38g
H = 8.12g
O = 53.5g
Divide each by their molar mass
C = 48.38/12 = 4.032
H = 8.12/1 = 8.12
O = 53.5/16 = 3.344
Next, divide by the smallest
C = 4.032/3.344 = 1
H = 8.12/3.344 = 2
O = 3.344/3.344 = 1
Therefore, the empirical formula is CH2O.
2. The molecular formula is mostly a multiple of the empirical i.e
Molecular formula => [CH2O]n
Now, we need to find the value of 'n' in order to obtain the molecular formula.
From the question given, we were told that the molar mass of the compound is 180.15 g/mol. With this information, the molecular formula can be obtained as follow:
[CH2O]n = 180.15
[12 + (2x1) + 16]n = 180.15
[12 + 2 + 16]n = 180.15
30n = 180.15
Divide both side by the coefficient of n i.e 30
n = 180.15/30
n = 6
Therefore, the Molecular formula is
=> [CH2O]n
=> [CH2O]6
=> C6H12O6
