Question

The empirical formula for a compound is CH2O, and the molar mass is 180.2 g/mol. Which is the molecular formula for this compound?A) C6H12O6
B) C7H16O5
C) C8H20O4
D) C3H6O3

Answer 1

Answer : The correct option is, (A) $C_{6}H_{12}O_6$

Explanation :

Empirical formula : It is the simplest form of the chemical formula which depicts the whole number of atoms of each element present in the compound.  

Molecular formula : it is the chemical formula which depicts the actual number of atoms of each element present in the compound.  

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is :

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

As we are given that the empirical formula of a compound is $CH_2O$ and the molar mass of compound is, 180.2 gram/mol.

The empirical mass of $CH_2O$ = 1(12) + 2(1) + 1(16) = 30 g/eq

$n=\frac{\text{molecular mass}}{\text{empirical mass}}$

$n=\frac{180.2}{30}=6$

Molecular formula = $(CH_2O)_n=(CH_2O)_6=C_{6}H_{12}O_6$

Thus, the molecular formula of the compound will be, $C_{6}H_{12}O_6$