Question 1 Report
A compound has an empirical formular CH2O and molecular mass of 90.
[H = 1.00, C = 12.0, O = 16.0]
The empirical formula of the compound is CH2O, which indicates that for every carbon atom there are two hydrogen atoms and one oxygen atom. The molecular mass of the compound is 90, which is the sum of the atomic masses of all the atoms in the molecule. Let's calculate the molecular formula of the compound using this information. The empirical formula mass of CH2O is: (1 x 12.0) + (2 x 1.00) + (1 x 16.0) = 30.0 g/mol To calculate the molecular formula, we need to divide the molecular mass by the empirical formula mass: Molecular formula mass / Empirical formula mass = n 90.0 / 30.0 = 3 Therefore, the molecular formula of the compound is three times the empirical formula: C3H6O3 So, the correct option is C3H6O3.