The empirical formula of a compound is CH2O and the molecular mass is 180. What is the molecular formula of the compound?
http://www.ausetute.com.au/empirical.html
To find the molecular formula of a compound given its empirical formula and molecular mass, you need to determine the ratio between the empirical formula mass and the molecular mass.
Step 1: Calculate the empirical formula mass:
The empirical formula of the compound is CH2O, which consists of 1 carbon (C) atom, 2 hydrogen (H) atoms, and 1 oxygen (O) atom.
The atomic masses are:
C = 12.01 g/mol
H = 1.01 g/mol
O = 16.00 g/mol
Therefore, the empirical formula mass is:
(1 × 12.01) + (2 × 1.01) + (1 × 16.00) = 12.01 + 2.02 + 16.00 = 30.03 g/mol
Step 2: Calculate the ratio between the empirical formula mass and the molecular mass:
The given molecular mass is 180.
Ratio = Molecular Mass / Empirical Formula Mass
Ratio = 180 g/mol / 30.03 g/mol
Ratio ≈ 5.99
Step 3: Multiply the subscripts of the empirical formula by the ratio obtained:
The subscripts in the empirical formula are C1H2O1.
Multiplying each subscript by approximately 6 gives:
C6H12O6
Therefore, the molecular formula of the compound is C6H12O6.