We have to determine the molecular formula of a hydrocarbon, 0.460 g of which 0.477 g CO, 0.749 g CO2 and 0.460 g H2O upon combustion.
Empirical formula is a chemical formula that gives the relative proportions of elements in a compound but not the actual number of atoms of elements in a compound.
We will calculate the empirical formula through these steps:
Step 1: Find the mass of C and H using the given masses of CO, CO2 and H2O.
Step 2: Find the percentage of C and H in the compound.
Step 3: Dividing the percentages of C and H by their average atomic masses.
Step 4: Dividing the obtained numbers by the smallest number among them and rounding off to the nearest whole numbers to get the empirical formula.
When hydrocarbons are burned in a limited amount of air, both CO and CO2 form. When 0.460 g of a particular hydrocarbon was burned in air, 0.477 g of CO, 0.749 g of CO2, and 0.460 g of H2O were formed.
What is the empirical formula of the compound?