A compound contains C, H and O as the elements. A 20.0 g-sample is comprised of 1.34 g H and also 8.00g of C. What is the empirical formula of the compound?

Explanation:

Total mass of sample = 20 g

mass of H = 1.34 g

mass of C = 8.00 g

mass of O = 20 - ( 8 + 1.34 )

= 10.66 g

no of atom of H in 1.34 g

= 1.34 / atomic weight of H .

= 1.34 / 1 = 1.34

no of atom of C in 8.00 g

= 8.00 / atomic weight of C

= 8.00 / 12 = .67

no of atom of O in 10.66 g

= 10.66 / atomic weight of O .

= 10.66 / 16 = .67

Ratio of no of atoms of H , C , O in the compound

= 1.34 : 0.67 : 0.67

Divide all by .67  

= 2 : 1 : 1  ( integral ratio )

Hence empirical formula of compound

= CH₂O.

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.

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