CHAPTER 19. QUANTITATIVE ASPECTS OF CHEMICAL CHANGE 19.2
n=Mm
nC =^39 ,^9 g
12 , 0 g·mol−^1
= 3, 325 mol
nH =^6 ,^7 g
1 , 01 g·mol−^1
= 6, 6337 mol
nO =^53 ,^4 g
16 , 0 g·mol−^1
= 3, 3375 mol
Step 3:Find the empirical formula
C : H : O
3 , 325 : 6 , 6337 : 3 , 3375
1 : 2 : 1
Empirical formula is CH 2 O
Step 4:Find the molecular formula
The molar mass of acetic acid using the empirical formula is 30 , 02 g·
mol−^1. However the question gives the molar mass as 60 , 06 g·mol−^1.
Therefore the actual number of moles of each element must be double
what it is in the empirical formula (^6030 ,,^0602 = 2). The molecular formula
is therefore C 2 H 4 O 2 or CH 3 COOH
Example 11: Waters of crystallisation
QUESTION
Aluminium trichloride (AlCl 3 ) is an ionic substance that forms crystals in the solid
phase. Water molecules may be trapped inside the crystal lattice. We represent this
as: AlCl 3 ·nH 2 O. Carine heated some aluminium trichloride crystals until all the
water had evaporated and found that the mass after heating was 2 , 8 g. The mass
before heating was 5 g. What is the number of moles of water molecules in the
Chemistry: Chemical change 347