a sample of anhydrous copper 2 sulphate contains 6.54g copper 3.2g sulphur and 6.4g oxygen determine the empirical formula of the compound (c=64.0,o=16,s=32)

1 answer

To determine the empirical formula, we need to find the ratio of the elements present in the compound.

1. Convert the masses of each element to moles using their molar masses:

Copper: 6.54 g / 63.55 g/mol = 0.103 mol
Sulfur: 3.2 g / 32.06 g/mol = 0.100 mol
Oxygen: 6.4 g / 16.00 g/mol = 0.400 mol

2. Divide each mole value by the smallest one to get the mole ratio:

Copper: 0.103 mol / 0.100 mol = 1.03
Sulfur: 0.100 mol / 0.100 mol = 1.00
Oxygen: 0.400 mol / 0.100 mol = 4.00

3. If necessary, adjust the ratios to the nearest whole number:

Copper: 1.03 ≈ 1
Sulfur: 1.00 ≈ 1
Oxygen: 4.00 ≈ 4

The empirical formula of the compound is therefore CuSO4.