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)
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.