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To find the empirical formula of the compound, we first need to determine the number of moles of each element.
The molar mass of phosphorus (P) is 30.97 g/mol, and the molar mass of fluorine (F) is 19.00 g/mol.
Number of moles of phosphorus:
0.76 g / 30.97 g/mol = 0.025 mol
Number of moles of fluorine:
0.324 g / 19.00 g/mol = 0.017 mol
Next, we need to determine the ratio of the elements in the compound by dividing the number of moles of each element by the smallest number of moles:
Phosphorus: 0.025 mol / 0.017 mol = 1.47
Fluorine: 0.017 mol / 0.017 mol = 1
The ratio of phosphorus to fluorine in the compound is approximately 1.47:1. To get whole numbers, we can round these values:
Phosphorus: 1.47 ≈ 1
Fluorine: 1
So, the empirical formula of the compound is PF.