If a laboratory analysis of the mineral aegirine yields 10.0% na, 24.2% fe, 24.3% si, and 41.5% o, what is the empirical formula of the compound?

To make it easier, assume that we have a total of 100 g of aegirine. Hence, we have 10g of Na, 24.2g of Fe, 24.3g of Si and 41.5g of O. Know we will convert each of these masses to moles by using the atomic masses of Na, Fe, Si, and O:

Now, we will divide all the mole numbers by the smallest among them and get the number of atoms in the mineral:

Na = 0.43/0.43 = 1

Fe = 0.43/0.43 = 1

Si = 0.86/0.43 = 2

O = 2.59/0.43 = 6

So, the empirical formula of the compound NaFeSi2O6

explanation:

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