Question

A 13.58 g sample of a compound contains 8.67 g of iron, Fe, 1.60 g of phosphorus, P, and oxygen, O. Calculate the empirical
formula for the compound.

Answer 1

Answer:

$Fe_3PO_4$

Explanation:

To do this, we find the moles of each element. We get around 0.155 moles of Fe, 0.051 moles of P, and 0.206 moles of O. We then divide each one by the smallest one (which is 0.051 moles of P). We then get 3 for Fe, 1 for P, and 4 for O. This correlates to the empirical formula of the compound.

Answer 2

The empirical formula for the compound is $Fe_3PO_4$ if a 13.58 g sample of a compound contains 8.67 g of iron, Fe, 1.60 g of phosphorus, P, and oxygen, O.

What is the empirical formula?

An empirical formula tells us the relative ratios of different atoms in a compound.

We need to calculate the number of moles:

Given data:

Mass of iron - 8.67 g

Mass of phosphorus -1.60 g

Mass of oxygen -3.31 g

Moles of iron - $\frac{mass}{molar \;mass}$

Moles of iron - $\frac{8.67 g}{56 g/mol}$

0.15 mole

Moles of phosphorus $-\frac{mass}{molar \;mass}$

Moles of phosphorus -  $\frac{1.60 g}{31 g/mol}$

0.051 moles

Moles of oxygen -$\frac{mass}{molar \;mass}$

Moles of oxygen - $\frac{3.31 g}{16 g/mol}$

0.20 moles

Dividing each mole using the smallest number that is divided by 0.051 moles.

Fe:P:O :: 3:1:4

The empirical formula for the compound is $Fe_3PO_4$.

Learn more about empirical formula here:

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