Ferrophosphorus (fe2p) reacts with pyrite (fes2), producing iron (ii) sulfide and a compound that is 27.87% p and 72.13% s by mass and has a molar mass of 444.56 g/mol. determine the empirical and molecular formulas of the compound.

The empirical and molecular formula for the formed compound is and respectively.

Explanation:

We are given:

Percentage of P = 27.87 %

Percentage of S = 72.13 %

Let the mass of compound be 100 g. So, percentages given are taken as mass.

Mass of P = 27.87 g

Mass of S = 72.13 g

To formulate the empirical formula, we need to follow some steps:

Moles of Phosphorus =

Moles of Sulfur =

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.899 moles.

For Phosphorus =

For Sulfur =

The ratio of P : S = 1 : 2.5

Converting the mole ratio into whole number by multiplying it by '2'

Now, the ratio becomes,   P : S = 2 : 5

The empirical formula of the compound is

The equation used to calculate the valency is:

We are given:

Mass of molecular formula = 444.56 g/mol

Mass of empirical formula = 222 g/mol

Putting values in above equation, we get:

Multiplying this valency by the subscript of every element of empirical formula, we get:

Hence, the empirical and molecular formula for the formed compound is and respectively.

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fe 55.85 g/mol and h2o 18.02 g/mol.