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.

a. determine the empirical and molecular formulas of this compound.
b. empirical formula: molecular formula:
c. write a balanced chemical equation for this reaction. do not include phases.

The molecular formula of the compound =

The empirical formula of the compound =

The balanced chemical equation for this reaction:

Explanation:

Compound that is 27.87% P and 72.13% S by mass and has a molar mass of 444.56 g/mol.

Molar mass of compound = 444.56 g/mol

Number of phosphorus atom = x

Number of sulfur atom = y

Atomic  mass of phosphorus  31 g/mol

Atomic mass of sulfur = 32 g/mol

Percentage of element in compound :

Phosphorus :

x = 4

Sulfur :

y = 10

The molecular formula of the compound =

Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.

The empirical formula of the compound =

The balanced chemical equation for this reaction:

im pretty sure its b