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:

answer : a model is often used to explain and make things easier to understand when any scientific topic needs to be demonstrated and explained.

as in this case where a scientist wants to use a model to present the results of his detailed scientific investigation. he should do it as it will him to make the audience understand the concept in a much better way. also, it can be changed according to new scientific understandings.

2b2t

explanation:

2b2t