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:

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

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