Question

A 3.78-gram sample of iron metal is reacted with sulfur to produce 5.95 grams of iron sulfide. Determine the empirical formula of this compound.

Answer 1

Answer:

The answer to your question is FeS₃

Explanation:

Data

mass of Fe = 3.78g

mass of S = 5.95 g

mass of FeS

Chemical Balanced Reaction

                           Fe   +   S     ⇒    FeS

Process

1.- Convert the grams to moles

For Iron

                              55.85g of Fe --------------  1 mol

                               3.78 g of Fe -----------  x

                               x = (3.78 x 1) / 55.85

                               x = 0.0677 moles

For Sulfur

                              32 g of S ------------------- 1 mol

                               5.95 g     ------------------  x

                               x = (5.95 x 1)/32

                               x = 0.185 moles

2.- Divide by the lowest number of moles

Iron = 0.0677 /0.0677 = 1

Sulfur = 0.185 /0.0677 = 2.73 ≈  3

3.- Write the empirical formula

                                 FeS₃                                

Answer 2

Answer:FeS

Explanation:

Mass of sulphur=5.95-3.78=2.17g

Fe S

3.78/56. 2.17/32

0.0675/0.0675. 0.0678/0.0675

1:1

Empirical formula=Fe1S1=FeS