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QuestionFind the empirical formula of a metal sulfide formed from 8.741 g of iron and 13.76 g of product mass.

Studdy Solution

STEP 1

Assumptions1. The initial mass of iron is8.741 g. The final mass of the metal sulfide is13.76 g3. The excess sulfur reacts completely with the iron to form the metal sulfide4. The difference in mass between the metal sulfide and the initial iron sample is the mass of sulfur in the compound

STEP 2

First, we need to find the mass of sulfur in the metal sulfide. We can do this by subtracting the initial mass of iron from the final mass of the metal sulfide.
Mass of ulfur=Final mass of metal sulfide−Initial mass of ironMass\, of\,ulfur = Final\, mass\, of\, metal\, sulfide - Initial\, mass\, of\, iron

STEP 3

Now, plug in the given values for the final mass of the metal sulfide and the initial mass of iron to calculate the mass of sulfur.
Mass of ulfur=13.76 g−8.741 gMass\, of\,ulfur =13.76\, g -8.741\, g

STEP 4

Calculate the mass of sulfur.
Mass of ulfur=13.76 g−8.741 g=.019 gMass\, of\,ulfur =13.76\, g -8.741\, g =.019\, g

STEP 5

Next, we need to convert the mass of iron and sulfur to moles. We can do this by dividing the mass by the atomic mass. The atomic mass of iron (Fe) is approximately55.85 g/mol, and the atomic mass of sulfur () is approximately32.06 g/mol.
Moles of Fe=Mass of Fe/Atomic mass of FeMoles\, of\, Fe = Mass\, of\, Fe / Atomic\, mass\, of\, FeMoles of =Mass of /Atomic mass of Moles\, of\, = Mass\, of\, / Atomic\, mass\, of\,

STEP 6

Now, plug in the given values for the mass of iron and sulfur and the atomic masses to calculate the moles of iron and sulfur.
Moles of Fe=8.741 g/55.85 g/molMoles\, of\, Fe =8.741\, g /55.85\, g/molMoles of =5.019 g/32.06 g/molMoles\, of\, =5.019\, g /32.06\, g/mol

STEP 7

Calculate the moles of iron and sulfur.
Moles of Fe=.741 g/55.85 g/mol=0.1565 molMoles\, of\, Fe =.741\, g /55.85\, g/mol =0.1565\, molMoles of =5.019 g/32.06 g/mol=0.1566 molMoles\, of\, =5.019\, g /32.06\, g/mol =0.1566\, mol

STEP 8

To find the empirical formula, we need to find the ratio of moles of iron to moles of sulfur. Since the numbers are very close, we can assume the ratio is11.
Ratio of Fe:S=11Ratio\, of\, Fe:S =11

STEP 9

Therefore, the empirical formula of the metal sulfide is Fe.

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