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QuestionDetermine the empirical formula of a metal sulfide formed from 8.741 g of iron and 13.76 g of sulfide. Enter as Fe, S.

Studdy Solution

STEP 1

Assumptions1. The initial mass of iron is8.741 g. . The final mass of the metal sulfide is13.76 g.
3. The metal sulfide is formed by the reaction of iron with sulfur.
4. The excess sulfur ensures that all the iron is converted to the metal sulfide.

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 each element to moles. We can do this by dividing the mass of each element by its molar mass. The molar mass of iron (Fe) is55.845 g/mol and that of sulfur () is32.06 g/mol.
Moles of Iron=Mass of Iron/Molar mass of IronMoles\, of\, Iron = Mass\, of\, Iron / Molar\, mass\, of\, IronMoles of ulfur=Mass of ulfur/Molar mass of ulfurMoles\, of\,ulfur = Mass\, of\,ulfur / Molar\, mass\, of\,ulfur

STEP 6

Now, plug in the given values for the mass of iron, the mass of sulfur, the molar mass of iron, and the molar mass of sulfur to calculate the moles of iron and sulfur.
Moles of Iron=8.741 g/55.845 g/molMoles\, of\, Iron =8.741\, g /55.845\, g/molMoles of ulfur=5.019 g/32.06 g/molMoles\, of\,ulfur =5.019\, g /32.06\, g/mol

STEP 7

Calculate the moles of iron and sulfur.
Moles of Iron=.741 g/55.845 g/mol=0.1565 molMoles\, of\, Iron =.741\, g /55.845\, g/mol =0.1565\, molMoles of ulfur=5.019 g/32.06 g/mol=0.1565 molMoles\, of\,ulfur =5.019\, g /32.06\, g/mol =0.1565\, mol

STEP 8

The empirical formula is the simplest whole number ratio of the moles of each element. In this case, the ratio of moles of iron to moles of sulfur is11. Therefore, the empirical formula of the metal sulfide is Fe.
empirical formula =Fe= Fe

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