A115.0-g sample of iron (fe) is burned in excess oxygen. the result is a pure solid with a mass of 164.5 grams. what is the empirical formula of the solid?

The empirical formula is Fe2O3

Explanation:

Step 1: Data given

Mass of the iron sample = 115.0 grams

Mass of the pure solid = 164.5 grams

Molar mass of Fe = 55.845 g/mol

Molar mass of O = 16 g/mol

Step 2: Calculate mass of oxygen

mass of oxygen = mass of solid - mass of iron

Mass of oxygen = 164.5 grams - 115.0 grams

MAss of oxygen = 49.5 grams

Step 3: Calculate moles of oxygen

Moles oxygen = mass oxygen / molar mass oxygen

Moles oxygen = 49.5 grams / 16.0 g/mol

Moles oxygen = 3.09 moles

Step 4: Calculate moles of Fe

Moles Fe = mass Fe / molar mass Fe

Moles Fe = 115.0 grams / 55.845 g/mol

Moles Fe = 2.06 moles

Step 5: Calculate mol ratio

We divide by the smallest amount of moles

O: 3.09/2.06 = 1.5

Fe: 2.06 / 2.06= 1

This means for 1  mol Fe we have 1.5 mol O  OR for each 2 moles Fe we have 3 moles O.

The empirical formula is Fe2O3

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be