The formula for rust can be represented by Fe2O3. How many moles of Fe are present in 27.6 g of the compound?

Mass=moles/atomic mass of fe2o3

mols Fe2O3 = grams Fe2O3/molar mass Fe2O3

Then there are 2 mols Fe for every 1 mol Fe2O3.

To find the number of moles of Fe in a given mass of Fe2O3, we first need to calculate the molar mass of Fe2O3.

To calculate the molar mass of Fe2O3, we add the atomic masses of the elements present in the compound, Fe and O. The atomic mass of Fe is 55.845 g/mol, and the atomic mass of O is 16.00 g/mol.

Therefore, the molar mass of Fe2O3 is:

Molar mass of Fe: 55.845 g/mol
Molar mass of O: 16.00 g/mol

Molar mass of Fe2O3 = (2 * Molar mass of Fe) + (3 * Molar mass of O)
= (2 * 55.845 g/mol) + (3 * 16.00 g/mol)
= 111.69 g/mol + 48.00 g/mol
= 159.69 g/mol

Now, using the molar mass of Fe2O3, we can calculate the number of moles of Fe in 27.6 g of the compound using the formula:

Number of moles = Mass of sample / Molar mass

Number of moles of Fe = 27.6 g / 159.69 g/mol

Calculating this, we find:

Number of moles of Fe = 0.173 moles

Therefore, there are approximately 0.173 moles of Fe present in 27.6 g of Fe2O3.