How many moles of iron atoms are in
22.37 g of iron (II) sulfide, FeS?
mols FeS = grams/molar mass = ?
There is 1 mol Fe in 1 mol FeS.
To find the number of moles of iron atoms in 22.37 g of iron (II) sulfide, FeS, we need to follow these steps:
Step 1: Determine the molar mass of iron (II) sulfide, FeS.
The molar mass of FeS can be calculated by adding up the atomic masses of its constituent elements. The atomic mass of iron (Fe) is 55.845 g/mol, and the atomic mass of sulfur (S) is 32.06 g/mol. So, the molar mass of FeS is:
(1 × atomic mass of Fe) + (1 × atomic mass of S)
= (1 × 55.845 g/mol) + (1 × 32.06 g/mol)
= 87.905 g/mol.
Step 2: Convert the given mass of FeS to moles using the molar mass.
To convert grams to moles, we divide the given mass by the molar mass:
moles = mass (in grams) / molar mass
moles = 22.37 g / 87.905 g/mol.
Calculating this division gives us the number of moles of FeS:
moles = 0.2542 mol.
Step 3: Determine the mole ratio of iron atoms to FeS.
From the chemical formula FeS, we can see that there is one mole of iron atoms (Fe) for every one mole of iron (II) sulfide (FeS). Therefore, the number of moles of iron atoms is also 0.2542 mol.
So, there are 0.2542 moles of iron atoms in 22.37 g of iron (II) sulfide, FeS.