1. Write the Balanced Chemical Equation:

The reaction between iron (Fe) and sulfur (S) produces iron sulfide (FeS):

Fe + S → FeS

2. Determine the Molar Masses:

* Iron (Fe): 55.845 g/mol

* Sulfur (S): 32.065 g/mol

3. Calculate Moles of Sulfur:

* Moles of sulfur = mass of sulfur / molar mass of sulfur

* Moles of sulfur = 16 g / 32.065 g/mol

* Moles of sulfur ≈ 0.5 mol

4. Use the Mole Ratio from the Balanced Equation:

* The balanced equation shows a 1:1 mole ratio between iron and sulfur. This means for every 1 mole of sulfur, you need 1 mole of iron.

5. Calculate Moles of Iron Needed:

* Since the mole ratio is 1:1, you need approximately 0.5 moles of iron.

6. Calculate the Mass of Iron:

* Mass of iron = moles of iron * molar mass of iron

* Mass of iron ≈ 0.5 mol * 55.845 g/mol

* Mass of iron ≈ 27.92 g

Therefore, approximately 27.92 grams of iron are needed to react with 16 grams of sulfur.