How many grams of FeS are formed from 7.62g of Fe reacted with excess S? Fe+Sarrow FeS 3.829 7.629 11.979 11.49

To determine the amount of FeS formed from 7.62g of Fe reacted with excess S, we need to use stoichiometry.Given information:- Reaction: Fe + S → FeS- Mass of Fe: 7.62g- Excess S (sulfur)Step 1: Calculate the molar mass of Fe and FeS.Molar mass of Fe = 55.85 g/molMolar mass of FeS = 87.91 g/molStep 2: Calculate the moles of Fe.Moles of Fe = Mass of Fe / Molar mass of FeMoles of Fe = 7.62g / 55.85 g/mol = 0.136 molStep 3: Calculate the moles of FeS formed.Since the reaction is 1:1, the moles of FeS formed will be the same as the moles of Fe.Moles of FeS = 0.136 molStep 4: Calculate the mass of FeS formed.Mass of FeS = Moles of FeS × Molar mass of FeSMass of FeS = 0.136 mol × 87.91 g/mol = 11.97gTherefore, the correct answer is 11.97g.