33 grams of iron metal are dissolved in 50 mL if 6 M hydrochloric acid according to the following reaction:?

Molar mass of Fe = 55.85 g/mol

Fe(s) + 2HCl(aq) → FeCl₂(aq) + H₂(g)
OR: Mole ratio Fe : HCl = 1 : 2

Initial number of moles of Fe = (33 g) / (55.85 g/mol) = 0.5909 mol
Initial number of moles of HCl = (6 mol/L) × (50/1000 L) = 0.3 mol

For complete reaction of HCl :
Number of moles of Fe needed = (0.3 mol) × (1/2) = 0.15 mol < 0.5909 mol
Hence, Fe is in excess, and HCl is the limiting reactant (completely reacts)

According to the above equation, mole ratio HCl : H₂ = 2 : 1
Number of moles of HCl reacted = 0.3 mol
Number of moles of H₂ produced = (0.3 mol) × (1/2) = 0.15 mol

Volume of H₂ produced at STP = (22.4 L/mol) × (0.15 mol) = 3.36 L
Volume of H₂ produced at RTP = (24 L/mol) × (0.15 mol) = 3.6 L

For this same question,it is asking what is the excess reactant and how much excess is left over^^