A 22.4 g sample of iron is allowed to react with 76.3 g of sulfuric acid.?

Question

Fe(s) + H2SO4(aq)----> FeSO4(aq) + H2(g)

(a) How many liters of hydrogen measured at STP can be produced?
(b) Calculate the number of moles of excess reagent remaining at the end of the reaction.

Answer 1

22.4/55.85 = 0.4010743 M Fe
76.3/(2*1.008 + 32.07 + 4*16) = 0.7778888 M H2SO4
(a) 0.4010743*22.4 = 8.984064 ≈ 9 L
(b) 0.7778888 - 0.4010743 = 0.3768145 M H2S04