Hi guys, im having some doubts getting this exercise: 20,0 g of iron (60% purity) are reacted with sulphuric acid (80 % pure) Iron (II) sulphate and hydrogen are formed: Fe + H2SO4 → H2 + FeSO4 1. Which is the limiting reactant? 2. How much Iron (II) sulphate will be obtained? 3. What volume (r.t.p) of H2 (g) will be obtained? 4. What volume would be obtained if the yield were just 80 %? 5. How much iron should be used in this case if the amount calculated in (2) were to be obtained= Info Ar(H)= 1 Ar(O)= 16 Ar (Fe)= 56 Molar volume (r.t.p) 24dm^3 So, Iron(II) Sulphate mass= 56 + 32 + (16x4) = 152 is that the iron sulphate obtained? answer to number 5 should the be: 152/0.8? please, im needing some help!