Solve the equation

Question

How many mL of 0.18 M H2SO4 solution are needed to react completely with 11.15 g of Fe2O3 in the following reaction?



Fe2O3(s) + 3H2SO4(aq) → Fe2 (SO4)3(aq) + 3 H2O(l)

Answer 1

Fe2O3(s) + 3 H2SO4(aq) → Fe2(SO4)3(aq) + 3 H2O(l)  Balanced equation

moles of Fe2O3 present = 11.15 g x 1 mole/159.69 g = 0.0700 moles Fe2O3

moles H2SO4 required to react = 0.0700 moles Fe2O3 x 3 moles H2SO4/mole Fe2O3 = 0.2100 moles H2SO4 needed

volume H2SO4 needed = 0.2100 moles H2SO4 x 1 L/0.18 moles = 1.17 liters = 1170 mls