Question

How many milliliters of 5.00 M H2SO4(aq) are needed to react completely with 49.5 g of BaO2(s)?

Answer 1

Balanced equation is

BaO2 + H2SO4 -----> BaSO4 + H2O2

number of moles of BaO2 = 49.5 g / 169.33 g/mol = 0.292 mole

from the balancced equation we can say that

1 mole of BaO2 requires 1 mole of H2SO4 so

0.292 mole of BaO2 will require 0.292 mole of H2SO4

molarity of H2SO4 = number of moles of H2SO4 / volume of solution in L

5.00 M = 0.292 mole / volume of solution in L

volume of solution in L = 0.292 / 5.00 = 0.0584 L

1 L = 1000 mL

0.0584 L = 58.4 mL

Therefore, the volume of HSO4 required would be 58.4 mL