Question

Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to

BaO₂(s)+H2SO₄(aq)->BaSO₄(s)+H₂O₂(aq)

How many milliliters of 2.75 M H2SO4(aq) are needed to react completely with 52.7 g of BaO2(s)?

Answer 1

Number of moles of BaO2 = 52.7 g / 169.33 g/mol = 0.311 mole

From the balanced equation we can say that

1 mole of BaO2 requires 1 mole of H2SO4 so

0.311 mole of BaO2 will require 0.311 mole of H2SO4

Therefore, the number of moles of H2SO4 = 0.311

Moalrity = number of moles / volume of solution in L

2.75 = 0.311 / volume of solution in L

volume of solution in L = 0.311 / 2.75 = 0.113 L

1 L = 1000 mL

0.113 L = 113 mL

Therefore, the number of moles of H2SO4 required would be 113 mL