Question

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

Answer 1

BaO₂ + H₂SO₄ ⇒ BaSO₄ + H₂O₂
169g : 98g
23.1g : mx

mx = [23.1*98g]/169g ≈ 13.4g
Mr = 98g/mol

n = 13.4g/98g/mol ≈ 0.14mol

Cm = 4.5M
n = 0.14mol

V = 0.14mol/4.5mol/dm³ ≈ 0.031L = 31mL

Answer 2

31.43 ml of sulfuric acid is needed to react with 23.1 g of barium peroxide.

Step-by-step explanation:

For the reaction:

BaO₂(s) + H₂SO₄(aq) ⇒ BaSO₄(s) + H₂O₂(aq)

We need 1 mole of BaO₂ to react with 1 mole of H₂SO₄ and then forming 1 mole of BaSO₄ and 1 mole of H₂O₂.

We know that 4.5 M solution of H₂SO₄ means 4.5 moles of H₂SO₄ in 1000 ml of solution.

Then,

23.1 g BaO₂ ×
`(1 mole_(BaO_2))/(163.33g_(BaO_2))` ×
`\frac{1 mole_{H_(2)SO_(4)}}{1mole_(BaO_2)}` ×
`\frac{1000ml}{4.5 mole_{H_(2)SO_(4)}}` = 31.43 ml H₂SO₄