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 4.00 M H2SO4(aq) are needed to react completely with 32.5 g of BaO2(s)?

Answer 1

Given Chemical reaction

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

In above reaction , 1 mole of BaO2 reacts with 1 mole of H2SO4 to produce 1 mole of BaSO4(s) and 1 mole of H2O2(aq)

So we can say

Moles of BaO2 : Moles of H2SO4 = 1:1 ---------------(1)

Using above information now we can say that every mole of BaO2 to react , we need an equal amount of moles of H2SO4.

We know No. of Moles = (Given mass in gram)/ Molecular Mass

Moles of BaO2 = (32.5g)/169.33 g/mol = 0.192 mol

Using relationship (1) , we need 0.192 mol of H2SO4

From question,

4.00M of H2SO4 means we have 4 moles in 1.0 Litre

So 0.192 mole ------------ ( 1.0 Litre* 0.192 mole)/ 4 mol = 0.048Litre = 0.048*1000 ml = 48 Millilitres

So 48 Millilitres of 4.00 M H2SO4(aq) are needed to react completely with 32.5 g of BaO2(s)?