Question

Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to the reaction BaO2(s)+H2SO4(aq)⟶BaSO4(s)+H2O2(aq) How many milliliters of 4.00 M H2SO4(aq) are needed to react completely with 32.7 g BaO2(s)?

Answer 1

The answer to your question is: Volume = 15.2 ml

Step-by-step explanation:

Data

H2SO4 4M = ?

BaO2 = 32.7 g

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

MW BaO2 = 137 + 32 = 169 g

MW H2SO4 = 2 + 32 + 64 = 98 g

169 g of BaO2 ----------------- 98 g of H2SO4

32.7 g of BaO2 -------------- x

x = (32.7 x 98)/ 169

x = 18.99 ≈ 19 g of H2SO4

Density of H2SO4 = 1.25 g/lml

Volume = mass / density

Volume = 19 g / 1.25 g/ml

Volume = 15.2 ml