o 6/30/2016 1 1:55 PM O 5.5/10 6/29/2016 1 1:57 PM Gradebook Print CalculatorPer

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o 6/30/2016 1 1:55 PM O 5.5/10 6/29/2016 1 1:57 PM Gradebook Print CalculatorPeriodic Table - Question 15 of 25 Map da General Chemistry 4th Edition University Science Books presented by Sapling Learning Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to Ba02(s) + H2SO4(aq) BaSO4(s) + H2O2(aq) How many milliliters of 3.50 M H2SO4(aq) are needed to react completely with 64.3 g of BaO2(s)? Number mL O Previous & Give Up & View Solution O Check Answer Next Exit Y Hint

Explanation / Answer

no of moles of BaO2 = 64.3 g / 169.3258 g/mol = 0.3797 mol

given reaction is balanced reaction

from this it is clear that one mole of BaO2 required 1 mole of H2SO4 to react completely

accordingly 0.3797 mole of BaO2 required 0.3797 mole of H2SO4

volume of H2SO4 required = moles of H2SO4 / molarity of H2SO4 = 0.3797 mol / 3.5 M

= 0.1084L

= 108.4 mL

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