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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms: It decomposes upon contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams upon contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the action of an acid on an alkaline earth metal peroxide, such as barium peroxide.

BaO 2 ( s ) + 2 HCl ( a q ) H 2 O 2 ( a q ) + BaCl 2 ( a q )

What amount of hydrogen peroxide should result when 1.50 g of barium peroxide is treated with 25.0 mL of hydrochloric acid solution containing 0.0272 g of HCI per mL?

Interpretation Introduction

Interpretation:

The amount of hydrogen peroxide formed should be calculated.

Concept Introduction:

The expected or theoretical yield of the product depends on the limiting reactant of the reaction. Limiting reactant is the reactant that limits the mass of product formed in the reaction. The reactant other than limiting reactant is known as excess reactant.

Explanation

The balanced chemical reaction is as follows:

BaO2(s)+2HCl(aq)H2O2(aq)+BaCl2(aq)

Mass of barium peroxide is 1.50 g. The volume of hydrochloric acid is 25 mL and 0.0272 g of HCl is present in 1 mL of HCl solution thus, mass of HCl will be m=0.0272 g/mL×25 mL=0.68 g

To determine the mass of hydrogen peroxide, first determine the limiting reactant as follows:

Calculate the number of mole of BaO2 as follows:

n=mM

Molar mass of BaO2 is 169.33 g/mol thus,

n=1.50 g169.33 g/mol=0.0088 mol

From the balanced chemical reaction, 1 mol of BaO2 gives 1 mol of hydrogen peroxide thus, 0.0088 mol of BaO2 will give 0

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