   Chapter 13, Problem 147AP ### Introductory Chemistry: A Foundati...

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

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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# oncentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe):msp;  2H ­ 2 O 2 ( a q )   2H 2 O ( l ) + O 2 ( g ) at volume of pure O 2 ( g ) , collected at 27  ° C and 764 to torr, would be generated by decomposition of 125 g of a 5 0.0 % by mass hydrogen peroxide solution?

Interpretation Introduction

Interpretation:

To interpret the volume of O2 gas evolved during the decomposition of H2 O2 solution.

Concept Introduction:

The balance equation of decomposition of H2 O2 helps to calculate mole ratio of reactant and product. Moles can be calculated with the help of mass and molar mass with the given formula:

Number of moles =MassMolar mass.

Explanation

Given information:

Temperature = 27°C

Pressure = 764 torr

Mass = 125 g (50.0 % by mass hydrogen peroxide solution)

The mass of hydrogen peroxide must be calculated with the given mass percentage which further changes to moles. The mole ratio of hydrogen peroxide and oxygen is 2:1 hence it gives moles of oxygen gas. At STP conditions; we need to change the moles to volume.

Molar mass of H2 O2 = 34.01 g/mol

Mass percentage of H2 O2 = 50.0 %

Hence, mass of H2 O2 = 125 g ×50100=62.5 g

Number of moles of H2 O2 = massmolar mass=62.5 g34.01 g/mol=1.84 mol

According to given balance equation, 2 mole of H2 O2 form 1 moles of O2 gas. Hence,

1.84 moles of H2O2×1 mol

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