Explanation The given cell reaction is as follows: 2H 2 O 2 (l) → 2H 2 O(l)+O 2 (g) The two half-reactions are as follows: H 2 O 2 (aq)+2H + (aq)+2e - → 2H 2 O(l) E o = +1 .78 V -(1) O 2 (g)+2H + (aq)+2e - → H 2 O 2 (aq) E o = +0 .70 V -(2) In the activity series, which is given in table 19.1, it is clear that the reaction equation (2) lies in the bottom as compared to reaction (1), which means that O 2 is a better reducing agent than H 2 O 2 . Therefore, the reaction (2) will occur at the anode while reaction (1) will occur at the cathode. The standard reduction potential for the cell reaction can be calculated as follows: E o = E cathode o -E anode o =1

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ISBN: 9780135214756

Author: Robinson

Publisher: PEARSON

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Chapter 19, Problem 19.115SP

Interpretation Introduction

Interpretation:

The equilibrium constant for the given reaction is to be determined.

Concept introduction:

The standard reduction potential for a given cell can be defined as the tendency of a chemical species to get reduced and is measured in volts provided that the conditions are standard.

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Chapter 19, Problem 19.114SP

Chapter 19, Problem 19.116SP

Chapter 19 Solutions

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The equilibrium constant for the given reaction is to be determined. Concept introduction: The standard reduction potential for a given cell can be defined as the tendency of a chemical species to get reduced and is measured in volts provided that the conditions are standard.

Solution Summary: The author explains that the equilibrium constant for the given reaction is 3.47times 1036. The reaction equation (2) lies in the bottom as compared to reaction (1).

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Interpretation: The equilibrium constant for the given reaction is to be determined. Concept introduction: The standard reduction potential for a given cell can be defined as the tendency of a chemical species to get reduced and is measured in volts provided that the conditions are standard.

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Chapter 19 Solutions

Interpretation:

The equilibrium constant for the given reaction is to be determined.

Concept introduction:

The standard reduction potential for a given cell can be defined as the tendency of a chemical species to get reduced and is measured in volts provided that the conditions are standard.