   Chapter 20.7, Problem 1.2ACP

Chapter
Section
Textbook Problem

What is the overall equilibrium constant for the disproportionation reaction of Cl2 in water?

Interpretation Introduction

Interpretation:

The equilibrium constant K for the reaction has to be determined.

Concept introduction:

• If the oxidation number of an element increases then the element is said to be oxidized and the oxidation number value of decreases for an element which is reduced.
• Ecell0=Ecathode0Eanode0
• In cathode, reduction reaction will take place and in an anode oxidation reaction will happen.
• The equation to determine the equilibrium constant K by using the value of E0 is,

lnK=nE00.0257     n is the number of electrons involved in the reaction

Explanation

The balanced chemical reaction equation for the given reaction is,

Cl2(g)+2H2O(l)HClO(aq)+H3O(aq)++Claq

Oxidation number for each element involved in the reaction can be written as follows,

Cl2(g)0+2H2O(l)0HClO(aq)+1+12+H3O(aq)++Claq1

Reduction reaction in cathode is,

Cl2+2e2Cl                            Ecathode0=1.36V

Oxidation reaction in anode is,

Cl2+2H2O2HClO+2H++2e                    Eanode0=1

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Find more solutions based on key concepts 