Use the standard reduction potentials to find the equilibrium constant for each of the following reactions at
Interpretation:
The equilibrium constant for each of the given chemical reactions is to be determined.
Concept introduction:
The standard cell potential of a particular cell is given as:
Here,
The relation between the cell potential
Here,
Answer to Problem 23QP
Solution:
(a)
(b)
(c)
Explanation of Solution
a)
This reaction can be written as two half-reactions, as shown below:
From table 19.1, the reduction potential of bromine is
The standard cell potential of the cell is given by the expression shown below:
Substitute the values:
Now, the relation between the cell potential
Here, the number of exchange of electrons is two;
Thus, the value of
Substitute the values of
Thus, the equilibrium constant of this reaction is
b)
This reaction can be written as two half-reactions, as shown below:
Fromtable 19.1, the reduction potential of cerium is
Now, the standard cell potential of a cell is given by the expression shown below:
Substitute the values of half-cell potentials to the above expression,
Now, the relation between the cell potential
Here, the number of exchange of electrons is two;
Thus, the value of
Substitute the values of
Thus, the equilibrium constant of this reaction is
c)
This reaction can be written as two halves reactions as follows:
From table 19.1, the reduction potential of manganese is
Now, the standard cell potential of a cell is given by the expression shown below:
Substitute the values of half-cell potential in the above expression,
Now, the relation between the cell potential
Here, the number of exchange of electrons is five;
Thus, the value of
Substitute the values of
Thus, the equilibrium constant of this reaction is
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Chapter 19 Solutions
Chemistry
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