
Calculate the equilibrium constant for the
(a) A piece of iron is placed in a 1.0 M solution of NiCl2(aq).
(b) A copper wire is placed in a 1.0 M solution of Pb(NO3)2(aq).
(a)

Interpretation: The equilibrium constant for the redox reaction should be determined along with by using the value of equilibrium constant identifies whether the reaction occurs or not.
A piece of iron is placed in a 1.0 M solution of
Concept introduction: The equilibrium constant
Answer to Problem 13.43PAE
Solution:
Kc=0.4407 and reaction will occur.
Explanation of Solution
An iron piece is placed in
Anode:
Cathode:
Formula used:
where,
n =number of electrons
Kc= equilibrium constant
Calculation: Cathode and anode is identified from above equation
The value of equilibrium constant is positive which implies product is more and reaction will occur.
Thus, reaction will occur.
(b)

Interpretation: The equilibrium constant for the redox reaction should be determined along with by using the value of equilibrium constant identifies whether the reaction occurs or not.
A copper wire is placed in a 1.0 M solution of
Concept introduction: The equilibrium constant
Answer to Problem 13.43PAE
Solution:
Kc=1.175×10-16 and reaction will not occur.
Explanation of Solution
Anode:
Cathode:
Formula used:
where,
n =number of electrons
Kc= equilibrium constant
Calculation: Cathode and anode is identified from the above equation.
In this case, the value of equilibrium constant is so small and reactants predominates over products.
Thus, reaction will not occur.
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Chapter 13 Solutions
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