
Calculate the standard cell potentials of galvanic cell in which the following reactions take place:
(i)
(ii)
Calculate the and equilibrium constant of the reactions
Answer
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Hint: The standard cell potential, and equilibrium constant of the reactions can be calculated using standard electrode potentials of the elements involved. The electrode potential cannot be obtained empirically. It is calculated using a reference hydrogen electrode.
Complete step by step solution:
Standard electrode potential is defined as the measures the individual potential of reversible electrode at standard state with ions at an effective concentration of 1mol at the pressure of 1 atm.
(i)
The formula of calculating cell potential is :
In the equation, cathode is cadmium with electrode potential , -0.40V, anode is chromium with electrode potential, -0.74V. Therefore, substituting the value in the above formula,
In a galvanic cell, where a spontaneous redox reaction drives the cell to produce an electric potential, Gibbs free energy must be negative, in accordance with the following equation:
Since we know the electrode potential, and number electrons involved in the reaction is 6 and value of faraday constant is 96500, Therefore, substituting the value in the above formula,
The formula for equilibrium constant is,
Equilibrium constant is .
(ii)
In the equation, cathode is silver with electrode potential , 0.80V, anode is iron with electrode potential, 0.77V. Therefore, substituting the value in the above formula,
Now Gibbs free energy will be:
The equilibrium constant is,
Note: The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium, a state approached by a dynamic chemical system after sufficient time has elapsed at which its composition has no measurable tendency towards further change.
Complete step by step solution:
Standard electrode potential
(i)
The formula of calculating cell potential is :
In the equation, cathode is cadmium with electrode potential , -0.40V, anode is chromium with electrode potential, -0.74V. Therefore, substituting the value in the above formula,
In a galvanic cell, where a spontaneous redox reaction drives the cell to produce an electric potential, Gibbs free energy
Since we know the electrode potential, and number electrons involved in the reaction is 6 and value of faraday constant is 96500, Therefore, substituting the value in the above formula,
The formula for equilibrium constant is,
Equilibrium constant is
(ii)
In the equation, cathode is silver with electrode potential , 0.80V, anode is iron with electrode potential, 0.77V. Therefore, substituting the value in the above formula,
Now Gibbs free energy will be:
The equilibrium constant is,
Note: The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium, a state approached by a dynamic chemical system after sufficient time has elapsed at which its composition has no measurable tendency towards further change.
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