A nickel-cadmium electrochemical cell functions according to the following reaction:
Cd+ Ni2+ → Cu2+ + Ni
What is the standard cell potential of a nickel-cadmium electrochemical cell?
To determine the standard cell potential of a nickel-cadmium electrochemical cell, we need to know the standard reduction potentials of the involved half-reactions. However, the provided reaction Cd+ Ni2+ → Cu2+ + Ni seems to be incorrect because it involves the reduction of both Cd and Ni2+ ions, which are unlikely to occur simultaneously.
If you have the correct and balanced half-reactions for the cell, please provide them so that I can calculate the standard cell potential for you.
To determine the standard cell potential (E°cell) of a nickel-cadmium (Ni-Cd) electrochemical cell, we need to look at the reduction potentials (E°red) of each half-reaction involved in the cell.
The given reaction:
Cd + Ni2+ → Cu2+ + Ni
We have the reduction half-reaction:
Cd2+ + 2e- → Cd (E°red = -0.40 V) -- (1)
And the oxidation half-reaction:
Ni → Ni2+ + 2e- (E°red = ?) -- (2)
To find the oxidation reduction potential for the Ni half-reaction, we can use table of standard reduction potentials. According to the table, the reduction potential for the Ni2+/Ni half-reaction is -0.25 V.
Now, we can calculate the standard cell potential using the formula:
E°cell = E°red (reduction) - E°red (oxidation)
E°cell = (-0.40 V) - (-0.25 V)
E°cell = -0.40 V + 0.25 V
E°cell = -0.15 V
Therefore, the standard cell potential of a nickel-cadmium electrochemical cell is -0.15 V.
You made a typo. I'm sure you meant
Cd + Ni2+ → Cd2+ + Ni
Look up the Cd ==> Cd(2+) OXIDATION potential.
Look up the Ni^2+ + 2e ==> REDUCTION potential.
Add the two to get the standard cell potential.
Your text probably gives only the reduction potential. Reverse the reaction in the text, change the sign of the potential listed, and that convert the reduction potential into the oxidation potential