The standard electrode potentials of $ A{{g}^{+}}/Ag $ is $ +0.80\text{ }V $ and $ C{{u}^{+}}/Cu $ is $ +0.34\text{ }V $ . These electrodes are connected through a salt bridge and if:
- copper electrode acts as a cathode then $ E{}^\circ $ cell is $ +0.46\text{ }V $
- silver electrode acts as anode then $ E{}^\circ $ cell is $ -0.34\text{ }V $
- copper electrode acts as anode then $ E{}^\circ $ cell is $ +0.46V $
- silver electrode acts as a cathode then $ E{}^\circ $ cell is $ -0.34\text{ }V $
The Correct Option is C
Solution and Explanation
$ =E_{A{{g}^{+}}/Ag}^{o}-E_{C{{u}^{+}}/Cu}^{o} $
$ =-0.80-0.34 $
$ =+0.46 $
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Concepts Used:
Nernst Equation
This equation relates the equilibrium cell potential (also called the Nernst potential) to its concentration gradient across a membrane. If there is a concentration gradient for the ion across the membrane, an electric potential will form, and if selective ion channels exist the ion can cross the membrane.
