Chemistry > Electrochemistry > 3.0 Electrochemical Cells
Electrochemistry
1.0 Introduction
2.0 Conductors and Non-Conductors
3.0 Electrochemical Cells
4.0 Electrolysis and electrode Reactions
5.0 Electrochemical Cell
6.0 Electrode Potential
7.0 Nature of Electrodes
8.0 IUPAC Cell Representation and Convention
9.0 Standard Cell EMF and Standard Reduction Potential
10.0 Electropositive Character of Metals
11.0 Difference between EMF and potential difference
12.0 Nernst Equation
13.0 Laws of Electrolysis
14.0 Electromotive Force
15.0 Thermodynamics of the Cells
16.0 Concentration Cells
17.0 Battery
18.0 Fuel Cell
3.1 Difference Between Electrolytic Cell and Galvanic Cell
| Galvanic Cell | Electrolytic Cell |
| $(i)$ Chemical energy is converted into electrical energy | $(i)$ Electrical energy is converted into chemical energy |
| $(ii)$ Only at cathode, ions are discharged. | $(ii)$ Ions are discharged at both the electrodes. |
| $(iii)$ Anode-negative electrode Cathode-positive electrode | $(iii)$ Anode-Positive electrode Cathode-negative electrode |
| $(iv)$ Electrodes are fitted in separate compartments. | $(v)$ Both the electrodes cab be fitted in same compartment. |
| $(v)$ Concentration of anodic half cell reaction increases while concentration of cathodic half cell reaction decreases when two electrodes are joined by a wire. | $(v)$ If the electrodes are inert, the concentration of the electrolyte decreases when current is circulated. |
