Galvanic Cell: It is a device that converts chemical energy into electrical energy.

Electrolytic Cell: It is a device that converts electrical energy into Chemical energy.

Difference Between Galvanic Cell and Electrolytic Cell

Galvanic Cell: It is a type of electrochemical cell

Construction of Galvanic Cells

Role Of Salt Bridge:

1. glass tube/polyethylene tube (U-shaped) is filled with a paste of any electrolyte (generally KCl) with agar-agar powder and dried. The electrolyte to be used in the salt bridge should be such that the speed of its cations is equal to the speed of its anions.

2. Salt bridge completes the internal circuit of the cell as well as maintains electrical neutrality.
3. bridge also minimizes liquid-liquid junction potential.

Cell Representation:

Electrode Potential:

Standard Electrode Potential: SRP or SOP of all other electrodes are calculated by making a cell using a standard hydrogen electrode (SHE) and the other electrode dipped In 1 Molar electrolyte and then the potential difference of this cell is measured using a potentiometer. The SRP or SOP of SHE is taken to be zero, at all temperatures but actually, it is not zero.

Electrochemical Series: The SRP values of different electrodes are calculated with reference to (SHE) and are arranged in a series (in increasing order) and the series is called electrochemical series.

Features Of Electrochemical Series:

1. Greater the value of S.R.P. greater will be tendency to get reduced, so, the element or compound will be stronger oxidizing agent.
2. Smaller the value of SRP (higher the value of SOP) so greater will be the tendency to get oxidized hence compound or elements will be a better reducing agent.
3. Anode – Electrode upper in the series
4. Cathode – any lower in series in comparison to anode
5. Metals which are higher up in the series can displace metals in lower in the series from their salt
6. On moving down the series the electro (+ve) nature of the metals or elements decreases and also the reactivity of metals decreases.
7. Metals placed above than hydrogen can release H ₂ gas on reaction with dilute acid solution ex