The unit of electrochemical equivalent is
- $gm \,ampere^{-1}$
- $gm/coulomb$
- $gm-ampere$
- $coulomb/gram$
The Correct Option is B
Solution and Explanation
Top Questions on Electrochemical Cells
Consider the following electrochemical cell at standard condition. $$ \text{Au(s) | QH}_2\text{ | QH}_X(0.01 M) \, \text{| Ag(1M) | Ag(s) } \, E_{\text{cell}} = +0.4V $$ The couple QH/Q represents quinhydrone electrode, the half cell reaction is given below: $$ \text{QH}_2 \rightarrow \text{Q} + 2e^- + 2H^+ \, E^\circ_{\text{QH}/\text{Q}} = +0.7V $$
- JEE Main - 2025
- Chemistry
- Electrochemical Cells
- For a given half cell, \( \text{Al}^{3+} + 3e^- \rightarrow \text{Al} \) on increasing the concentration of aluminium ion, the electrode potential will
- KCET - 2025
- Chemistry
- Electrochemical Cells
- Match the following and select the correct option for the quantity of electricity, in Cmol\(^{-1}\), required to deposit various metals at the cathode.
- KCET - 2025
- Chemistry
- Electrochemical Cells
- Catalysts are used to increase the rate of a chemical reaction. Because it
- KCET - 2025
- Chemistry
- Electrochemical Cells
In the above diagram, the standard electrode potentials are given in volts (over the arrow). The value of \( E^\circ_{\text{FeO}_4^{2-}/\text{Fe}^{2+}} \) is:
- JEE Main - 2025
- Chemistry
- Electrochemical Cells
Notes on Electrochemical Cells
Concepts Used:
Electrochemical Cells
An electrochemical cell is a device that is used to create electrical energy through the chemical reactions which are involved in it. The electrical energy supplied to electrochemical cells is used to smooth the chemical reactions. In the electrochemical cell, the involved devices have the ability to convert the chemical energy to electrical energy or vice-versa.
Classification of Electrochemical Cell:
Cathode
- Denoted by a positive sign since electrons are consumed here
- A reduction reaction occurs in the cathode of an electrochemical cell
- Electrons move into the cathode
Anode
- Denoted by a negative sign since electrons are liberated here
- An oxidation reaction occurs here
- Electrons move out of the anode
Types of Electrochemical Cells:
Galvanic cells (also known as Voltaic cells)
- Chemical energy is transformed into electrical energy.
- The redox reactions are spontaneous in nature.
- The anode is negatively charged and the cathode is positively charged.
- The electrons originate from the species that undergo oxidation.
Electrolytic cells
- Electrical energy is transformed into chemical energy.
- The redox reactions are non-spontaneous.
- These cells are positively charged anode and negatively charged cathode.
- Electrons originate from an external source.