During electrolysis of a solution of $AgNO_3$, $9650$ coulombs of charge is passed through the solution. What will be the mass of silver deposited on the cathode?
- $108\,g$
- $10.8\,g$
- $1.08\,g$
- $216\,g$
The Correct Option is B
Solution and Explanation
The breakdown and chemical transformation of an element under the influence of any electric current is known as electrolysis. Sir Humphrey Davey performed the first electrolysis in the year 1808. Both galvanic and electrolytic cells are capable of experiencing electrolysis. We shall focus on electrolytic cells in particular in this essay.
Through the application of an electric current, the process of electrolysis can modify a substance's chemical composition. Ionic chemicals include charged particles known as ions. The electrolysis procedure cannot begin until they are unrestricted in their movements.
The ions are liberated when an ionic material is dissolved in water.
Two electrodes are positioned in the solution and an electrical current is run between them during the electrolysis process.
Anode refers to the electrode linked to the positive terminal of the power source, whereas cathode refers to the electrode attached to the negative terminal.
This occurs as a result of the ions in the material moving towards the electrodes as a result of the electric current.
As a result, the compounds in the solution break down as the current passes through it.
The cathode receives positively charged ions, whereas the anode receives negatively charged ions.
The ions either form new molecules or break apart into their component components when they come into contact with the electrodes, depending on whether they gain or lose electrons. The manufacture of metals like aluminium and copper, the purification of chemicals, and the creation of hydrogen gas are just a few of the businesses that employ electrolysis.
Top Questions on Electrochemistry
- In an electrochemical cell, the standard electrode potential of Zn\(^{2+}\)/Zn is \(-0.76\, \text{V}\) and that of Cu\(^{2+}\)/Cu is \(+0.34\, \text{V}\). What is the standard EMF of the cell?
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\[ {Mg(s)} | {Mg}^{2+}(x M) || {Zn}^{2+}(y M) | {Zn(s)} \] The cell reaction reached the equilibrium state. What is the value of \(\log \frac{[{Mg}^{2+}]}{[{Zn}^{2+}]}\)? Given: \[ E^\circ_{{Mg}^{2+}/{Mg}} = -2.36\, V; E^\circ_{{Zn}^{2+}/{Zn}} = -0.76\, V; \frac{2.303 RT}{F} = 0.06\, V \]- AP EAPCET - 2025
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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.