Question:
The standard potentials of $Ag^+/Ag, Hg_2^{2+}/2Hg, Cu^{2+}/Cu$ and $Mg^{2+}/Mg$ electrodes are $0.80,0.79, 0.34$ and $-2.37\, V$, respectively. An aqueous solution which contains one mole per litre of the salts of each of the four metals is electrolyzed. With increasing voltage, the correct sequence of deposition of the metals at the cathode is
The standard potentials of $Ag^+/Ag, Hg_2^{2+}/2Hg, Cu^{2+}/Cu$ and $Mg^{2+}/Mg$ electrodes are $0.80,0.79, 0.34$ and $-2.37\, V$, respectively. An aqueous solution which contains one mole per litre of the salts of each of the four metals is electrolyzed. With increasing voltage, the correct sequence of deposition of the metals at the cathode is
Updated On: Jul 5, 2022
- $Ag, Hg, Cu, Mg$
- $Cu,Hg,Ag$ only
- $Ag, Hg, Cu$ only
- $Mg,Cu,Hg,Ag$
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The Correct Option is D
Solution and Explanation
More the reduction potential, more is the deposition of metals at cathode. Cation having $E^0$ value less than $- 0.83\,V$ (reduction potential of $H_2O$) will not deposit from aqueous solution. Hence correct order of A deposition of the metal at the cathode is
$Ag > Hg >Cu$
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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.