Question:
$E^{\circ}$ values of three metals are listed below.
$Zn^{2+}_{\left(aq\right)}+2e^{-} \to Zn_{\left(s\right)};\quad E^{\circ}=-0.76\,V$
$Fe^{2+}_{\left(aq\right)}+2e^{-} \to2Fe_{\left(s\right)}; \quad E^{\circ}=-0.44\,V$
$Sn^{2+}_{\left(aq\right)}+2e^{-} \to Sn_{\left(s\right)}; \quad E^{\circ}=-0.14\,V$
Which of the following statements are correct on the basis of the above information?
(i) Zinc will be corroded in preference to iron if zinc coating is broken on the surface.
(ii) If iron is coated with tin and the coating is broken on the surface then iron will be corroded.
(iii) Zinc is more reactive than iron but tin is less reactive than iron.
$E^{\circ}$ values of three metals are listed below.
$Zn^{2+}_{\left(aq\right)}+2e^{-} \to Zn_{\left(s\right)};\quad E^{\circ}=-0.76\,V$
$Fe^{2+}_{\left(aq\right)}+2e^{-} \to2Fe_{\left(s\right)}; \quad E^{\circ}=-0.44\,V$
$Sn^{2+}_{\left(aq\right)}+2e^{-} \to Sn_{\left(s\right)}; \quad E^{\circ}=-0.14\,V$
Which of the following statements are correct on the basis of the above information?
(i) Zinc will be corroded in preference to iron if zinc coating is broken on the surface.
(ii) If iron is coated with tin and the coating is broken on the surface then iron will be corroded.
(iii) Zinc is more reactive than iron but tin is less reactive than iron.
Updated On: Jul 31, 2023
- (i) and (ii) only
- (ii) and (iii) only
- (i), (ii) and (iii)
- (i) and (iii) only
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The Correct Option is C
Solution and Explanation
Iron coated with zinc does not get rusted even if cracks appear on the surface because $Zn$ will take part in redox reaction not $Fe$ as $Zn$ is more reactive than $Fe$. If iron is coated with tin and cracks appear on the surface, $Fe$ will take part in redox reaction because $Sn$ is less reactive than $Fe$.
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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.