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Write Faraday’s second law of electrolysisDraw labelled diagram of standard hydrogen electrode

Last updated date: 20th Jun 2024
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Hint: Faraday’s law is the basic law of electromagnetism which helps to predict how a magnetic field would interact with an electric current to produce an electromotive force. Moreover, a standard hydrogen electrode is a redox electrode which forms the basis of the thermodynamic scale of oxidation-reduction potentials.

Faraday’s law was proposed in the year 1831 by a physicist and chemist named Michael Faraday. This further consists of two laws. The first law describes the induction of emf in a conductor and the second law quantifies the emf produced in the conductor. Now let’s discuss Faraday’s second law of electromagnetic induction in detail.
Now, the second law states that the induced emf in a coil is equal to the rate of change of the flux linkage. Further, the flux is the product of the number of turns in the coil and the flux associated with the coil. The formula is given below:
${\rm E} = - N\dfrac{{\Delta \phi }}{{\Delta t}}$
Where, E is the electromotive force
N is the number of turns,
$\phi$ is the magnetic flux
Moreover, the negative sign indicates that the direction of the induced emf and change in the direction of magnetic fields have the opposite signs.
Now, we will discuss the standard hydrogen electrode. Basically, this electrode is used as a reference electrode while calculating the standard electrode potential of a half cell. Its standard electrode potential is declared to be zero at a temperature of 298K because it acts as a reference for comparison with any other electrode. The redox half-cell of the standard hydrogen electrode is where the following reaction takes place:
$2{H^ + }(aq) + 2{e^ - } \to {H_2}(g)$
This reaction generally takes place on a platinum electrode. The diagram is as shown:

Note:
Platinum is used in the hydrogen electrode due to many reasons. It is a relatively inert metal which does not corrode easily and has a catalytic quality which further promotes the proton reduction. Moreover, it also improves the reaction kinetics by adsorbing hydrogen at the surface.