Dîrokên Faraday derbarê Elektroliz – Dîroka Yekem û Dîroka Dwyem (Ekuasyon û Pêşnûan)

Faraday’s Laws of Electrolysis

Beforê inke bînin Faraday’s laws of electrolysis, pirin dibe ku hewce bikin procesa electrolysis ya sulfateya metal.

Her çendî elektrolit wek sulfateya metal di ser deraveyê de dilanîne, molekulên wê divê bibin bi îonên pozîtif û negatif. Îonên pozîtif (an jî metal îon) duvare be destên neyên negatîf a battery da ku wan îonên pozîtif elektronên ji wan re hin, bibin metal pûr atom û hewl bike bin destên ney.

Îonên negatif (an jî sülfîon) duvare be destên neyên pozitîf a battery, ku wan îonên negatif elektronên ekstra yên wan re din, bibin SO4 radical. Ji ber ku SO4 nabe ku bibe di navcheyê elektrik de, ew duvare be destên metal pozitîf ê xebit bike - formîn sulfateya metal ke dibê dilanîne di deraveyê de.

Faraday’s laws of electrolysis heye parastayên kantitatîv (matematîkî) ku tefsir bikin di du fenomenên serokan de.

Faraday’s First Law of Electrolysis

Ji tevlî bînin ku hate werd, dibe ku şevê current di cihên sereketîn battery de li virê ku çend elektron ji destên neyên negatîf an cathode re hatin şevkirin ji bo îonên pozitîf metal an cations. Eger cations valency dijîn wek Cu++ heye, her cation ji ro çend elektron ji cathode re şevkirin. Ez dînim ku her elektron gotarî negatîf dikin – 1.602 × 10-19 Coulombs û dewamê e. Ji ber vê yekê, her Cu atom ji ro şevkirin ji cathode re bibe – 2.e gotarî şevkirin ji cathode re cation.

Ewêstîn, ji bo dem t, çendiyek n number of copper atoms deposited on the cathode, total charge transferred, would be – 2.n.e Coulombs. Mass m of the deposited copper is obviously a function of the number of atoms deposited. So, it can be concluded that the mass of the deposited copper is directly proportional to the quantity of electrical charge that passes through the electrolyte. Hence mass of deposited copper m ∝ Q quantity of electrical charge passes through the electrolyte.

Faraday’s First Law of Electrolysis states that the chemical deposition due to the flow of current through an electrolyte is directly proportional to the quantity of electricity (coulombs) passed through it.

i.e. mass of chemical deposition:

Where, Z is a constant of proportionality and is known as electro-chemical equivalent of the substance.

If we put Q = 1 coulombs in the above equation, we will get Z = m which implies that electrochemical equivalent of any substance is the amount of the substance deposited on the passing of 1 coulomb through its solution. This constant of the passing of electrochemical equivalent is generally expressed in terms of milligrams per coulomb or kilogram per coulomb.

Faraday’s Second Law of Electrolysis

So far we have learned that the mass of the chemical, deposited due to electrolysis is proportional to the quantity of electricity that passes through the electrolyte. The mass of the chemical, deposited due to electrolysis is not only proportional to the quantity of electricity passes through the electrolyte, but it also depends upon some other factor. Every substance will have its own atomic weight. So for the same number of atoms, different substances will have different masses.

Again, how many atoms deposited on the electrodes also depends upon their number of valency. If valency is more, then for the same amount of electricity, the number of deposited atoms will be less whereas if valency is less, then for the same quantity of electricity, more number of atoms to be deposited.

So, for the same quantity of electricity or charge passes through different electrolytes, the mass of deposited chemical is directly proportional to its atomic weight and inversely proportional to its valency.

Faraday’s second law of electrolysis states that, when the same quantity of electricity is passed through several electrolytes, the mass of the substances deposited are proportional to their respective chemical equivalent or equivalent weight.

Chemical Equivalent or Equivalent Weight

The chemical equivalent or equivalent weight of a substance can be determined by Faraday’s laws of electrolysis, and it is defined as the weight of that subtenancy which will combine with or displace the unit weight of hydrogen.

The chemical equivalent of hydrogen is, thus, unity. Since valency of a substance is equal to the number of hydrogen atoms, which it can replace or with which it can combine, the chemical equivalent of a substance, therefore may be defined as the ratio of its atomic weight to its valency.

Who Invented Faraday’s Laws of Electrolysis?

Faraday’s Laws of Electrolysis were published by Michael Faraday in 1834. Michael Faraday was also responsible

As well as discovering these laws of electrolysis, Michael Faraday is also responsible for popularizing terminologies such as electrodes, ions, anodes, and cathodes.

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