Faraday's laws of electrolysis

Michael Faraday reported that the mass ({{mvar|m}}) of a substance deposited or liberated at an electrode is directly proportional to the charge ({{mvar|Q}}, for which the SI unit is the ampere-second or coulomb).{{cite web|title=Faraday's laws of electrolysis {{!}} chemistry | url=https://www.britannica.com/science/Faradays-laws-of-electrolysis | access-date=2020-09-01 | website=Encyclopedia Britannica |language=en}}

$$m\; \backslash propto\; Q\; \backslash quad\; \backslash implies\; \backslash quad\; \backslash frac\{m\}\{Q\}\; =\; Z$$

Here, the constant of proportionality, {{mvar|Z}}, is called the electro-chemical equivalent (ECE) of the substance. Thus, the ECE can be defined as the mass of the substance deposited or liberated per unit charge.

Faraday discovered that when the same amount of electric current is passed through different electrolytes connected in series, the masses of the substances deposited or liberated at the electrodes are directly proportional to their respective chemical equivalent/equivalent weight ({{mvar|E}}). This turns out to be the molar mass ({{mvar|M}}) divided by the valence ({{mvar|v}})

: $\backslash begin\{align\}$

& m \propto E; \quad E = \frac{\text{molar mass}}{\text{valence}} = \frac{M}{v} \\

& \implies m_1 : m_2 : m_3 : \ldots = E_1 : E_2 : E_3 : \ldots \\

& \implies Z_1 Q : Z_2 Q : Z_3 Q : \ldots = E_1 : E_2 : E_3 : \ldots \\

& \implies Z_1 : Z_2 : Z_3 : \ldots = E_1 : E_2 : E_3 : \ldots

\end{align}

A monovalent ion requires one electron for discharge, a divalent ion requires two electrons for discharge and so on. Thus, if {{mvar|x}} electrons flow, $\backslash tfrac\{x\}\{v\}$ atoms are discharged.

Thus, the mass {{mvar|m}} discharged is

m = \frac{x M}{v N_{\rm A}} = \frac{Q M}{e N_{\rm A} v} = \frac{Q M}{vF}

where

• {{math|N{{sub|A}}}} is the Avogadro constant;
• {{math|1=Q = xe}} is the total charge, equal to the number of electrons ({{mvar|x}}) times the elementary charge {{mvar|e}};
• {{math|F}} is the Faraday constant.

Faraday's laws can be summarized by

: $Z\; =\; \backslash frac\{m\}\{Q\}\; =\; \backslash frac\{1\}\{F\}\backslash left(\backslash frac\{M\}\{v\}\backslash right)\; =\; \backslash frac\{E\}\{F\}$

where {{mvar|M}} is the molar mass of the substance (usually given in SI units of grams per mole) and {{mvar|v}} is the valency of the ions .

For Faraday's first law, {{mvar|M, F, v}} are constants; thus, the larger the value of {{mvar|Q}}, the larger {{mvar|m}} will be.

For Faraday's second law, {{mvar|Q, F, v}} are constants; thus, the larger the value of $\backslash tfrac\{M\}\{v\}$ (equivalent weight), the larger {{mvar|m}} will be.

In the simple case of constant-current electrolysis, {{math|1=Q = It}}, leading to

: $m\; =\backslash frac\{ItM\}\{Fv\}$

and then to

: $n\; =\backslash frac\{It\}\{Fv\}$

where:

• {{mvar|n}} is the amount of substance ("number of moles") liberated: $n\; =\; \backslash tfrac\; m\; M$
• {{mvar|t}} is the total time the constant current was applied.

For the case of an alloy whose constituents have different valencies, we have

$$m\; =\; \backslash frac\{It\}\{F\; \backslash times\; \backslash sum\_\{i\}\; \backslash frac\{w\_i\; v\_i\}\{M\_i\}\}$$

where {{mvar|w_i}} represents the mass fraction of the {{mvar|i}}th element.

In the more complicated case of a variable electric current, the total charge {{mvar|Q}} is the electric current {{math|I(τ)}} integrated over time {{mvar|τ}}:

: $Q\; =\; \backslash int\_0^t\; I(\backslash tau)\; \backslash ,\; d\backslash tau$

Here {{mvar|t}} is the total electrolysis time.For a similar treatment, see {{cite journal | author = Strong, F. C. | title = Faraday's Laws in One Equation | journal = Journal of Chemical Education | year = 1961 | volume = 38 | issue = 2| pages = 98 | doi = 10.1021/ed038p98 |bibcode = 1961JChEd..38...98S }}

• Electroplating – a process where a thin layer of metal is deposited onto the surface of an object using an electric current
• Electrochemical cells – generates electrical energy from chemical reactions
• Electrotyping – a process used to create metal copies of designs by depositing metal onto a mold using electroplating
• Electrowinning – a process that extract metals from their solutions using an electric current
• Electroforming – a process that deposits metal onto a mold or substrate to create metal parts
• Anodization – a process that converts the surface of a metal into a durable corrosion-resistant oxide layer
• Conductive polymers – organic polymers that conduct electricity
• Water electrolysis – a process that uses an electric current to split water molecules into hydrogen and oxygen gases
• Electrolytic capacitors – a type of capacitor that uses an electrolytic solution as one of its plates

• Electrolysis
• Faraday's law of induction
• Tafel equation

{{reflist}}

• Serway, Moses, and Moyer, Modern Physics, third edition (2005), principles of physics.
• [https://pineresearch.com/shop/kb/applications/laboratory-exercises/exploring-inexpensive-electrodes/ Experiment with Faraday's laws]

{{Electrolysis}}

{{Michael Faraday}}

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