Faraday Constant - Definition, Formula, Applications, Values - Byju's

Faraday Constant Formula

This constant can be expressed in terms of two other physical constants as-

F = eNAWhere,

• e is the charge of the electron in coulombs e = 1.60217662×10−19 C
• NA is the Avogadro constant. NA = 6.022141×1023 mol−1.

Applications

One of the most common uses of Faraday constant is in electrolysis. Dividing the amount of charge in coulombs by the Faraday constant gives the amount in moles of elements that have been oxidized.

Calculation

Researches have been carrying out till today to increase the accuracy of Faraday constant. Although it was initially determined using Faraday’s law of electrolysis. In general, for an electrochemical reaction, a measured value of current is made to pass for a certain time and the value of F was calculated by measuring the amount of silver deposited.

Hope you have understood about Faraday constant, How it is calculated, Its physical properties like – Value, Formula along with terms, units and values, Applications in electrolysis.

Physics Related Topics:

Proton Mass

Neutron Mass

Alpha Particle Mass

Value Of Electron

Frequently Asked Questions – FAQs

Q1

What is Faraday Constant?

It represents the magnitude of electric charge per mole of the electron.Q2

What is the value of the Faraday Constant?

It has currently the universally accepted value Faraday constant (F) =96485.33289(59) C mol−1Q3

What is the formula of the Faraday Constant?

This constant can be expressed in terms of two other physical constants as F = eNA Where, e is the charge of the electron in coulombs e = 1.60217662×10-19 C NA is the Avogadro constant. NA = 6.022141×1023 mol-1. Q4

What is the value of the Faraday Constant in kcal per volt gram equivalent?

Faraday constant (F) = 23.061 kcal per volt gram equivalentQ5

What is the application of Faraday’s constant?

One of the most common uses of Faraday constant is in electrolysis. Dividing the amount of charge in coulombs by the Faraday constant gives the amount in moles of elements that have been oxidized.

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