Faraday constant. Faraday constant is an important physical constant in modern scientific research, which represents the charge carried by each mole of electrons, and the unit is Cmol- 1. This constant is very important, especially when determining how many ions or electrons a substance carries. Faraday constant is named after michael faraday, and Faraday's research work is of decisive significance to the determination of this constant.

Faraday constant is an important constant in physics and chemistry, especially in electrochemistry. It is a basic constant, and its value only changes with its unit. Faraday constant is a very important constant in the process of electrolysis, electroplating, fuel cells and batteries involving substances and their charges.

So it is also a very important technical constant. Faraday constant is also needed when calculating the energy change per mole of matter. One example is to calculate the energy gained or released by one mole of electrons when the voltage changes. In practical application, Faraday constant is used to calculate the general reaction coefficient, such as calculating the conversion of voltage into free energy.

The mathematical expression of Faraday's law is:

Q=nZF, where q is the amount of electricity passing through the electrode and n is the amount of substance that deposits metal. The electric quantity of 1mol electron is called 1 Faraday, which is expressed by f as Faraday constant, and f = na e = 6.022×1023 mol-/kloc-0 /×1.6022×10-655.

For example, depositing 1mol of silver from a solution containing Ag+ requires 96,485 c of electricity, while reducing 1mol of Cu2+ to copper on the electrode requires 2mol of electrons, that is, 192970C of electricity. Faraday's law of electrolysis is not only applicable to the electrolysis process, but also to the redox process of all electrode reactions.