The chemical effect of current refers to the process of electrolysis, where a direct current is passed through an electrolytic solution to cause a chemical reaction. Faraday's laws of electrolysis explain the quantitative relationship between the amount of current passed through an electrolytic cell and the amount of substance produced or consumed at the electrodes.

Faraday Constant

The Faraday constant is a proportionality constant that relates the amount of electric charge per mole of electrons involved in a redox reaction. It is defined as the charge carried by one mole of electrons, which is equal to the Avogadro constant times the charge of an electron.

The value of the Faraday constant is approximately 96,485 coulombs per mole (C/mol). It is named after the British scientist Michael Faraday, who made significant contributions to the field of electrochemistry.

Chemical Equivalent and Electrochemical Equivalent

The chemical equivalent is the amount of a substance that reacts with or is produced by one mole of electrons in a redox reaction. It is defined as the ratio of the molar mass of the substance to the number of electrons involved in the reaction.

The electrochemical equivalent is the amount of a substance that is produced or consumed at the electrode per unit charge passed through the electrolytic cell. It is defined as the ratio of the molar mass of the substance to the amount of charge required to produce or consume one mole of the substance at the electrode.

Relationship between Faraday Constant, Chemical Equivalent and Electrochemical Equivalent

According to Faraday's laws of electrolysis, the amount of substance produced or consumed at the electrode is directly proportional to the amount of charge passed through the electrolytic cell. The proportionality constant is the Faraday constant.

Therefore, we can use the following relationships to relate the Faraday constant to the chemical equivalent and electrochemical equivalent:

- Faraday constant = charge per mole of electrons involved in the reaction
- Chemical equivalent = molar mass of substance / number of electrons involved in the reaction
- Electrochemical equivalent = molar mass of substance / amount of charge required to produce or consume one mole of the substance at the electrode

From these relationships, we can derive the following equation:

Faraday constant = chemical equivalent x electrochemical equivalent

Therefore, the correct option is D - chemical equivalent divided by electrochemical equivalent.