Explain Fraday's law of electrolysis and their application.
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Faraday’s Laws of Electrolysis
In the early nineteenth century, Michael Faraday carried out a number of experiments on electrolysis and discovered two important laws of electrolysis as:
Must Read- What is Electrolysis process and its Uses
Faraday’s First Law of Electrolysis
It states that the amount of any substance deposited at an electrode is directly proportional to the quantity of electricity passed through the electrolyte solution.
Mathematically: W ∝ Q
where W is the weight (in grams) of the substance deposited and Q is the quantity of electricity (in coulombs) which is passed through the electrolyte.
Since the quantity of electricity Q = I x t, where I is the current strength in amperes and t is the time in seconds, therefore, the above expression can be written as:
W ∝ I x t Or W=Z×I×t
where z is a constant of proportionality and is called the electrochemical equivalent of the substance. If I = 1 ampere and t = 1 second, then: W = Z
Thus, an electrochemical equivalent is defined as the weight of a substance deposited by the passage of one ampere current for one second (or one coulomb of electricity).
Importance of First Law of Electrolysis
This law is used to calculate:
The values of electrochemical equivalents of different ions.
The weights of different ions deposited by passing different quantities of electricity through their electrolytes.
It has been found out experimentally that by passing one Faraday, i.e., 96500 coulombs of electricity through an electrolyte, it results in the decomposition of one gram equivalent (i.e., equivalent weight expressed in grams) of the substance being deposited on the electrode. Therefore:
On the other hand, one coulomb of electricity deposits electrochemical equivalent (z) of the substance Hence, we may conclude that:
One Faraday or 96500 coulombs deposit one gram equivalent of the substance.
Electrochemical equivalent (Z) x 96500 = Gram equivalent
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In the early nineteenth century, Michael Faraday carried out a number of experiments on electrolysis and discovered two important laws of electrolysis as:
Must Read- What is Electrolysis process and its Uses
Faraday’s First Law of Electrolysis
It states that the amount of any substance deposited at an electrode is directly proportional to the quantity of electricity passed through the electrolyte solution.
Mathematically: W ∝ Q
where W is the weight (in grams) of the substance deposited and Q is the quantity of electricity (in coulombs) which is passed through the electrolyte.
Since the quantity of electricity Q = I x t, where I is the current strength in amperes and t is the time in seconds, therefore, the above expression can be written as:
W ∝ I x t Or W=Z×I×t
where z is a constant of proportionality and is called the electrochemical equivalent of the substance. If I = 1 ampere and t = 1 second, then: W = Z
Thus, an electrochemical equivalent is defined as the weight of a substance deposited by the passage of one ampere current for one second (or one coulomb of electricity).
Importance of First Law of Electrolysis
This law is used to calculate:
The values of electrochemical equivalents of different ions.
The weights of different ions deposited by passing different quantities of electricity through their electrolytes.
It has been found out experimentally that by passing one Faraday, i.e., 96500 coulombs of electricity through an electrolyte, it results in the decomposition of one gram equivalent (i.e., equivalent weight expressed in grams) of the substance being deposited on the electrode. Therefore:
On the other hand, one coulomb of electricity deposits electrochemical equivalent (z) of the substance Hence, we may conclude that:
One Faraday or 96500 coulombs deposit one gram equivalent of the substance.
Electrochemical equivalent (Z) x 96500 = Gram equivalent
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Answer:
Faraday's Law:
The laws state that
(1) the amount of chemical change produced by current at an electrode-electrolyte boundary is proportional to the quantity of electricity used, and
(2) the amounts of chemical changes produced by the same quantity of electricity in different substances are proportional to their equivalent weights.
Applications of Electrolysis
- Extraction and Refining of Metals
- Production of chemicals
- Electrolytic Reduction of Metals from their Compounds
- Electroplating
- Electro-forming
- Corrosion of metals
- Electrowinning,
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