Electrochemistry - 1 Faraday Concept
Based on experiments conducted by Faraday, the electric charge of 1 mole of electrons is around 95 600 Coulombs. This charge value is known as 1 Faraday. Thus, 1 mole of electrons = 1 Faraday = 96 500 Coulombs. Through this conversion system, we can calculate the electron charge required in the electrolysis reaction.
Examples of electrolysis questions:
How much electric charge is needed to reduce:
a. 0.8 moles of Ag⁺ ions become Ag
b. 1.2 moles of Cu²⁺ ions become Cu
Examples of electrolysis questions:
How much electric charge is needed to reduce:
a. 0.8 moles of Ag⁺ ions become Ag
b. 1.2 moles of Cu²⁺ ions become Cu
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LearningTranscript
00:00What electric charge is required to reduce 0.8 moles of Ag plus ions to Ag and 1.2 moles of Cu2 plus ions to Cu?
00:14Okay, here is an electrolysis cell.
00:18In the electrolyte solution, there are silver ions and nitrate ions.
00:23Two electrodes made of platinum are dipped into it.
00:26Platinum is an inert metal.
00:30This metal does not react chemically.
00:36These two metals are connected by a cable to the battery.
00:43Not long after that, electrons flow from the negative pole of the battery to the positive pole of the battery through the solution.
00:52These electrons are absorbed by silver ions to form silver metal.
00:56These atoms stick to the surface of the electrode.
01:00So, the sticking of silver atoms on the surface of this electrode can be called a deposit.
01:08Note, each silver ion absorbs one electron.
01:14If there is one mole of silver ions, then one mole of electrons will be absorbed.
01:19Based on experiments conducted by Faraday, the electric charge of one mole of electrons is around 95,600 coulombs.
01:33This charge value is known as 1 Faraday.
01:38Thus, one mole of electrons is equal to 1 Faraday, also equal to 96,500 coulombs.
01:45Through this conversion system, we can calculate the electron charge required in the electrolysis reaction.
01:55The first stage is identification.
01:58The number of silver ions, n, is equal to 0.8 moles.
02:03The number of copper ions, n, is equal to 1.2 moles.
02:07In case A, the reduction reaction at the cathode, the silver ion and an electron react to form a silver atom.
02:17The ratio of moles of silver ion and electron is 1 to 1.
02:22So, the moles of electrons required is 0.8 moles.
02:26So, the moles of electrons required is 0.8 moles.
02:34The charge is, Q1 is equal to 0.80 times 96,500 coulombs.
02:41This value is equal to 7,720 coulombs.
02:46In case B, the reduction reaction at the cathode, copper ions and two electrons react to form copper atoms.
02:56The ratio of copper ions and electrons is 1 to 2.
03:01So, the moles of electrons needed are 2 times 1.2.
03:05This value is equal to 2.4 moles.
03:10The charge is, Q2 is equal to 2.4 times 96,500.
03:16This value is equal to 23,160 coulombs.
03:21Hope it is useful.
03:23And, don't forget to watch the next video.
03:26Thank you.