Question

Name the law or principle confirmed by the following observations:
When 96500 coulombs of electricity is passed through acidulated water, 5−6 litres of oxygen at S.T.P. is liberated at the anode.

Answer 1

Hint- In this question, as mentioned this question gives an observation that when 96500 columns of electricity are passed through acidulated water 5-6 liter of oxygen at S.T.P is liberated at the anode. We need to name the law or principle which is confirmed by this observation: the amount of substance liberated at the electrode is directly proportional to the amount of electricity passed through the electrodes.

Complete step-by-step answer:
Before analysis of Faraday’s laws of electrolysis, we need to first understand the process of electrolysis of a metal sulfate. Whenever an electrolyte like metal sulfate is diluted in ${H_2}O$, the molecules of this split into positive and negative ions. The positive ions (or metal ions) strike to the electrodes connected with the negative terminal of the battery where these positive ions take electrons from it, forming a refined metal atom and also deposited on the electrode.
As we know, -ve ions (or sulphions) move to the electrode connected with the positive terminal of the battery, where these negative ions give up their extra e’s (electrons) and become $S{O_4}$ radical. Since $S{O_4}$ cannot exist in neutral state, it will be attacking the metallic +ve electrode and forming a metallic sulfate which will again dissolve in the ${H_2}O$.
Faraday’s First Law of Electrolysis states that the chemical deposition due to the movement leads to flow of current through an electrolyte is directly proportional to the quantity of electricity (coulombs) passed through it.
The amount of substance liberated at electrodes is directly proportional to the amount of electricity passed through electrodes is called Faraday's first law of electrolysis.

Note- Remember, Faraday’s laws of electrolysis provide the quantitative (mathematical) relationships that describe the above two phenomena. Thus, for the same quantity of charge passing through different electrolytes, the mass of deposited chemical is directly proportional to its atomic weight and inversely proportional to its valency.