 # How can you verify the Faraday's First Law Of Electrolysis experimentally?

Faraday’s – First Law of Electrolysis

It states, during electrolysis, the amount of chemical reaction which occurs at any electrode under the influence of electrical energy is proportional to the quantity of electricity passed through the electrolyte.

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Consider a battery, rheostat, key and ammeter are connected to an electrolyte cell in series. Cleaning, drying, measuring the cathode and then inserting it into the cell. For a time t, a current I1 is passed. The ammeter is used to measure current. The cathode is removed, cleaned, dried and weighed once more. While mass m1 of the deposited material is obtained.

The cathode is reinserted into the cell, and at the same time, t different current I2 is passed. Deposit mass m2 is obtained. It is observed that

m1/m2 = I1/I2

so mass is directly proportional to the current passed.

i.e m ∝ I ……………………………(1)

The experiment is repeated with the same I current but t1 and t2 with different periods. If the deposit masses are m3 and m4 respectively, it is observed that

m3/m4 = t1/t2

So mass is directly proportional to the period

i.e m ∝ t………………………….(2)

From equation (1) and (2)

m ∝ It

But It = q

So m ∝ q…………………..(3)

Equation proves the Faraday’s – First Law of Electrolysis.