A mass of 18.2304 g of silver is formed during the electrolysis.
During the electrolysis procedure, ions and atoms are exchanged as a result of the addition or subtraction of electrons from the external circuit. In essence, cations are discharged into the neutral atom by migrating to the cathode in response to current flow, stealing electrons from the cathode (supplied by the supply source battery), and then leaving the cathode.
According to Faraday's law, the mass of any substance that is electrolyzed or dissolved is proportional to the product of the equivalent weight of the substance times the quantity of electricity passed during the reaction.
The molar mass of Ag= 108 [tex]mol^{-1}[/tex]
1 Faraday= 96500 C
Q=It
=(1.12)(2.4(60)(60))
=16289.28 Coulombs
According to Faraday Law
[tex]Z= \frac{M}{nF}[/tex]
n-factor of [tex]AgNO_{3}=1[/tex]
Therefore,
[tex]Z=\frac{108}{1(96500)}[/tex]
Now, the weight of the substance will be
[tex]=\frac{108}{96500} (16289.28)\\=18.2304 g[/tex]
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