Statement I: 96,500 C charge is required for the reduction of one mole of silver ions

Statement II: The amount of electricity (or) charge required for oxidation or reduction depends on the stoichiometry of the electrode reaction

Both Statement I and Statement II are correct and Statement II is not a correct explanation of Statement I

The correct answer is option 1. Both Statement I and Statement II are correct, and Statement II is the correct explanation of Statement I.
Statement I: 96,500 C charge is required for the reduction of one mole of silver ions.
This statement is correct. The quantity of electric charge required for the reduction (or oxidation) of one mole of a substance during an electrochemical reaction is known as the Faraday constant. For silver ions (Ag⁺) to be reduced to solid silver (Ag⁰), one mole of Ag⁺ ions requires 96,500 coulombs of charge.

Statement II: The amount of electricity (or) charge required for oxidation or reduction depends on the stoichiometry of the electrode reaction.
This statement is also correct. The amount of electric charge required for any electrochemical reaction, be it oxidation or reduction, depends on the stoichiometry of the reaction. In other words, it depends on the balanced chemical equation for the electrode reaction. The stoichiometry determines the number of moles of electrons exchanged during the reaction, and one mole of electrons corresponds to one Faraday of charge (approximately 96,500 C).

So, both statements are correct, and Statement II correctly explains why a 96,500 C charge is required for the reduction of one mole of silver ions (Statement I). The Faraday constant is a fundamental constant in electrochemistry and relates the amount of charge to the number of moles of electrons transferred in an electrochemical reaction.