Final answer:
To calculate the mass of p-aminophenol produced when a 9.65 ampere current is passed for 1 hour, Faraday's laws of electrolysis are used, combined with the molar mass of p-aminophenol and the stoichiometry of the reaction.
Step-by-step explanation:
When 9.65 ampere current is passed for 1.0 hour into nitrobenzene in an acidic medium to produce p-aminophenol, we need to use Faraday's laws of electrolysis to calculate the mass of the substance produced. According to the laws, the amount of substance produced during electrolysis is directly proportional to the quantity of electricity (Q) that passes through the cell, where Q = current (I) multiplied by time (t).
To calculate the mass of p-aminophenol produced, we first need the molar mass of p-aminophenol and the number of moles of electrons (Faradays) required to reduce a mole of nitrobenzene to p-aminophenol. Then the number of moles of p-aminophenol produced can be calculated by dividing the total charge passed (in coulombs) by the charge of one mole of electrons (Faraday's constant, approximately 96485 C/mol).
Assuming the reaction for the electrolysis requires one mole of electrons per mole of p-aminophenol produced, we can calculate the number of moles of p-aminophenol, and then the mass by multiplying by the molar mass of p-aminophenol. For a current of 9.65 A over 1 hour (3600 seconds), the total charge Q is 9.65 A * 3600 s = 34740 C. The number of moles of electrons is 34740 C / 96485 C/mol ≈ 0.36 mol. Finally, the mass can be calculated by multiplying the moles by the molar mass of p-aminophenol.