The number of coulombs required to reduce $12.3 \ g$ of nitrobenzene to aniline is:

When two electrolytic cells containing $NiSO_4$ and $CuSO_4$ solutions are connected in series and an electric current is passed,$1.6 \ g$ of $Cu$ is deposited on the electrode. How much $Ni$ metal is produced? If a cell containing $AgNO_3$ solution is connected instead of $NiSO_4$,how many grams of silver will be obtained? [Atomic mass: $Cu = 63.5 \ g/mol$,$Ni = 58.7 \ g/mol$,$Ag = 108 \ g/mol$]

How many electrons would be required to deposit $6.35 \ g$ of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate? (Atomic mass of copper $= 63.5 \ u$,$N_A =$ Avogadro's constant)

In order to separate oxygen from one mole of $H_2O$,the required quantity of electricity in coulombs is:

One gram of metal ion $M^{3+}$ is discharged by the passage of $1.81 \times 10^{23}$ electrons. What is the atomic weight of the metal?

The relation between Faraday constant $F$,electron charge $e$,and Avogadro number $N$ is: