The amount of substance deposited when a current of $1 \ A$ is passed for $1 \ s$ is equal to:

What is the time (in $sec$) required for depositing all the silver present in $125 \ mL$ of $1 \ M \ AgNO_3$ solution by passing a current of $241.25 \ A$? $(1 \ F = 96500 \ C)$

The number of moles of electrons passed when a current of $2 \ A$ is passed through a solution of electrolyte for $20 \ minutes$ is

If the total electricity required to deposit $1$ mole of a metal $M$ is equal to that of $10.7$ amperes of current for $10$ hours,the equivalent weight of the metal is (atomic weight $= M \ u$):

What current strength is required to deposit $36 \ g$ of $Ag$ in $7 \ minute$ from $AgNO_3$ solution by electrolysis (in $A$)? (Atomic mass $Ag = 108$)

How many moles of electrons (how many Faradays of electricity) are required to reduce $1 \ mol$ of $MnO_4^-$ to $MnO_2$?