How many total Faraday currents will be required to obtain $1 \ mole$ of $Ag$,$Mg$,and $Al$ respectively?

What amount of $Cl_2$ gas is liberated at the anode if $1 \ A$ current is passed for $30 \ min$ through an $NaCl$ solution?

$0.066 \ g$ of metal was deposited when a current of $2 \ A$ is passed through a metal ion solution for $100 \ s$. What is the electrochemical equivalent (in $g \ C^{-1}$) of the metal?

During the electrolysis of a solution of $AgNO_3$,$9650 \ C$ of charge passes through the electroplating bath. The mass of silver deposited at the cathode will be .............. $g$.

Electrolysis of dilute aqueous $NaCl$ solution was carried out by passing $10 \ mA$ current. The time required to liberate $0.01 \ mol$ of $H_2$ gas at the cathode is $(1 \ F = 96500 \ C \ mol^{-1})$

How much electricity in terms of Faraday is required to produce $2.7 \ g$ of $Al$ from molten $Al_2O_3$? (Atomic mass of $Al = 27 \ u$)