The number of moles of electrons required to deposit $1 \, g$ equivalent of aluminium $(At. \, wt. = 27)$ from a solution of aluminium chloride will be

When $3 \ F$ of electricity is passed through an aqueous solution of iron $(II)$ bromide,what is the mass of iron metal deposited at the cathode in $g$?

During electrolysis,the amount of ions discharged is $NOT$ proportional to which of the following?

What is the nature of the Faraday constant?

$0.592 \ g$ of copper is deposited in $60 \ minutes$ by passing $0.5 \ amperes$ current through a solution of copper$(II)$ sulphate. The electrochemical equivalent of copper$(II)$ (in $g \ C^{-1}$) is $\left(F=96500 \ C \ mol^{-1}\right)$

Mass in grams of copper deposited by passing $9.6487 \ A$ current through a voltmeter containing copper sulphate solution for $100 \ s$ is (Given : Molar mass of $Cu: 63 \ g \ mol^{-1}, 1 \ F=96487 \ C$ ) (in $g$)