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 $g$?

What is the volume of $H_2$ gas produced at $S.T.P.$ when $1 \ Faraday$ of electricity is passed through a dilute solution of acid (in $mL$)?

In a certain electrolysis experiment,$0.650 \ g$ of zinc is deposited in a cell having $ZnSO_4$ solution. Calculate the mass of $Cu$ deposited in another cell having $CuSO_4$ solution arranged in series with the first cell (in $g$)? (Molar mass of $Zn = 65 \ g \ mol^{-1}$,$Cu = 63.5 \ g \ mol^{-1}$)

Faraday's laws of electrolysis are related to

Consider the following reaction:
$MnO_4^- + 8H^{+} + 5e^- \rightarrow Mn^{2+} + 4H_2O$,$E^\circ = 1.51 \ V$
The quantity of electricity required in Faraday to reduce five moles of $MnO_4^-$ is ..... .

How much current in amperes should be passed through a $Na_2SO_4$ solution using graphite electrodes to obtain $250 \ mL$ of $O_2$ gas per minute at $1 \ bar$ pressure and $300 \ K$ temperature (in $A$)? $[R = 0.08314 \ L \ bar \ K^{-1} \ mol^{-1}]$