If the electrochemical equivalent of a substance is $0.0006735 \ g/C$,what is its equivalent weight?

$A$ current of $0.4 \ A$ is passed through excess of molten $MgCl_2$ for $9.65 \times 10^4 \ sec$. The mass of $Mg$ deposited at the cathode is .............. $gm$

When $1 \ C$ of charge is passed through an electrolyte solution,the mass deposited is equal to:

Three faradays of electricity were passed through an aqueous solution of iron $(II)$ bromide. The weight of iron metal (atomic weight $= 56$) deposited at the cathode (in $g$) is

$250 \ mL$ of a waste solution obtained from the workshop of a goldsmith contains $0.1 \ M \ AgNO_3$ and $0.1 \ M \ AuCl$. The solution was electrolyzed at $2 \ V$ by passing a current of $1 \ A$ for $15 \ minutes$. The metal/metals deposited will be
$(E^0_{Ag^+/Ag} = 0.80 \ V, E^0_{Au^+/Au} = 1.69 \ V)$

$9.65 \ C$ of electric current is passed through fused anhydrous magnesium chloride. The magnesium metal thus obtained is completely converted into a Grignard reagent. The number of moles of the Grignard reagent obtained is