When $9.65 \ C$ of electricity is passed through a solution of silver nitrate (atomic weight of $Ag = 108$),the amount of silver deposited is $............ \ mg$.

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

How much electricity in terms of Faraday is required for the reduction of $2 \ mol$ of $Cr_2O_7^{2-}$ into $Cr^{3+}$ in an acidic medium (in $F$)?

On passing a current of $1.2 \ A$ through a solution of salt of copper for $40 \ min$,$0.96 \ g$ of copper was deposited. The equivalent weight of copper in $g$ is

Aluminum oxide is electrolyzed at $1000^\circ C$ to produce aluminum metal. The cathode reaction is $Al^{3+} + 3e^- \rightarrow Al$. What quantity of electricity is required to produce $5.12 \ kg$ of aluminum metal? (Given: $1 \ Faraday = 96500 \ C$)

When the same quantity of electricity is passed through aqueous $H_2SO_4$ and molten $MgSO_4$,what is the ratio of the weights of hydrogen and magnesium deposited?