When $9650 \ C$ of charge is passed through an $AgNO_3$ solution during the electrolysis process in an electroplating bath,what is the weight of silver deposited at the cathode in $g$?

Faraday's laws of electrolysis will fail when

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

When $0.1 \ mol$ of $MnO_4^{2-}$ is oxidized,the quantity of electricity required to completely oxidize $MnO_4^{2-}$ to $MnO_4^-$ is $........ \ C$.

$A$ solution of a salt of a metal was electrolysed for $150$ minutes with a current of $0.15$ amperes. The weight of metal deposited was $0.783 \ g$. The equivalent weight of the metal is ................... $g$. (in $.97$)

If a current of $5 \ A$ is passed through a zinc sulfate solution for $40 \ \text{minutes}$,what is the mass of zinc deposited at the cathode (in $g$)?