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 $............ \ mg$.

Match the column :-

Column $I$ (Reduction process)	Column $II$ (Charge required)
$(a)$ $1$ mol of $MnO_4^-$ to $Mn^{2+}$	$(p)$ $193000$ $C$
$(b)$ $1$ mol of $Cr_2O_7^{2-}$ to $Cr^{3+}$	$(q)$ $289500$ $C$
$(c)$ $1$ mol of $Sn^{4+}$ to $Sn^{2+}$	$(r)$ $482500$ $C$
$(d)$ $1$ mol of $Al^{3+}$ to $Al$	$(s)$ $579000$ $C$

When the same quantity of electricity is passed through solutions of different electrolytes connected in series,the amounts of substances deposited at the electrodes are in the ratio of their ...?

When electricity is passed through a solution of $AlCl_3$,$13.5 \ g$ of $Al$ is deposited. What is the number of Faradays used?

Total charge on $1 \, \text{mole}$ of a monovalent metal ion is equal to

$0.066 \ g$ of metal was deposited when a current of $2 \ A$ is passed through a metal ion solution for $100 \ s$. What is the electrochemical equivalent (in $g \ C^{-1}$) of the metal?