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

$0.066 \ g$ 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?

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

If $0.5 \, A$ current is passed through an acidified silver nitrate solution for $10 \, min$,the mass of silver deposited on the cathode is ........... $g$ (equivalent weight of silver $= 108$).

When a current of $0.1 \, A$ is passed through $200 \, mL$ of a $0.1 \, N$ $AgNO_3$ solution,silver is deposited. How much time in $sec$ is required to remove half of the silver from the solution?

When $96500 \ C$ of electricity is passed through a copper sulphate solution,the amount of copper deposited will be ............... $mol$.