If a current of $0.5 \ A$ is passed through a solution of $AgNO_3$ for $193 \ s$,$0.108 \ g$ of $Ag$ is deposited. What is the equivalent weight of $Ag$?

The amount of charge required to liberate $11.5 \ g$ of sodium is .....

Passage of a current for $548 \, s$ through a silver coulometer results in the deposition of $0.746 \, g$ of silver. What is the current (in $A$)?

If $96500 \ C$ of electricity liberates one gram equivalent of any substance,the time taken for a current of $0.15 \ A$ to deposit $20 \ mg$ of copper from a solution of copper sulphate is (Chemical equivalent of copper = $32$).

$250 \ mL$ 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
$(E^0_{Ag^+/Ag} = 0.80 \ V, E^0_{Au^+/Au} = 1.69 \ V)$

Which of the following aqueous solutions will result in the maximum number of moles of metal deposited on passing the same amount of charge?