When the same quantity of electricity is passed through aqueous $AgNO_3$ and $H_2SO_4$ solutions connected in series,$5.04 \times 10^{-2} \ g$ of $H_2$ is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen $= 1.008$,silver $= 108$)

When a current of $2 \ A$ is passed for $2 \ hours$ through a copper voltameter,$W \ g$ of copper is deposited. If a current of $1 \ A$ is passed for $4 \ hours$ through the same voltameter,how much copper will be deposited?

How many grams of chlorine gas will be produced as a product when a current of $2 \ A$ is passed through a concentrated aqueous solution of $NaCl$ for $30 \ \text{minutes}$?

The chemical equivalents of copper and silver are $32$ and $108$ respectively. When copper and silver voltameters are connected in series and electric current is passed through for some time,$1.6 \ g$ of copper is deposited. Then,the mass of silver deposited will be .......... $g$.

Three electrolytic cells $A, B, C$ containing solutions of $ZnSO_{4}, AgNO_{3}$ and $CuSO_{4}$ respectively are connected in series. $A$ steady current of $1.5 \ A$ was passed through them until $1.45 \ g$ of silver deposited at the cathode of cell $B$. How long did the current flow? What mass of copper and zinc were deposited?

The electrochemical equivalent $Z$ of any element can be obtained by multiplying the electrochemical equivalent of hydrogen with