During the electrolysis of ${\mathrm{CrCl}}_3$, chlorine gas is evolved at the anode and chromium is deposited at the cathode. How many grams of $\mathrm{Cr}$ and how many litres of chlorine (at NTP) are produced when a current of $6$$\mathrm{A}$ is passed for one hour? 

A current passes through two cells containing respectively-($\mathrm{i}$) ${\mathrm{CuSO}}_4$ solution between $\mathrm{Cu}$electrode and ($\mathrm{ii}$) ${\mathrm{AgNO}}_3$ solution between $\mathrm{Pt}$electrodes. Calculate the loss or gain in weight of the different electrodes in the time in which $40 \mathrm{cc}$ of oxygen at $\mathrm{NTP}$collects in the second cell. 

First cell $\left\{\begin{array}{l}0.228 \mathrm{g} \mathrm{Cu}\text{ deposited at cathode. }\\ 0.228 \mathrm{g} \mathrm{Cu}\text{ dissolved out from anode }\end{array}\right.$

$\mathrm{Ag}$is electro deposited on a metallic vessel of surface area $800 {\mathrm{cm}}^2$ by passing a current of $0.2$ amp for three hours. Calculate the thickness of silver deposited. (given density is $10.47 \mathrm{g}/\mathrm{cc}$). If thickness $= \mathrm{A}\times {10}^{-4} \mathrm{cm}.$

Give the value of A up to two places of decimal.

$50 \mathrm{mL}$ of hydrogen gas was collected over at $23°\mathrm{C}, 740 \mathrm{mmHg}$ barometric pressure. ${\mathrm{H}}_2$ was produced by the electrolysis of water. The voltage was constant at $2.1$ $\mathrm{volts}$, the current averaged $0.50 \mathrm{amp}$ for $12 \mathrm{minutes}$ and $20 \mathrm{seconds}$. Calculate the Avogadro's constant. 

Divide the answer by $1\times {10}^{23}$ and give the answer up to two places of decimal.

A current of $0.5 \mathrm{amp}$ is sent through a solution of ${\mathrm{CuSO}}_4$ for $20 \mathrm{minutes}$ using $\mathrm{Pt}$ electrodes.

(a) Calculate the weight of $\mathrm{Cu}$deposited.

(b) Find out the total number of copper atoms deposited. 

(Atomic mass of copper=$63.5$)

What current is required to pass $1 \mathrm{mole}$ of electrons per hour through an electrolytic bath? How many grams of $\mathrm{Al}$and $\mathrm{Cd}$will be liberated by $1 \mathrm{mole}$ of electrons?

(Atomic mass of $\mathrm{Al}=27, \mathrm{Cd}=112.4$)