Interpretation of Faraday's Second Law

Electric current is passed through two cells $\text{'}\mathrm{A}\text{'}$ $\text{'}\mathrm{B}\text{'}$ in series. Cell$\text{'}\mathrm{A}\text{'}$ contains an aqueous solution of ${\mathrm{Ag}}_2{\mathrm{SO}}_4$ and platinum electrodes. The cell  $\text{'}\mathrm{B}\text{'}$ contains an aqueous solution of ${\mathrm{CuSO}}_4$ and $\mathrm{Cu}$ electrodes. The current is passed till $1.6 \mathrm{g}$ of oxygen is liberated at the anode of cell $\text{'}\mathrm{A}\text{'}.$

Calculate the quantities of substances deposited at the cathodes of the two cells.$(\mathrm{Ag}=108, \mathrm{Cu}=63.5)$

Electric current is passed through two cells$\text{'}\mathrm{A}\text{'}$and $\text{'}\mathrm{B}\text{'}$ in series. Cell $\text{'}\mathrm{A}\text{'}$ contains an aqueous solution of ${\mathrm{Ag}}_2{\mathrm{SO}}_4$ and platinum electrodes. The cell ' ${\mathrm{B}}^{\text{'}}$ contains aqueous solution of ${\mathrm{CuSO}}_4$ and $\mathrm{Cu}$ electrodes. The current is passed till $1.6 \mathrm{g}$ of oxygen is liberated at the anode of cell $\text{'}\mathrm{A}\text{'}$.

Give equations for the reaction taking place at each electrode.

For the electrolytic production of ${\mathrm{NaClO}}_4$ from ${\mathrm{NaClO}}_3$ as per reactions:

${\mathrm{ClO}}_3^{-}+{\mathrm{H}}_2\mathrm{O}\to {\mathrm{ClO}}_4^{-}+2{\mathrm{H}}^{+}+2e^{-}$

The aqueous solutions of the following substances were electrolysed. In which case, the $\mathrm{pH}$ of the solution does not change if inert electrodes are used?

In which of the following aqueous solutions, ${\mathrm{H}}_2$ and ${\mathrm{O}}_2$ are not liberated at cathode and anode respectively on electrolysis using inert electrodes?

Which of the following processes is used in the extraction metallurgy of $\mathrm{Mg}$?

In the electrolysis of ${\mathrm{H}}_2\mathrm{O}$, $11.2 \mathrm{L}$ of ${\mathrm{H}}_2$ was liberated at cathode at $\mathrm{NTP}$. How much ${\mathrm{O}}_2$ will be liberated at anode under the same conditions?

In a fuel cell, hydrogen and oxygen react to produce electricity. In the process, hydrogen gas is oxidised at the anode and oxygen at the cathode. If $67.2 \mathrm{litres}$ of ${\mathrm{H}}_2$ at $\mathrm{STP}$ reacts in $15 \mathrm{minutes}$, what is the average current produced? If the entire current is used for electrodeposition of copper from $\mathrm{Cu} \left(\mathrm{II}\right)$ solution, how many $\mathrm{grams}$ of copper will be deposited?

$\begin{array}{l}\text{Anode reaction: }{\mathrm{H}}_2+2{\mathrm{OH}}^{-}\to 2{\mathrm{H}}_2\mathrm{O}+2{\mathrm{e}}^{-}\\ \text{Cathode reaction: }{\mathrm{O}}_2+2{\mathrm{H}}_2\mathrm{O}+4{\mathrm{e}}^{-}\to 4{\mathrm{OH}}^{-}\end{array}$

An electric current is passed through a solution of

$\left(\mathrm{i}\right)$ silver nitrate 

$\left(\mathrm{ii}\right)$ a solution of $10 \mathrm{g}$ of copper sulphate $\left({\mathrm{CuSO}}_4 .5{\mathrm{H}}_2\mathrm{O}\right)$ crystals in $500 \mathrm{mL}$ of water, with platinum electrodes being used in each case.

After $30 \mathrm{minutes}$, it was found that $1.307 \mathrm{g}$ of silver has been deposited. What was the concentration of copper, expressed as $\mathrm{grams}$ of copper per $\mathrm{liter}$, in the copper sulphate solution after electrolysis?

$0.2964 \mathrm{g}$ of $\mathrm{Cu}$ was deposited on passage of a current of $0.5 \mathrm{amp}$ for $30 \min$, through a solution of copper sulphate. Calculate the atomic weight of $\mathrm{Cu}$.

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 $\mathrm{Al}=27, \mathrm{Cd}=112.4$)

The water is electrolysed in a cell, hydrogen is liberated at one electrode and oxygen is simultaneously liberated at the other. In particular experiment hydrogen and oxygen so produced were collected together and the total volume measured $16.8 \mathrm{mL}$ at $\mathrm{NTP}$. How many coulombs were passed through the cell in the experiment?

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

In an electrolysis experiment, the current was passed for $5 \mathrm{h}$ through two cells connected in series. The first cell contains a solution of gold and the second contains ${\mathrm{CuSO}}_4$ solution. $9.85 \mathrm{g}$ of gold was deposited in the first cell. If the oxidation number of gold is $+3,$ find the amount of $\mathrm{Cu}$ deposited on the cathode of the second cell. Also, calculate the magnitude of the current in amperes. 

At the Nangal fertiliser plant in Punjab, hydrogen is produced by the electrolysis of water. This hydrogen is used for the production of ammonia and nitric acid (by oxidation of ammonia). If the average production of ammonium nitrate is $5000 \mathrm{kg}/\mathrm{day}$, the daily consumption of electricity per day is $\mathrm{x} \times {10}^5$. 

Give thevalue of $\mathrm{x}$ to the nearest integer value.

A steady current passing through a solution of ${\mathrm{AgNO}}_3$ deposits $0.50 \mathrm{g}$ of $\mathrm{Ag}$ in $1 \mathrm{h}$. Calculate the number of coulombs. What volume of hydrogen at $27°\mathrm{C}$ and $750 \mathrm{mm}$ pressure would the same current liberate in one hour?

A spoon used as a cathode is dipped in ${\mathrm{AgNO}}_3$ solution and a current of $0.2$ $\mathrm{A}$ is passed for one hour. Calculate

(a) how much silver plating has occurred?

(b) how many electrons were involved in the process?

(c) what amount of copper would have been plated under similar conditions?