Faraday's Law of Electrolysis

Find out the volume of gases evolved by passing $0.965 \mathrm{A}$ current for $1\mathrm{hr}$ through an aqueous solution of ${\mathrm{CH}}_3\mathrm{COONa}$ at $25°\mathrm{C}$ and $1 \mathrm{atm}$.

A current of $9.65$ $\mathrm{ampere}$is passed through the aqueous solution $\mathrm{NaCl}$ using suitable electrodes for $1000 \mathrm{s}$. The amount of $\mathrm{NaOH}$ formed during electrolysis is:

A current of $2 \mathrm{A}$ was passed for $1 \mathrm{h}$ through a solution of ${\mathrm{CuSO}}_4. 0.237 \mathrm{g}$ of ${\mathrm{Cu}}^{2+}$ ions were discharged at cathode. The current efficiency is:

Three faradays of electricity was passed through an aqueous solution of iron $\left(\mathrm{II}\right)$ bromide. The mass of iron metal (at. mass $56$) deposited at the cathode is -

Electrolysis of a solution of ${\mathrm{HSO}}_4^{-}$ ions produces ${\mathrm{S}}_2{\mathrm{O}}_8^{--}$ Assuming $75\%$ current efficiency, what current should be employed to achieve a production rate of $1$ mole of ${\mathrm{S}}_2{\mathrm{O}}_8^{--}$ per hour ?

A current of $2.68 \mathrm{A}$ is passed for one hour through an aqueous solution of $\mathrm{CuSO},$ using copper electrodes. Select the correct statement(s) from the following:

How long (approximate) should water be electrolysed by passing through $100$ amperes current so that the oxygen released can completely burn $27.66 \mathrm{g}$ of diborane? (Atomic weight of $\mathrm{B}=10.8 \mathrm{u}$)

A current of $5.0 \mathrm{A}$ flows for $4.0 \mathrm{h}$ through an electrolytic cell containing a molten salt of metal $\mathrm{M}$. This results in deposition of $0.25 \mathrm{mol}$ of the metal $\mathrm{M}$ at the cathode. The oxidation state of $\mathrm{M}$ in the molten salt is $(1$ Faraday $=96485 \mathrm{C} {\mathrm{mol}}^{-1})$

The salts of $\mathrm{A}$ (atomic $\mathrm{mass} 15$ ), $\mathrm{B}$ (atomic$\mathrm{mass} 27$) and $\mathrm{C}$ (atomic $\mathrm{mass} 48$) were electrolysed using same amount of charge. It was found that when $4.5 \mathrm{g}$ of $\mathrm{A}$ was deposited, the mass of $\mathrm{B}$ and $\mathrm{C}$ deposited were $2.7 \mathrm{g}$ and $9.6 \mathrm{g}.$The valencies of $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$, respectively.

How many faradays are required to reduce one $\mathrm{mol}$ of ${\mathrm{MnO}}_4^{-}$ to ${\mathrm{Mn}}^{2+}$

The amount of copper (At. wt. $63.54$ ) deposited by passing $0.2$ faraday of electricity through copper sulphate is

An electric current is passed through a silver voltameter connected to a water voltameter. $0.324 \mathrm{g}$ of silver was deposited on the cathode of the silver voltameter. The volume of oxygen evolved at $\mathrm{NTP}$ is :

One of the methods of preparation of per disulphuric acid, ${\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_8,$ involve electrolytic oxidation of ${\mathrm{H}}_2{\mathrm{SO}}_4$ at anode $\left(2{\mathrm{H}}_2{\mathrm{SO}}_4⟶{\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_8+2{\mathrm{H}}^{+}+2{\mathrm{e}}^{-}\right)$ with oxygen and hydrogen as by-products. In such an electrolysis, $9.722 \mathrm{L}$ ${\mathrm{H}}_2$ of and $2.35 \mathrm{L}$ ${\mathrm{O}}_2$ were generated at $\mathrm{STP}$ . What is the weight of ${\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_8$ formed'?

The quantity of electricity which deposits $1.08 \mathrm{g}$ of silver from ${\mathrm{AgNO}}_3$ solution is:

Three moles of electrons are passed through three solutions in succession containing ${\mathrm{AgNO}}_3, {\mathrm{CuSO}}_4$ and ${\mathrm{AuCl}}_3$, respectively. The molar ratio of amounts of cations reduced at cathode will be:

Four moles of electrons were transferred from anode to cathode in an experiment on electrolysis of water. The total volume of the two gases (dry and at $\mathrm{STP}$) produced will be approximately (in litres).

During the preparation of ${\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_8$ (per disulphuric acid) ${\mathrm{O}}_2$ gas also releases at anode as byproduct. When $9.72 \mathrm{L}$ of ${\mathrm{H}}_2$ releases at cathode and $2.35 \mathrm{L}$ ${\mathrm{O}}_2$ at anode at $\mathrm{STP}$, the weight of ${\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_8$ produced in gram is:

Electrolysis of a solution of ${\mathrm{MnSO}}_4$ in aqueous sulphuric acid is a method for the preparation of ${\mathrm{MnO}}_2$. Passing a current of $27 \mathrm{A}$ for $24$ hours gives $1 \mathrm{kg}$ of ${\mathrm{MnO}}_2$. The current efficiency in this process is:

One $\mathrm{g}$ equivalent of $\mathrm{Na}$metal is formed from electrolysis of fused $\mathrm{NaCl}$. No. of moles of $\mathrm{Al}$from the fused ${\mathrm{Na}}_3$ ${\mathrm{AlF}}_6$ with the same current passed is:

A current of $0.5 \mathrm{ampere}$, when passed through ${\mathrm{AgNO}}_3$ solution for $193 \mathrm{seconds}$, deposited $0.108 \mathrm{g}$ of $\mathrm{Ag}$. The equivalent weight of $\mathrm{Ag}$ is: