Faraday’s Laws of Electrolysis

A current of $1.70 \mathrm{A}$ is passed through $300.0 \mathrm{mL}$ of $0.160 \mathrm{M}$ solution of ${\mathrm{ZnSO}}_4$ for $230 \mathrm{s}$ with a current efficiency $90\%$. Find out the molarity$\left(\mathrm{mol} {\mathrm{L}}^{-1}\right)$  of ${\mathrm{Zn}}^{2+}$after the deposition of $\mathrm{Zn}$. Assume the volume of the solution to remain constant during the electrolysis.

Electrolysis of dilute aqueous$\mathrm{NaCl}$ solution was carried out by passing $10$ milli ampere current. The time required to liberate $0.01 \mathrm{mol}$ of  ${\mathrm{H}}_2$ gas at the cathode is $(1 \mathrm{Faraday}=96500\hspace{0.17em}\hspace{0.17em}\mathrm{C}\hspace{0.17em}{\mathrm{mol}}^{-1})$:

Aluminium oxide may be electrolysed at  $\text{1}000°\text{C}$ to give Al metal (at mass = 27 amu, 1F = 96,500 C). To prepare 5.12 kg of Al would require

The weight of silver deposited when $0.2$ faraday current is passed through silver nitrate solution.

An electric current is passed through silver nitrate solution using silver electrodes. $15.28\mathrm{ }\mathrm{g}$ of silver was found to be deposited on cathode. What will be the weight of copper deposited on cathode if same amount of electricity is passed through copper sulphate solution using copper electrodes?

$\mathrm{Zn}$ amalgam is prepared by electrolysis of aqueous ${\mathrm{ZnCl}}_2$ using $\mathrm{Hg}$ cathode $(9 \mathrm{gm}).$ How much current is to be passed through ${\mathrm{ZnCl}}_2$ solution for $1000$ seconds to prepare a $\mathrm{Zn}$ amalgam with $25\% \mathrm{Zn}$ by weight $(\mathrm{Zn}=65.4)$

Same quantity of electricity was passed through solutions of salts of elements $\mathrm{X}, \mathrm{Y}$ and $\mathrm{Z}$ with atomic masses $7, 27$ and $48$ respectively. The masses of $\mathrm{X}, \mathrm{Y}$ and $\mathrm{Z}$ deposited were $2.1 \mathrm{g}, 2.7 \mathrm{g}$ and $7.2 \mathrm{g}$ respectively. The valence's of $\mathrm{X}, \mathrm{Y}$ and $\mathrm{Z}$ respectively are

Salts of $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ were electrolyzed under identical conditions using the same quantity of electricity. It was found that when $2.1 \mathrm{g}$ of $\mathrm{A}$ was deposited. The weights of $\mathrm{B}$ and $\mathrm{C}$ deposited were $2.7 \mathrm{g}$ and $9.6 \mathrm{g}$ respectively. If the atomic mass of $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ respectively are $7,27$ and $64,$ then the valancies of $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ respectively are ______

Oxidation of succinate ion produces ethylene and carbon dioxide gases. $0.2$  What is the total volume of gases (at both cathode and anode) at STP ($1 \mathrm{atm}$ and $273 \mathrm{K}$) On passing  $0.2$Faraday electricity through an aqueous solution of potassium succinate,?

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

What is the correct graph from the following? If during electrolysis the amount of product liberated at electrode is plotted against charge in Faraday.