Electro chemistry practice · Mixed difficulty

An electric current is passed through silver voltameter connected to a water voltameter. The cathode of the silver voltameter weighed $0.108 \mathrm{~g}$ more at the end of the electrolysis. The volume of oxygen evolved at STP is

Salts of metals ${X}, {Y}$ and ${Z}$ are electrolysed under identical condition using same quantity of electricity. It was observed that $4.2 {~g}$ of ${X}, 5.4 {~g}$ of ${Y}$ and $19.2 {~g}$ of ${Z}$ were deposited at respective cathode. If the atomic weights of ${X}, {Y}, {Z}$ are 7 , 27 and 64 respectively, then their ratio of valencies is

Electrolysis of aq. Solution of $\mathrm{LiCl}$ shows :

Maximum number of mole of oxygen gas that can be obtained by the electrolytic decomposition of 90 g of water will be:

In the electrochemical cell,
${A}({s})+{B}^{2+}({aq}) \longrightarrow {A}^{2+}({aq})+{B}({s})$

Increase in the concentration of $\mathrm{A}^{2+}$

What pressure (bar) of $\mathrm{H}_2$ would be required to make emf of hydrogen electrode zero in pure water at $25^{\circ} \mathrm{C}$?

Given the ionic equivalent conductivities for the following ions:

$\lambda^{\circ}{ }_{\text {eq }} \mathrm{K}^{+}=73.5 \mathrm{~cm}^2 \mathrm{ohm}^{-1} \mathrm{eq}^{-1}$

$\lambda^{\circ}{ }_{\text {eq }} \mathrm{Al}^{3+}=149 \mathrm{~cm}^2 \mathrm{ohm}^{-1} \mathrm{eq}^{-1}$

$\lambda^{\circ}{ }_{\text {eq }} \mathrm{SO}_4{ }^{2-}=85.8 \mathrm{~cm}^2 \mathrm{ohm}^{-1} \mathrm{eq}^{-1}$

The $\Lambda_{\text {eq }}^{\circ}$ for potash alum $\left(\mathrm{K}_2 \mathrm{SO}_4 \cdot \mathrm{Al}_2\left(\mathrm{SO}_4\right)_3\right.$. $24 \mathrm{H}_2 \mathrm{O}$ ) is

$\mathrm{Cu} + 2\mathrm{HCl} \to \mathrm{CuC}{\mathrm{l}_2} + {\mathrm{H}_2}\left( \mathrm{g} \right)$

$\left[ {E_{C{u^{2 + }}/Cu}^ \circ = + 0.34V} \right]$

$\mathrm{Zn} + 2\mathrm{HCl} \to \mathrm{ZnC}{\mathrm{l}_2} + {\mathrm{H}_2}\left( \mathrm{g} \right)$

$\left[ {E_{Z{n^{2 + }}/Zn}^ \circ = - 0.76V} \right]$

$\mathrm{Ag} + 2\mathrm{HCl} \to \mathrm{AgCl} + \frac{1}{2}{\mathrm{H}_2}\left( \mathrm{g} \right)$

$\left[ {E_{A{g^ + }/Ag}^ \circ = + 0.80V} \right]$

Which of the following reaction is feasible ?

The standard electrode potential is measured by

The limiting molar conductivity of calcium acetate is

Select the appropriate statement for Daniell cell containing $\mathrm{Cu}^{2+}$ and $\mathrm{Zn}^{2+}$ ions.

$0.5 \mathrm{~F}$ charge is passed through $1 \mathrm{~L}, 1 \mathrm{~M}\,\, {CuCl}{ }_2(\mathrm{aq})$, using inert electrodes. Final concentration of ${Cu}^{2+}$ in the solution will be :-

Equivalent conductivity of $\mathrm{Fe}_2\left(\mathrm{SO}_4\right)_3$ is related to molar conductivity by the expression:

Find the standard cell potential involving the cell reaction:

${In}^{2+}+{Cu}^{+2} \rightarrow {In}^{+3}+{Cu}^{+} \text {, at } 298 {~K}$

Given:

${E}_{{Cu}^{+2} / {Cu}^{+}}^0={X}_1 {~V}, {E}_{{In}^{3+} / {In}^{+}}^0={X}_2 {~V} {E}_{{In}^{2+} / {In}^{+}}^0={X}_3 {~V}$

0.04 $N$ solution of a weak acid has conductivity $4.23 \times {10^{ - 4}}{\rm{mho {\kern 1pt}{\kern 1pt}c}}{\mathrm{m}^{ - 1}}$ . If the degree of dissociation of acid at this dilution is 0.0612, then equivalent conductivity at infinite dilution is ……${\rm{mho {\kern 1pt}{\kern 1pt}c}}{\mathrm{m}^2}\mathrm{eq}{.^{ - 1}}$ ∶

Which metal is most readily corroded in moist air?

Total charge required for the oxidation of two moles ${Mn}_3 {O}_4$ into ${MnO}_4^{2-}$ in presence of alkaline medium is

Galvanised iron sheets are coated with

The most durable metal plating on iron to protect against corrosion is

What weight of copper will be deposited by passing 2 faraday of electricity through a solution of Cu(II) salt?

Assertion (A) At the end of electrolysis using platinum electrodes, an aqueous solution of $\mathrm{CuSO}_4$ turns colourless.

Reason (R) During the electrolysis $\mathrm{CuSO}_4$ changes to $\mathrm{Cu}(\mathrm{OH})_2$ during electrolysis.

Three faradays of electricity is passed through three electrolytic cells connected in series containing ${Ag}^{+}, {Ca}^{2+}$ and ${Al}^{3+}$ ions respectively. The molar ratio in which the three metal ions are liberated at the electrodes is

Also the [${\mathrm{H}^ + }$] for problem 9 using the same data is :

At ${18^ \circ }\mathrm{C}$ the conductance of ${\mathrm{H}^ + }$ and $\mathrm{C}{\mathrm{H}_3}\mathrm{CO}{\mathrm{O}^ - }$ at infinite dilution are 315 and 35 ${\rm{mho {\kern 1pt} {\kern 1pt} c}}{\mathrm{m}^2}{\kern 1pt} {\kern 1pt} \mathrm{e}{\mathrm{q}^{ - 1}}$ respectively. The equivalent conductivity of $\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}$ at infinite dilution is ……${\rm{mho {\kern 1pt} {\kern 1pt} c}}{\mathrm{m}^2}{\kern 1pt} {\kern 1pt} \mathrm{eq}{.^{ - 1}}$

The value of electrode potential $\left(10^{-4} \, \mathrm{M}\right) {H}^{+}\left|{H}_2(1 \mathrm{~atm})\right| {Pt}$ at $298 \mathrm{~K}$ would be

Assume that during electrolysis of $AgN{O_3}$, only ${H_2}O$ is electrolysed and ${O_2}$ is formed as: $2{H_2}O \to 4{H^ + } + {O_2} + 4{e^ - }$ . ${O_2}$ formed at NTP due to passage of 2A of current for 965 s is

During electrolysis of an aqueous solution of $\mathrm{C}{\mathrm{u}^{2 + }}$ sulphate, 0.635 g of copper was deposited at cathode. The amount of electricity consumed in coulomb is :

Assertion: More negative the electrode potential greater is the power to act as oxidising agent.

Reason: As the electrode potential becomes more negative there is greater tendency to undergo oxidation.

Mark the false statement?

The oxidation potential values of A, B, C and D are -0.03, +0.108 V,-0.07 V and +0.1 V respectively. The non-spontaneous cell reaction takes place between