Electro chemistry practice · Mixed difficulty

The equivalent conductance of $NaCl$ at concentration $C$ and at infinite dilution are ${\lambda _C}$ and ${\lambda _\infty }$, respectively. The correct relationship between ${\lambda _C}$ and ${\lambda _\infty }$ is given as (where, the constant $B$ is positive)

When an electric current is passed through an aqueous solution of sodium chloride :

${E^ \circ }$ values of $M{g^{(2 + )}}$ / Mg is -2.37 V, of $\mathrm{Z}{\mathrm{n}^{2 + }}$ / Zn is -0.76 V and $\mathrm{F}{\mathrm{e}^{2 + }}$ / Fe is -0.44 V.
Which of the statements is correct?

What would be the ratio of moles each of $A{g^ + },\,C{u^{ + 2}},\,F{e^{ + 3}}$ ions would be deposited by passage of same quantity of electricity through solutions of their salts

The cell reaction of the galvanic cell

$\mathrm{Cu}\left( s \right)\left| {\mathrm{C}{\mathrm{u}^{2 + }}\left( {aq} \right)} \right|\left| {\mathrm{H}{\mathrm{g}^{2 + }}\left( {aq} \right)} \right|\mathrm{Hg}\left( l \right)$ is

In an electrolytic cell, the anode and cathode are respectively represented as :

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

The reduction electrode potential, E of 0.1 M solution of ${M^ + }$ ions

$\left( {{E_{RP}} = - 2.36V} \right)$ is

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

In the electrochemical cell
$\mathrm{Zn|ZnS}{\mathrm{O}_4}(0.01\mathrm{M})||\mathrm{CuS}{\mathrm{O}_\mathrm{4}}(1.0\mathrm{M})\mathrm{|Cu,}$ the emf of this Daniel cell is ${\mathrm{E}_1}.$ When the concentration of $\mathrm{ZnS}{\mathrm{O}_4}$ is changed to 1.0 M and that of $\mathrm{CuS}{\mathrm{O}_\mathrm{4}}$ changed to 0.01 M, the emf changes to ${\mathrm{E}_2}.$ From the following , which one is the relationship between ${\mathrm{E}_\mathrm{1}}\mathrm{ \;and\;}\,{\mathrm{E}_2}\,?$ (Given, $\frac{{\mathrm{RT}}}{\mathrm{F}} = 0.059$)

The electrochemical equivalent of a substance is the mass of the substance liberated on passing a current of

The ionic conductance of $\mathrm{B}{\mathrm{a}^{2 + }}$ and $\mathrm{C}{\mathrm{l}^ - }$ are respectively 127 and 76 ${\Omega ^{ - 1}}\mathrm{c}{\mathrm{m}^2}$ at infinite dilution. The equivalent conductance (in ${\Omega ^{ - 1}}\mathrm{c}{\mathrm{m}^2}$) of $\mathrm{BaC}{\mathrm{l}_2}$ at infinite dilution will be

At 298 K, the standard electrode potentials of $C{u^{2 + }}/Cu,Z{n^{2 + }}/Zn,F{e^{2 + }}/Fe\,\,\mathrm{and}\,\,A{g^ + }/Ag$ are 0.34 V, - 0.76 V, - 0.44 V and 0.80 V, respectively.
On the basis of standard electrode potential, predict which of the following reaction cannot occur?

A cell necessarily does not contain :

Select the correct statements among the following.

(i) Copper sulphate solution can't be stored in a zinc pot.

(ii) The potential of individual half cell can be measured at $298 \mathrm{~K}$ and at 1 bar pressure.

(iii) Copper can dissolve in dil. $\mathrm{HCl}$ but it cannot dissolve in nitric acid due to passive nature of nitrate ion towards copper.

(iv) Platinum and gold electrodes can be used both as anode and cathode.

Which of the following metal has the highest conductivity at room temperature ?

Stainless steel does not rust because

Rust is a mixture of :

Consider the reaction of extraction of gold from its ore:

$\begin{aligned} & \mathrm{Au}(\mathrm{s})+2 \mathrm{CN}^{-}(\mathrm{aq})+\frac{1}{4} \mathrm{O}_2(\mathrm{g})+\frac{1}{2} \mathrm{H}_2 \mathrm{O}({l}) \rightarrow \mathrm{Au}(\mathrm{CN})_2{ }^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \end{aligned}$

Use the following data to calculate $\Delta G^{\circ}$ for the above reaction.

$\begin{aligned} & K_{\mathrm{f}}\left[\mathrm{Au}(\mathrm{CN})_2^{-}\right] =X \\ & \mathrm{O}_2+2 \mathrm{H}_2 \mathrm{O}+4 \mathrm{e}^{-} \rightarrow 4 \mathrm{OH}^{-} ; E^{\circ}=+0.41 \mathrm{~V} \\ & \mathrm{Au}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Au} ; E^{\circ}=+1.50 \mathrm{~V} \\ & \mathrm{Au}^{3+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Au}^{+} ; E^{\circ}=+1.40 \mathrm{~V} \end{aligned}$

Normal $\mathrm{Al} - \mathrm{AlC}{\mathrm{l}_3}$ coupled with normal hydrogen electrode gives an e.m.f. of 1.66 V. The standard oxidation electrode potential of aluminium is :

According to Faraday’s first law of electrolysis mass of substances liberated is equal to

The electroplating with chromium is undertaken because :

The resistance of 0.01 N solution of an electrolyte was found to be 210 ohm at 298 K, using a conductivity cell of cell constant $0.66\mathrm{c}{\mathrm{m}^{ - 1}}$ . The equivalent conductivity of solution is :

Coulomb is the quantity of current defined as :

The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the redox reaction of the cell is

Given that $\mathrm{E}_{\mathrm{Fe}^{3+}/\mathrm{Fe}^{2+}}^{\circ}=-0.36 \mathrm{~V}$ and $\mathrm{E}_{\mathrm{Fe}^{2+}/\mathrm{Fe}}^{\circ}=-0.439 \mathrm{~V}$ respectively. Therefore value of $\mathrm{E}_{\mathrm{F}^{3+}, \mathrm{Fe}^{2+} /\mathrm{Pt}}^{\mathrm{o}}$ is:

${\mathrm{H}_2}$ cannot be displaced by

When silver nitrate solution is added to potassium iodide solution then the sol produced is

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

Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are