Electro chemistry practice · Mixed difficulty

What will be pH of aqueous solution of electrolyte in electrolytic cell during electrolysis of $\mathrm{CuS}{\mathrm{O}_4}\left( {aq} \right)$ between graphite electrodes?

The charge required to deposit $40.5 \mathrm{~g}$ of $\mathrm{Al}$ (atomic mass $=27.0 \mathrm{~g}$) from the fused $\mathrm{Al}_2\left(\mathrm{SO}_4\right)_3$ is:

Rusting of iron is catalysed by which of the following?

A $0.200 \mathrm{~M} \mathrm{~KOH}$ solution is electrolysed for $1.5 \mathrm{~h}$ using a current of $8.00 \mathrm{~A}$. How many moles of $\mathrm{O}_2$ were produced at the anode?

For complete reduction of 1 mole of nitrobenzene to aniline, charge needed will be ( $F$ represents Faraday's constant)

Small quantities of solutions of compounds $TX,TY$ and $TZ$ are put into separate test tubes containing X, Y and Z solutions. $TX$ does not react with any of these. $TY$ reacts with both X and Z. $TZ$ reacts with X. The decreasing order of ease of oxidation of the anions ${X^ - },{Y^ - },{Z^ - }$ is

Statement I: At the end of electrolysis using platinum electrodes an aqueous solution of copper sulphate turns colourless

Statement II: Copper in $\mathrm{CuSO}_4$ is converted to $\mathrm{Cu}(\mathrm{OH})_2$ during electrolysis

The ${\mathrm{\Lambda }^\infty }$ of $\mathrm{N}{\mathrm{H}_4}\mathrm{OH}$ at infinite dilution is …$S{\kern 1pt} {\kern 1pt} \mathrm{c}{\mathrm{m}^2}\mathrm{eq}{\mathrm{.}^{ - 1}}$ .Given $\lambda _{\mathrm{O}{\mathrm{H}^ - }}^\infty = 174,\lambda _{\mathrm{C}{\mathrm{l}^ - }}^\infty = 66$ and $\lambda _{\mathrm{N}{\mathrm{H}_4}\mathrm{Cl}}^\infty = 130{\kern 1pt} {\kern 1pt} {\rm{S {\kern 1pt} {\kern 1pt}c}}{\mathrm{m}^2}{\kern 1pt} {\kern 1pt}\mathrm{e}{\mathrm{q}^{ - 1}}:$

Calculate the electrode potential of given electrode at $25^{\circ} {C}$

${Pt} / {H}_2 / {H}^{+}({pH}=6)$

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

Statement I: A negative value of standard reduction potential means that reduction takes place on this electrode with reference to standard hydrogen electrode.

Statement II: The standard electrode potential of a half-cell has fixed value.

How much charge (in $\mathrm{F}$) must flow through solution during electrolysis of aq. $\mathrm{Na}_2 \mathrm{SO}_4$ at $0^{\circ} \mathrm{C}$ and 1 atm to produce 33.6 L of product gases at $50 \%$ current efficiency?

Find weight of Zinc in Zinc sulphate electrolysis $\mathrm{i}=0.015 \mathrm{~A,t} =15$ minutes

Which of the following statements is/are incorrect?

Find the emf of the cell in which the following reaction takes place at 298 K
$Ni(s) + 2A{g^ + }(0.001M) \to N{i^{2 + }}(0.001M) + 2Ag(s)$
(Given that $E_{cell}^ \circ = 10.5\,V,\,\frac{{2.303\,RT}}{F} = 0.059$ at 298 K)

Consider the following cell representation:
$\mathrm{Pt}(\mathrm{s})\left|\mathrm{Br}_2({l})\right| \mathrm{Br}^{\ominus}(0.010)|| \mathrm{H}^{\oplus}(0.030 \mathrm{~M})\left|\mathrm{H}_2(\mathrm{g})(1 \mathrm{~bar})\right| \mathrm{Pt}(\mathrm{s})$
The EMF of the above cell at $298 \mathrm{~K}$ is $-\mathrm{xV}$. Find $3 \mathrm{x}$ (nearest integer)

$\begin{aligned} & \text {[Given } \mathrm{E}^{\circ}_{\frac{1}{2}\mathrm{Br}_2 \mid \mathrm{Br}^{-}} \text{ (Reduction potential of } \mathrm{Br}_2)=+1.08 \mathrm{~V} \text {]} \end{aligned}$

The cell, $\mathrm{Zn}\left| {\mathrm{Z}{\mathrm{n}^{2 + }}\left( {1\mathrm{M}} \right)} \right|\left| {\mathrm{C}{\mathrm{u}^{2 + }}\left( {1\mathrm{M}} \right)} \right|\mathrm{Cu}$

($E_{\mathrm{cell}}^ \circ =$1.10 V), was allowed to be completely discharged at 298 K. The relative concentration of

$\mathrm{Z}{\mathrm{n}^{2 + }}$ to $\mathrm{C}{\mathrm{u}^{2 + }}\left( {\frac{{\left[ {\mathrm{Z}{\mathrm{n}^{2 + }}} \right]}}{{\left[ {\mathrm{C}{\mathrm{u}^{2 + }}} \right]}}} \right)$ is

Electrode potential of hydrogen electrode is …….. Volt.

If the following half cells have the $E^{\circ}$ values as $\mathrm{Fe}^{3+}+e^{-} \rightarrow \mathrm{Fe}^{2+} ; E^{\circ}=+0.77 \mathrm{~V}$ and $\mathrm{Fe}^{2+}+2 e^{-} \rightarrow \mathrm{Fe} ; E^{\circ}=-0.44 \mathrm{~V};$ the $E^{\circ}$ of the half-cell $\mathrm{Fe}^{3+}+3 e^{-} \rightarrow \mathrm{Fe}$ will be

A standard hydrogen electrode has Zero electrode potential because

An electronic conductor is

The SRP values of the elements A, B and C are 0.68, -2.50 and 0.50V respectively. The order of their reducing power is

Find the solubility product of a saturated solution of $\mathrm{Ag}_2 \mathrm{CrO}_4$ in water at $298 \mathrm{~K}$ if the emf of the cell $\mathrm{Ag} | \mathrm{Ag}^{+} \text{(satd. }\mathrm{Ag}_2 \mathrm{CrO}_4 \text{ soln.)}\| \mathrm{Ag}{ }^{+}(0.1 \mathrm{~M}) | \mathrm{Ag}$ is $0.164 \mathrm{~V}$ at $298 \mathrm{~K}.$

Which colourless gas evolves when $\mathrm{N}{\mathrm{H}_4}\mathrm{Cl}$ reacts with zinc in A dry cell battery?

Without losing its concentration ${ZnCl}_2$ solution cannot be kept in contact with

Molar conductance of an electrolyte increases with dilution according to the equation.

$\Lambda_{\mathrm{m}}=\Lambda_{\mathrm{m}}^{\circ}-\mathrm{A} \sqrt{\mathrm{C}}$

Which of the following statement is/are true:

A certain quantity of electricity is passed through aqueous solution of $\mathrm{AgN}{\mathrm{O}_3}$ and $\mathrm{CuS}{\mathrm{O}_4}$ connected in series. If Ag (at.wt.108) deposited at the cathode is 1.08 g then Cu deposited at the cathode is (at. wt. of Cu is 63.53 ):

The molecular conductivity and equivalent conductivity are same for the solution of :

Calculate the standard Gibbs free energy of

$\mathrm{Zn}(s)+\mathrm{Cu}^{2+}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+\mathrm{Cu}(s)$

The cell reaction of A cell is
$\mathrm{Mg}\left( s \right) + \mathrm{C}{\mathrm{u}^{2 + }}\left( {aq} \right) \to \mathrm{Cu}\left( s \right) + \mathrm{M}{\mathrm{g}^{2 + }}\left( {aq} \right)$
If the standard reduction potentials of Mg and Cu are – 2.37 and + 0.34 V respectively. The emf of the cell is