Electro chemistry practice · Mixed difficulty

Assertion: On increasing dilution, the specific conductance keep on increasing.

Reason: On increasing dilution, degree of ionisation ofweak electrolyte increases and molality of ions also increases.

In mercury cell electrolyte used is

For cell reaction,

$\mathrm{Zn} + \mathrm{C}{\mathrm{u}^{2 + }} \to \mathrm{Z}{\mathrm{n}^{2 + }} + \mathrm{Cu}$

Cell representation is

Four colourless salt solutions are placed in separate test tubes and a strip of copper is placed in each. Which solution finally turns blue?

Correct order of limiting molar conductivity of the given ions is

When lead accumulator is charged, it is :

The number of electrons involved in the reaction when a faraday of electricity is passed through an electrolyte in solution is :

On the basis of electrochemical theory of aqueous corrosion, the reaction occurring at the cathode is

Statement (S): Speed of ions depends upon nature of ions only.
Explanation (E): Mobility of ions depends upon mass, charge and size of ions only.

Following cell has EMF $0.7995 \mathrm{~V}$.

$\mathrm{Pt}\left|\mathrm{H}_2(1 \mathrm{~atm})\right| \mathrm{HNO}_3(1 \mathrm{M}) \| \mathrm{AgNO}_3(1 \mathrm{M}) \mid \mathrm{Ag}$

If we add enough $\mathrm{KCl}$ to the $\mathrm{Ag}$ cell so that the
final $\mathrm{Cl}^{-}$is $1 \mathrm{M}$. Now the measured emf of the cell is $0.222 \mathrm{~V}$. The $\mathrm{K}_{s p}$ of $\mathrm{AgCl}$ would be-

Faraday's law of electrolysis are related to the

A hydrogen gas electrode is made by dipping platinum wire in a solution of HCl of pH = 4 and passing hydrogen gas around the platinum wire at one atm pressure and at 298 K. The reduction potential of the hydrogen electrode would be

A cell with two electrodes, one of grey tin and the other white tin, both dipping in solution of ${\left( {\mathrm{N}{\mathrm{H}_4}} \right)_2}\mathrm{SnC}{\mathrm{l}_6}$ showed zero e.m.f. at ${18^ \circ }C$. What conclusion may be drawn from this?

1.05 g of lead ore containing impurity of Ag was dissolved in $\mathrm{HN}{\mathrm{O}_3}$ and the volume was made 350 mL. An Ag electrode was dipped in the solution. $\mathrm{Pt}\left( {{\mathrm{H}_2}} \right)\left| {{\mathrm{H}^ + }\left( {1\mathrm{M}} \right)} \right|\left| {\mathrm{A}{\mathrm{g}^ + }} \right|\mathrm{Ag}$.
The${E_{\mathrm{cell}}}$ is 0.503 V at 298 K.The percent of lead in the ore is ($E_{\mathrm{A}{\mathrm{g}^ + }|\mathrm{Ag}}^ \circ = 0.80\mathrm{V}$)

Electrolysis of dilute aqueous NaCl solution was carried out by passing 10mA current. The time required to liberate 0.01 mole of ${\mathrm{H}_2}$ gas at the cathode is ($1\mathrm{F} = 96500{\kern 1pt}{\kern 1pt}{\rm{C{\kern 1pt}{\kern 1pt}mo}}{\mathrm{l}^{ - 1}}$ )

For a given cell reaction; $Cr + 3{H_2}O + OC{l^ - } \to C{r^{+3}}+3C{l^ - } + 6O{H^ - },$ the species undergoing reduction is :

A galvanic cell is composed of two hydrogen electrodes, one of which is a standard one. In which of the following solutions should the other electrode be immersed to get maximum e. m. f.?

Which is not true for a standard hydrogen electrode?

Iron can be prevented from rusting by

The potential of Hydrogen electrode at ${P^H} = 1$ is

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?

Which equation gives relation between concentration of ions is solution, electrode potential ($E$) and standard electrode potential $\left(E^0\right)$

A silver cup is plated with silver by passing 965 C of electricity. The amount of Ag deposited is

When during electrolysis of a solution of a $\mathrm{AgN}{\mathrm{O}_3},9650\mathrm{C}$ of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be

The standard electrode potential for the half – cell reactions are
$\mathrm{Z}{\mathrm{n}^{2 + }} + 2{e^ - } \to \mathrm{Zn};{E^ \circ }$ = -0.76 V
$\mathrm{F}{\mathrm{e}^{2 + }} + 2{e^ - } \to \mathrm{Fe};{E^ \circ }$ = -0.44 V
The emf of the cell reaction,
$\mathrm{F}{\mathrm{e}^{2 + }} + \mathrm{Zn} \to \mathrm{Z}{\mathrm{n}^{2 + }} + \mathrm{Fe}$ is

On passing electricity through dil. ${H_2}S{O_4}$ solution, the amount of substance liberated at the cathode and anode are in the ratio

What is the number of Faraday's of charge, that should be required to convert one mole of $\mathrm{FeCr}_2 \mathrm{O}_4$ to $\mathrm{Fe}^{3+}$ an $\mathrm{CrO}_4^{2-}$ through an electrolytic oxidation process consider the current efficiency to be $87.5 \%$ ?

If the molar conductance value of $\mathrm{C}{\mathrm{a}^{2 + }}$ and $\mathrm{C}{\mathrm{l}^ - }$ at infinite dilution are respectively
$118.88 \times {10^{ - 4}}{\mathrm{m}^2}\mathrm{mho}{\kern 1pt} {\kern 1pt} {\kern 1pt} \mathrm{mo}{\mathrm{l}^{ - 1}}$ and $77.33 \times {10^{ - 4}}{\mathrm{m}^2}\mathrm{mho}{\kern 1pt} {\kern 1pt} {\kern 1pt} \mathrm{mo}{\mathrm{l}^{ - 1}}$ then that of $CaC{l_2}$ is (in ${\mathrm{m}^2}\mathrm{mho}{\kern 1pt} {\kern 1pt} {\kern 1pt} \mathrm{mo}{\mathrm{l}^{ - 1}}$)

The emf of the cell, $\left( {{E_{\mathrm{Z}{\mathrm{n}^{2 + }}/\mathrm{Zn}}} = - 0.76V} \right)$

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

$\left( {{E_{\mathrm{C}{\mathrm{u}^{2 + }}/\mathrm{Cu}}} = + 0.34V} \right)$ will be

Statement (S): A graph plotted between ${\Lambda _v}\,vs.\,{c^{1/2}}$ gives a straight line with slope equal to $- A$ and intercept equal to ${\Lambda _\infty }$
Explanation (E): The value of $A$ for a given solvent and temperature depends upon the nature of electrolyte, i.e., charge on cation or anion furnished by electrolyte on dissolution.