Electro chemistry practice · Mixed difficulty

Statement I: A metal having negative reduction
potential when dipped in the solution of its own
ions has a tendency to pass into the solution.

Statement II: Metals having negative reduction
potential have large hydration energy.

The reduction potential of hydrogen half – cell will be negative if:

A Galvanic cell is represented as: $\mathrm{Pt}, \mathrm{H}_2(0.1 \mathrm{~bar})\left|\mathrm{H}^{+}(\mathrm{aq})(2 \mathrm{~M}) \| \mathrm{M}^{+}(0.2 \mathrm{~M})\right| \mathrm{M}(\mathrm{s})$ [Given : $\mathrm{K}_{\mathrm{w}}=10^{-14}, \mathrm{E}_{\mathrm{M}^{+} / \mathrm{M}}^{\mathrm{o}}=0.03 \mathrm{~V}$]. The correct statement for the given Galvanic cell is:

Which of the following solutions of ${KCl}$ will have the highest value of specific conductance?

The molar conductivity at infinite dilution of $\mathrm{AgN}{\mathrm{O}_3},\mathrm{NaCl}$ and $\mathrm{NaN}{\mathrm{O}_3}$ are 116.5, 110.3 and 105.2 ${\rm{mho{\kern 1pt} {\kern 1pt} c}}{\mathrm{m}^2}{\kern 1pt} {\kern 1pt} \mathrm{mo}{\mathrm{l}^{ - 1}}$ respectively. The molar conductivity of AgCl is :

Which of the following statements is correct

Effect of dilution on conductivity of solution:

The electrolytic bath used in gold plating of copper articles contains :

The value of $\mathrm{\Lambda }_{eq}^\infty$ for $\mathrm{N}{\mathrm{H}_4}\mathrm{Cl},{\rm{NaOH {\kern 1pt}{\kern 1pt}and {\kern 1pt}{\kern 1pt}NaCl}}$ are respectively, 149.74, 248.1 and 126.4 ${\Omega ^{ - 1}}{\kern 1pt}{\kern 1pt}\mathrm{c}{\mathrm{m}^2}{\kern 1pt}{\kern 1pt}\mathrm{equi}{\mathrm{v}^{ - 1}}$). The value of $\mathrm{\Lambda }_{eq}^\infty$ of $\mathrm{N}{\mathrm{H}_4}\mathrm{OH}$ is

In a cell containing zinc electrode and standard hydrogen electrode(SHE), the zinc electrode acts as :

Conductance ‘$C$’ (in$S$) in directly proportional to the area of the electrode and concentration and inversely proportional to length of separation of electrode, the unit of constant of proportionality is:

When electric current is passed through acidified water for 1930 s, 1120mL of ${\mathrm{H}_2}$ gas is collected (at STP) at the cathode. What is the current passed in amperes?

Consider the following reaction at $1100^{\circ} \mathrm{C}$.
(1) $2 \mathrm{C}+\mathrm{O}_2 \longrightarrow 2 \mathrm{CO} \,\Delta \mathrm{G}^{\circ}=-460 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(2) $2 \mathrm{Zn}+\mathrm{O}_2 \longrightarrow 2 \mathrm{ZnO} \,\Delta \mathrm{G}^{\circ}=-360 \mathrm{~kJ} \mathrm{~mol}^{-1}$
based on these, select correct alternate

Anode in the Leclanche cell is

A dilute solution of sulphuric acid is electrolysed using a current of $0.10 \mathrm{~A}$ for 2 hours to produce hydrogen and oxygen gas. The total volume of gases produced at STP is ____$\mathrm{cm}^3$. (Nearest integer)
[Given : Faraday constant $\mathrm{F}=96500 \mathrm{C} \mathrm{mol}^{-1}$ at STP, molar volume of an ideal gas is $22.7 \mathrm{~L} \mathrm{~mol}^{-1}$ ]

Which of the following aqueous solution will have the maximum specific conductance?

The factors which influence the conductance of solution.

Two half cells have reduction potentials $-0.76 \mathrm{~V}$ and $0.13 \mathrm{~V}$ respectively. A galvanic cell is made from these two half cells. Which of the following statements is correct?

Which set of relationships could apply to the same electrochemical cell?

Cell constant has the unit:

Conductivity (Seimen's $S)$ is directly proportional to area of the vessel and the concentration of the solution in it and is inversely proportional to the length of the vessel, then constant of proportionality is expressed in:

SI unit of conductivity is :

The value of electronic charge is equal to :

Which does not get oxidised by bromine water?

Equivalent conductance of $0.1 \mathrm{~M} \mathrm{~HA}$ (weak acid) solution is $10 \mathrm{~S~cm}^2 \mathrm{~equivalent}^{-1}$ and that at infinite dilution is $200 \mathrm{~S~cm}^2 \mathrm{~equivalent}^{-1}.$ Hence $\mathrm{pH}$ of $\mathrm{HA}$ solution is

A substance that will reduce $\mathrm{A}{\mathrm{g}^ + }$ to Ag but will not reduce $\mathrm{N}{\mathrm{i}^{2 + }}$ to Ni is :

Consider the following ${E^\mathrm{o}}$ Values.
$E_{F{e^{3 + }}/F{e^{2 + }}}^\mathrm{o} = 0.77\,V\,;\,E_{S{n^{2 + }}/Sn}^\mathrm{o} = - 0.14\,V$
Under standard conditions, the potential for the reaction:
$Sn\left( s \right) + 2F{e^{3 + }}\left( {aq} \right) \to 2F{e^{2 + }}\left( {aq} \right) + S{n^{2 + }}\left( {aq} \right)$

Calculate $K_{\mathrm{a}}$ of acetic acid if its $0.05 \mathrm{~M}$ solution has molar conductivity of $7.814 \times 10^{-4} \, \Omega^{-1} \mathrm{~m}^2 \mathrm{~mol}^{-1}$ at $25^{\circ} \mathrm{C}.$ Given: $\Lambda_{\mathrm{m}}^{\circ}$ for $\mathrm{CH}_3 \mathrm{COOH}=3.907 \times 10^{-2} \, \Omega^{-1} \mathrm{~m}^2 \mathrm{~mol}^{-1}.$

Which of the following has negative value?

When 1 F of electricity is passed through acidulated water, ${\mathrm{O}_2}$ evolved is