List of top Chemistry Questions on Electrochemistry asked in JEE Main

molar ionic conductivities of a divalent cation and anion are \(57 \, \text{S cm}^2 \text{mol}^{-1}\) and \(73 \, \text{S cm}^2 \text{mol}^{-1}\), respectively. The molar conductivity of the solution of an electrolyte with the above cation and anion will be:

The reaction at cathode in the cells commonly used in clocks involves.

Identify the factor from the following that does not affect electrolytic conductance of a solution.

The metals that are employed in the battery industries are
A. Fe 
B. Mn 
C. Ni 
D. Cr 
E. Cd 
Choose the correct answer from the options given below:

Which out of the following is a correct equation to show change in molar conductivity with respect to concentration for a weak electrolyte, if the symbols carry their usual meaning

One Faraday of electricity liberates \(x×10^{−1 }\)gram atom of copper from copper sulphate, x is ______.

The values of conductivity of some materials at \( 298.15 \, \text{K} \) in \( \text{S m}^{-1} \) are:
\( 2.1 \times 10^3, \, 1.0 \times 10^{-16}, \, 1.2 \times 10^1, \, 3.91, \, 1.5 \times 10^{-2}, \, 1 \times 10^{-7}, \, 1.0 \times 10^3 \).
The number of conductors among the materials is ______.

Match List I with List II

LIST-I (Cell)	LIST-II (Use/Property/Reaction)
A. Leclanche cell	IV. Reaction at anode Zn → Zn2+ + 2e-
B. Ni-Cd cell	III. Rechargeable
C. Fuel cell	I. Converts energy of combustion into electrical energy
D. Mercury cell	II. Does not involve any ion in solution and is used in hearing aids

Choose the correct answer from the options given below:

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

$\text{The hydrogen electrode is dipped in a solution of pH = 3 at } 25^{\circ}\text{C. The potential of the electrode will be } -\_\_\_\_\_ \times 10^{-2} \text{ V.}$
$\left( \frac{2.303RT}{F} = 0.059 \, \text{V} \right)$

The potential for the given half cell at 298 K is\[(-) \ldots \times 10^{-2} \, \text{V}.\]\[2\text{H}^+ (\text{aq}) + 2e^- \rightarrow \text{H}_2 (\text{g})\]\[[\text{H}^+] = 1M, \, P_{\text{H}_2} = 2 \, \text{atm}\](Given: \( 2.303 \frac{RT}{F} = 0.06 \, \text{V}, \log 2 = 0.3 \))

The mass of silver (Molar mass of Ag : 108 gmol^–1 ) displaced by a quantity of electricity which displaces 5600 mL of O₂ at S.T.P. will be _____ g.

The mass of zinc produced by the electrolysis of zinc sulfate solution with a steady current of 0.015 A for 15 minutes is _____ \( \times \, 10^{-4} \) g.
(Atomic mass of zinc = 65.4 amu)

$1 \times 10^{-5} M \,AgNO _3$ is added to $1\, L$ of saturated solution of $AgBr$ The conductivity of this solution at $298 \,K$ is ___ [Given : $K _{\text {SP }}( AgBr )=49 \times 10^{-13}$ at $298\, K$ $\lambda_{ Ag ^{+}}^0=6 \times 10^{-3} S\, m ^2\, mol ^{-1} $ $ \lambda_{ Br ^{-}}^0=8 \times 10^{-3} S\, m ^2\, mol ^{-1} $ $ \lambda_{ NO _3^{-}}^0=7 \times 10^{-3} \,S\, m ^2 \,mol ^{-1}$ ]

The resistivity of a $0.8 M$ solution of an electrolyte is $5 \times 10^{-3} \Omega cm$ Its molar conductivity is ____ $\times 10^4\, \Omega^{-1}\, cm ^2 \,mol ^{-1}$

At $298 \,K$, a 1 litre solution containing $10\, m\,mol$ of $Cr _2 O _7{ }^{2-}$ and $100\, m\,mol$ of $Cr ^{3+}$ shows a pH of 30.

Given: $Cr _2 O _7^{2-} \rightarrow Cr ^{3+} ; E ^{\circ}=1330 V$ and $\frac{2303 RT }{ F }=0059 V$.

The potential for the half cell reaction is $x \times 10^{-3} V$. The value of $x$ is ___ .

Select correct statements about lead storage battery:

For given cell, at T K
Pt | H₂(g) | H⁺ || Fe³⁺ ; Fe²⁺ | Pt
   ( 1 bar ) ( 1 M )
E_cell = .712 V
E^°_cell = .770 V
if \(\frac{[Fe^{2+}]}{[Fe^{3+}]}\) is t \((\frac{2.303\ RT}{F}=.058)\)
then find \((\frac{t}{5})\)

The number of correct statements from the following is ______
A. E^cell is an intensive parameter
B. A negative E^θ means that the redox couple is a stronger reducing agent than the H^– H₂ couple.
C. The amount of electricity required for oxidation or reduction depends on the stoichiometry of the electrode reaction.
D. The amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the quantity of electricity passed through the electrolyte.

The standard electrode potential \((\frac{M^{3+}}{M^{2+}})\) for V, Cr, Mn & Co are –0.26 V, –0.41 V, +1.57 V and +1.97 V, respectively. The metal ions which can liberate H₂ from a dilute acid are

\(Pt(s) | H_{2_{(g)}} (1 bar) | H^{+}_{(aq)}(1M) || M^{3+}_{(aq)}, M^{+}_{(aq)} | Pt(s)\)
The E_cell for the given cell is 0.1115 V at 298 K when \(\frac{[M^+(aq)}{[M^{3+}(aq)]}=10^{a}\)
The value of a is _________
Given: \(E^{\theta}_{M^{3+}/M^+}=0.2\;V\)
\(\frac{2.303RT}{F}=0.059V\)

How many of the following statements are correct:

The cell potential for \(\text{Zn}|\text{Zn}^{2+}\text{(aq)}||\text{Sn}^{x+}|\text{Sn}\) is 0.801 V at 298 K.The reaction quotient for the above reaction is 10^–2. The number of electrons involved in the given electrochemical cell reaction is _____. (Given: \(Eº_Zn^{2+}\)|Zn=-0.763V,Eºsn^x+|sn=+0.008V and 2.303RT/F=0.06V)