Electrochemistry JEE Main PYQs PDF, 2020–2026

Electrochemistry questions per year

in the free PDF asked, not in the PDFThe PDF only has questions we can print in full with a checked answer, so it holds 165 of the 167 asked.

Topic-wise weightage by year

How many Electrochemistry questions each topic had in every JEE Main year (all shifts), counting every question asked, including ones not in the PDF. Darker cells mean more questions.

Swipe the table sideways for older years.

Newest questions (2026)

The 12 newest of the 21 JEE Main 2026 Electrochemistry questions in the free PDF, latest shift first.

1. JEE Main 2026 · 8 Apr · Shift 2 · Electrochemical Cells

   Given at 298 K :

   $\begin{array}{cc} & {\mathrm{E}}_{{{\mathrm{Fe}}^{{2+}}/{\mathrm{Fe}}}}^{{\ominus}}={\mathrm{X}}\text{ Volt} \\ & {\mathrm{E}}_{{{\mathrm{Fe}}^{{3+}}/{\mathrm{Fe}}}}^{{\ominus}}={\mathrm{Y}}\text{ Volt}\end{array}$

   The ${\mathrm{E}}_{{{\mathrm{Fe}}^{{3+}}/{\mathrm{Fe}}^{{2+}}}}^{{\ominus}}$ in Volt at 298 K is given by :

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2. JEE Main 2026 · 6 Apr · Shift 1 · Kohlrausch's Law

   $\text{ Consider the following data.}$

   $\begin{array}{cc}\text{ Electrolyte} & \wedge_{{\mathbf{m}}}^{{\circ}}{{(}}{\mathbf{S}\ \mathbf{c}\mathbf{m}}^{{{\mathbf{2}}}}{\ \mathbf{m}\mathbf{o}\mathbf{l}}^{{{\mathbf{1}}}}{)} \\ {\mathrm{BaCl}}_{2} & x_{1} \\ {\mathrm{H}}_{2}{\mathrm{SO}}_{4} & x_{2} \\ {\mathrm{HCl}} & x_{3}\end{array}$

   ${\mathrm{BaSO}}_{4}$ is sparingly soluble in water. If the conductivity of the saturated ${\mathrm{BaSO}}_{4}$ solution is $x{\ \mathrm{S}}{\ \mathrm{cm}}^{{-1}}$ then the solubility product of ${\mathrm{BaSO}}_{4}$ can be given as (Here $\wedge_{{{\mathrm{m}}}}=\wedge_{{{\mathrm{m}}}}^{{\circ}}$ )

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3. JEE Main 2026 · 6 Apr · Shift 2 · Electrochemical Cells

   For a general redox reaction

   Anode $\;\mathrm{Red}_{1}\rightarrow {\mathrm{Ox}}_{1}^{{{\mathrm{n}}_{1}^{{+}}}}+{\mathrm{n}}_{1}{\mathrm{e}}^{{-}}$

   Cathode ${\mathrm{O}}x_{2}+{\mathrm{n}}_{2}{\mathrm{e}}^{{-}}\rightarrow \mathrm{Red}_{2}^{{{\mathrm{n}}_{2}-}}$

   Which of the following statement is incorrect?

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4. JEE Main 2026 · 5 Apr · Shift 2 · Electrochemical Cells

   One half cell in a voltaic cell is constructed by dipping silver rod in ${\mathrm{AgNO}}_{3}$ solution of unknown concentration, other half cell is Zn rod dipped in 1 molar solution of ${\mathrm{ZnSO}}_{4}$.

   A voltage of 1.60 V is measured at 298 K for this cell. What is the concentration of ${\mathrm{Ag}}^{{+}}$ions used in terms of $\log x\left(x=\left[{\mathrm{Ag}}^{{+}}\right]\right)$?

   ${\mathrm{E}}_{{{\mathrm{Zn}}^{{2+}}/{\mathrm{Zn}}}}^{{\ominus}}=-0.76{\ \mathrm{V}},\;{\mathrm{E}}_{{{\mathrm{Ag}}^{{+}}/{\mathrm{Ag}}}}^{{\ominus}}=+0.80{\ \mathrm{V}},\frac{2.303{\mathrm{RT}}}{{\ \mathrm{F}}}=0.059{\ \mathrm{V}}$

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5. JEE Main 2026 · 5 Apr · Shift 2 · Conductance and Conductivity

   At 298 K , the molar conductivity of $x\%({\mathrm{w}}/{\mathrm{w}}){\mathrm{MX}}$ solution (aqueous) is $123.5{\ \mathrm{S}}{\ \mathrm{cm}}^{2}{\ \mathrm{mol}}^{{-1}}$. The conductance of same solution is $1.9\times {10}^{{-3}}{\ \mathrm{S}}$. The value of $x$ is $\_\_\_\_$ $\times {10}^{{-2}}$.

   (Given: cell constant $=1.3{\ \mathrm{cm}}^{{-1}}$; molar mass of MX is $75{\ \mathrm{g}}{\ \mathrm{mol}}^{{-1}}$, density of aqueous solution of MX at 298 K is $1.0{\ \mathrm{g}}{\ \mathrm{mL}}^{{-1}}$ )

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6. JEE Main 2026 · 4 Apr · Shift 2 · Electrochemical Cells

   An electrochemical cell, consist of the following two redox couples, ${\mathrm{M}}^{{x+}}({\mathrm{aq}})/{\mathrm{M}}({\mathrm{s}})\left[{\mathrm{E}}_{{\text{red}}}^{{\Theta}}=+0.15{\ \mathrm{V}}\right]$ and ${\mathrm{Fe}}^{{3+}}({\mathrm{aq}})/{\mathrm{Fe}}({\mathrm{s}})\left[{\mathrm{E}}_{{\text{red}}}^{{\Theta}}=-0.036{\ \mathrm{V}}\right]$. The cell EMF $\left({\mathrm{E}}_{{\text{cell}}}\right)$ is recorded to be 0.2057 V . If the reaction quotient of the electrochemical reaction is found to be ${10}^{{-2}}$, then the value of $x$ is

   $\_\_\_\_$ .(Nearest integer)

   [Given : M is a p-block metal and $\frac{2.303RT}{F}=0.059{\ \mathrm{V}}$ ]

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7. JEE Main 2026 · 2 Apr · Shift 1 · Electrochemical Cells

   An electrochemical cell is constructed using half cells in the direction of spontaneous change:

   Fe(OH)₂(s) + 2e⁻ → Fe(s) + 2OH⁻(aq)      E^θ = −0.88 V

   and AgBr(s) + e⁻ → Ag(s) + Br⁻(aq)      E^θ = +0.07 V

   Which of the following option is correct?

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8. JEE Main 2026 · 2 Apr · Shift 2 · Batteries and Fuel Cells

   Consider the following two half-cell reactions along with the standard reduction potential given :

   ${\mathrm{CO}}_{2}+6{\mathrm{H}}^{+}+6e^{-}\longrightarrow {\mathrm{CH}}_{3}{\mathrm{OH}}+{\mathrm{H}}_{2}{\mathrm{O}}\;E_{{\text{red}}}^{{\circ}}=0.02\ {\mathrm{V}}$

   $\frac{1}{2}{\mathrm{O}}_{2}+2{\mathrm{H}}^{+}+2e^{-}\longrightarrow {\mathrm{H}}_{2}{\mathrm{O}}\;E_{{\text{red}}}^{{\circ}}=1.23\ {\mathrm{V}}$

   A fuel cell was set up using the above two reactions such that the cell operates under the standard condition of 1 bar pressure and 298 K temperature. The fuel cell works with 80% efficiency. If the work derived from the cell using 1 mol of ${\mathrm{CH}}_{3}{\mathrm{OH}}$ is used to compress an ideal gas isothermally against a constant pressure of 1 kPa, then the change in the volume of the gas,

   $\Delta V=\underline{\;}$ m${}^{3}$. (nearest integer)

   Given : ${\mathrm{F}}=96500\ {\mathrm{C}\ \mathrm{mol}}^{{-1}}$

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9. JEE Main 2026 · 28 Jan · Shift 2 · Electrochemical Cells

   A volume of x mL of 5 M NaHCO₃ solution was mixed with 10 mL of 2 M H₂CO₃ solution to make an electrolytic buffer. If the same buffer was used in the following electrochemical cell to record a cell potential of 235.3 mV, then the value of x = ______ mL (nearest integer).

   Sn(s) | Sn(OH)₆²⁻ (0.5 M) | HSnO₂⁻ (0.05 M) | OH⁻ | Bi₂O₃(s) | Bi(s)

   Consider up to one place of decimal for intermediate calculations

   
   $\left[\begin{array}{cc}\text{ Given:} & E_{{Sn{({OH})}_{6}^{{2-}}|HSnO_{2}^{-}}}^{o}=-0.9V \\ & {\mathrm{E}}^{{{\mathrm{o}}}}{}_{{{\mathrm{Bi}}_{2}{\mathrm{O}}_{3}\mid {\mathrm{Bi}}}}=-0.44{\ \mathrm{V}} \\ & {\mathrm{pKa}}_{{({\mathrm{H}}_{2}{\mathrm{CO}}_{3})}}=6.11 \\ & \frac{2.303{\mathrm{RT}}}{{\mathrm{F}}}=0.059{\ \mathrm{V}} \\ & \text{ Antilog}(1.29)=19.5\end{array}\right]$
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10. JEE Main 2026 · 28 Jan · Shift 1 · Electrochemical Cells

    Consider the following redox reaction taking place in acidic medium

    ${\mathrm{BH}}_{4}^{{-}}(aq)+{\mathrm{ClO}}_{3}^{{-}}(aq)\longrightarrow {\mathrm{H}}_{2}{\mathrm{BO}}_{3}^{{-}}(aq)+{\mathrm{Cl}}^{{-}}(aq)$

    If the Nernst equation for the above balanced reaction is

    ${\mathrm{E}}_{{{\mathrm{cell}}}}={\mathrm{E}}_{{{\mathrm{cell}}}}^{{\circ}}-\frac{{\mathrm{RT}}}{{\mathrm{nF}}}\ln {\mathrm{Q}},$

    then the value of $n$ is $\_\_\_\_$ .(Nearest integer)

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11. JEE Main 2026 · 28 Jan · Shift 2 · Kohlrausch's Law

    For strong electrolyte $\Lambda_{m}$ increases slowly with dilution and can be represented by the equation

    $\Lambda_{m}=\Lambda_{m}^{\circ}-Ac^{{1/2}}$

    Molar conductivity values of the solutions of strong electrolyte AB at 18°C are given below :

    c [mol L-1]	0.04	0.09	0.16	0.25
    $\Lambda_{m}$ [S cm2 mol-1]	96.1	95.7	95.3	94.9

    The value of constant A based on the above data [in S cm² mol^-1/(mol/L)^1/2] unit is ________.

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12. JEE Main 2026 · 24 Jan · Shift 1 · Electrolysis and Faraday's Laws

    Electricity is passed through an acidic solution of ${\mathrm{Cu}}^{{2+}}$ till all the ${\mathrm{Cu}}^{{2+}}$ was exhausted, leading to the deposition of 300 mg of Cu metal. However, a current of 600 mA was continued to pass through the same solution for another 28 minutes by keeping the total volume of the solution fixed at 200 mL . The total volume of oxygen evolved at STP during the entire process is $\_\_\_\_$ mL . (Nearest integer)

    [Given:

    $\begin{array}{cc} & {\mathrm{Cu}}^{{2+}}({\mathrm{aq}})+2{\mathrm{e}}^{{-}}\rightarrow {\mathrm{Cu}}({\ \mathrm{s}}){\mathrm{E}}_{{{\mathrm{red}}}}^{{{\mathrm{o}}}}=+0.34{\ \mathrm{V}} \\ & {\mathrm{O}}_{2}({\ \mathrm{g}})+4{\mathrm{H}}^{{+}}+4{\mathrm{e}}^{{-}}\rightarrow 2{\mathrm{H}}_{2}{\mathrm{O}}{\mathrm{E}}_{{{\mathrm{red}}}}^{{{\mathrm{o}}}}=+1.23{\ \mathrm{V}}\end{array}$

    Molar mass of ${\mathrm{Cu}}=63.54{\ \mathrm{g}}{\ \mathrm{mol}}^{{-1}}$

    Molar mass of ${\mathrm{O}}_{2}=32{\ \mathrm{g}}{\ \mathrm{mol}}^{{-1}}$

    Faraday Constant $=96500{\mathrm{C}}{\mathrm{mol}}^{{-1}}$

    Molar volume at ${\mathrm{STP}}=22.4{\ \mathrm{L}}$ ]

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