Skip to the question

JEE MainChemistry

Reviewed by Amrinder

+4 marks−1 if incorrectNumericalpyq

Redox Reactions and Electrochemistry: Chemistry | JEE Main

The number of correct statements from the following is : A.

\mathrm{E}_{\mathrm{cell}}

is an intensive parameter. B. A negative

\mathrm{E}^{\ominus}

means that the redox couple is a stronger reducing agent than the

\mathrm{H}^{+} / \mathrm{H}_2

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.

Your answer stays private

What feels right?

No score. Commit to your first instinct. We’ll show what your mind noticed and what it missed.

Type the value - units or words beside it are fine.

Step-by-step solutionView

Correct answer

All 4 statements (A, B, C, and D) are correct, so the answer is 4.

Option analysis

Why each option works or fails

Reviewed route

Solution

StepWorking

01given

Four statements related to electrochemistry: A. $\mathrm{E}_{\mathrm{cell}}$ is an intensive parameter. B. A negative $\mathrm{E}^{\ominus}$ means that the redox couple is a stronger reducing agent than the $\mathrm{H}^{+} / \mathrm{H}_2$ couple. C. The required electricity for oxidation or reduction depends on the stoichiometry of the electrode reaction. D. A chemical reaction occurs at an electrode during electrolysis. The amount of this reaction is proportional to the quantity of electricity passed through the electrolyte.

02strategise

Evaluate the thermodynamic and electrochemical validity of each statement (A through D) against standard NCERT definitions and Faraday's laws of electrolysis.

03execute

1. Statement A: $\mathrm{E}_{\mathrm{cell}} = -\Delta G / (nF)$ . Since $\Delta G$ and $n$ are both extensive, their ratio $\mathrm{E}_{\mathrm{cell}}$ does not depend on system size; it is an intensive parameter. (True) 2. Statement B: Standard reduction potential $E^{\ominus}(\mathrm{H}^+/\mathrm{H}_2) = 0.00\text{ V}$ . A negative standard reduction potential means the reduced form easily loses electrons relative to $\mathrm{H}_2$ , making the couple a stronger reducing agent than $\mathrm{H}^+/\mathrm{H}_2$ . (True) 3. Statement C: By Faraday's laws, $n$ moles of electrons ( $nF$ charge) are required per mole of product, which directly depends on the balanced stoichiometric half-reaction. (True) 4. Statement D: This is Faraday's first law of electrolysis: $m \propto Q$ , i.e., mass/extent of chemical reaction is directly proportional to the quantity of electricity passed. (True) Total number of correct statements = 1 + 1 + 1 + 1 = 4.

✓verify

All 4 statements are correct. They directly quote fundamental NCERT concepts. These include cell potential intensivity, standard reduction potential relative to SHE, stoichiometric electron requirement, and Faraday's first law.

✓ Source and academic review

Question type: Numerical
Exam relevance: JEE Main · Chemistry
Concepts assessed: Chemistry
Academic status: Reviewed by Amrinder
Source: pyq
Editorial review: 7 September 2026

Quick checks

Students also ask

Why is

E_{\mathrm{cell}}

intensive even though doubling the chemical equation doubles

\Delta G

?

Doubling the equation also doubles the number of transferred electrons ( $n$ ). Since $E_{\mathrm{cell}} = -\Delta G / (nF)$ , the factor of 2 cancels in the numerator and denominator, keeping $E_{\mathrm{cell}}$ unchanged.

Answer

All 4 statements (A, B, C, and D) are correct, so the answer is 4.

Why each option works or fails

Step-by-step solution

given: Four statements related to electrochemistry: A. $\mathrm{E}_{\mathrm{cell}}$ is an intensive parameter. B. A negative $\mathrm{E}^{\ominus}$ means that the redox couple is a stronger reducing agent than the $\mathrm{H}^{+} / \mathrm{H}_2$ couple. C. The required electricity for oxidation or reduction depends on the stoichiometry of the electrode reaction. D. A chemical reaction occurs at an electrode during electrolysis. The amount of this reaction is proportional to the quantity of electricity passed through the electrolyte.
strategise: Evaluate the thermodynamic and electrochemical validity of each statement (A through D) against standard NCERT definitions and Faraday's laws of electrolysis.
execute: 1. Statement A: $\mathrm{E}_{\mathrm{cell}} = -\Delta G / (nF)$ . Since $\Delta G$ and $n$ are both extensive, their ratio $\mathrm{E}_{\mathrm{cell}}$ does not depend on system size; it is an intensive parameter. (True) 2. Statement B: Standard reduction potential $E^{\ominus}(\mathrm{H}^+/\mathrm{H}_2) = 0.00\text{ V}$ . A negative standard reduction potential means the reduced form easily loses electrons relative to $\mathrm{H}_2$ , making the couple a stronger reducing agent than $\mathrm{H}^+/\mathrm{H}_2$ . (True) 3. Statement C: By Faraday's laws, $n$ moles of electrons ( $nF$ charge) are required per mole of product, which directly depends on the balanced stoichiometric half-reaction. (True) 4. Statement D: This is Faraday's first law of electrolysis: $m \propto Q$ , i.e., mass/extent of chemical reaction is directly proportional to the quantity of electricity passed. (True) Total number of correct statements = 1 + 1 + 1 + 1 = 4.
verify: All 4 statements are correct. They directly quote fundamental NCERT concepts. These include cell potential intensivity, standard reduction potential relative to SHE, stoichiometric electron requirement, and Faraday's first law.