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Electrochemistry: JEE Main Previous Year Questions (2021-2026)
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Page 1 JEE Main Previous Year Questions (2021-2026): Electrochemistry (January 2026) Q1: Consider the above electrochemical cell where a metal electrode ( M ) is undergoing redox reaction by forming M + (M ? M + + e - ). The cation M + is present in two different concentrations c 1 and c 2 as shown above. Which of the following statement is correct for generating a positive cell potential? A: If c1 is present at anode, then c1 > c2. B: If c1 is present at cathode, then c1 > c2. C: If c1 is present at cathode, then $c1 < c2. D: If c1 is present at anode, then c1 = c2. Answer: B Explanation: (1) If c 1 is at anode ? cell reaction Q2: In the given electrochemical cell, Ag(s) | AgCl(s) | FeCl2(aq), FeCl3(aq) | Pt(s) at 298 K, the cell potential (E cell ) will increase when: A. Concentration of Fe 2+ is increased. B. Concentration of Fe 3+ is decreased. C. Concentration of Fe 2+ is decreased. D. Concentration of Fe 3+ is increased. E. Concentration of Cl - is increased. Page 2 JEE Main Previous Year Questions (2021-2026): Electrochemistry (January 2026) Q1: Consider the above electrochemical cell where a metal electrode ( M ) is undergoing redox reaction by forming M + (M ? M + + e - ). The cation M + is present in two different concentrations c 1 and c 2 as shown above. Which of the following statement is correct for generating a positive cell potential? A: If c1 is present at anode, then c1 > c2. B: If c1 is present at cathode, then c1 > c2. C: If c1 is present at cathode, then $c1 < c2. D: If c1 is present at anode, then c1 = c2. Answer: B Explanation: (1) If c 1 is at anode ? cell reaction Q2: In the given electrochemical cell, Ag(s) | AgCl(s) | FeCl2(aq), FeCl3(aq) | Pt(s) at 298 K, the cell potential (E cell ) will increase when: A. Concentration of Fe 2+ is increased. B. Concentration of Fe 3+ is decreased. C. Concentration of Fe 2+ is decreased. D. Concentration of Fe 3+ is increased. E. Concentration of Cl - is increased. Choose the correct answer from the options given below : A: C, D and E Only B: A and B Only C: B Only D: A and E Only Answer: A Explanation: Q3: Consider the following reduction processes : Al³? + 3e? ? Al(s), E° = -1.66 V Fe³? + e? ? Fe²?, E° = +0.77 V Co³? + e? ? Co²?, E° = +1.81 V Cr³? + 3e? ? Cr(s), E° = -0.74 V The tendency to act as reducing agent decreases in the order : A: Al > Fe²? > Cr > Co²? B: Al > Cr > Co²? > Fe²? C: Cr > Fe²? > Al > Co²? D: Al > Cr > Fe²? > Co²? Answer: D Explanation: Reducing agent is the species that gets oxidised (donates electrons). In NCERT terms: More negative for a couple ? the reduced form is a stronger reducing agent (it will be more easily oxidised). Equivalently, higher ? stronger reducing agent. Page 3 JEE Main Previous Year Questions (2021-2026): Electrochemistry (January 2026) Q1: Consider the above electrochemical cell where a metal electrode ( M ) is undergoing redox reaction by forming M + (M ? M + + e - ). The cation M + is present in two different concentrations c 1 and c 2 as shown above. Which of the following statement is correct for generating a positive cell potential? A: If c1 is present at anode, then c1 > c2. B: If c1 is present at cathode, then c1 > c2. C: If c1 is present at cathode, then $c1 < c2. D: If c1 is present at anode, then c1 = c2. Answer: B Explanation: (1) If c 1 is at anode ? cell reaction Q2: In the given electrochemical cell, Ag(s) | AgCl(s) | FeCl2(aq), FeCl3(aq) | Pt(s) at 298 K, the cell potential (E cell ) will increase when: A. Concentration of Fe 2+ is increased. B. Concentration of Fe 3+ is decreased. C. Concentration of Fe 2+ is decreased. D. Concentration of Fe 3+ is increased. E. Concentration of Cl - is increased. Choose the correct answer from the options given below : A: C, D and E Only B: A and B Only C: B Only D: A and E Only Answer: A Explanation: Q3: Consider the following reduction processes : Al³? + 3e? ? Al(s), E° = -1.66 V Fe³? + e? ? Fe²?, E° = +0.77 V Co³? + e? ? Co²?, E° = +1.81 V Cr³? + 3e? ? Cr(s), E° = -0.74 V The tendency to act as reducing agent decreases in the order : A: Al > Fe²? > Cr > Co²? B: Al > Cr > Co²? > Fe²? C: Cr > Fe²? > Al > Co²? D: Al > Cr > Fe²? > Co²? Answer: D Explanation: Reducing agent is the species that gets oxidised (donates electrons). In NCERT terms: More negative for a couple ? the reduced form is a stronger reducing agent (it will be more easily oxidised). Equivalently, higher ? stronger reducing agent. Now write oxidation potentials for the given reducing species: Now arrange reducing strength (decreasing ): +1.66 > +0.74 > -0.77 > -1.81 So, tendency to act as reducing agent decreases as: Al > Cr > Fe 2+ > Co 2+ Correct option: D Q4: For a closed circuit Daniell cell, which of the following plots is the accurate one at a given temperature? A: Page 4 JEE Main Previous Year Questions (2021-2026): Electrochemistry (January 2026) Q1: Consider the above electrochemical cell where a metal electrode ( M ) is undergoing redox reaction by forming M + (M ? M + + e - ). The cation M + is present in two different concentrations c 1 and c 2 as shown above. Which of the following statement is correct for generating a positive cell potential? A: If c1 is present at anode, then c1 > c2. B: If c1 is present at cathode, then c1 > c2. C: If c1 is present at cathode, then $c1 < c2. D: If c1 is present at anode, then c1 = c2. Answer: B Explanation: (1) If c 1 is at anode ? cell reaction Q2: In the given electrochemical cell, Ag(s) | AgCl(s) | FeCl2(aq), FeCl3(aq) | Pt(s) at 298 K, the cell potential (E cell ) will increase when: A. Concentration of Fe 2+ is increased. B. Concentration of Fe 3+ is decreased. C. Concentration of Fe 2+ is decreased. D. Concentration of Fe 3+ is increased. E. Concentration of Cl - is increased. Choose the correct answer from the options given below : A: C, D and E Only B: A and B Only C: B Only D: A and E Only Answer: A Explanation: Q3: Consider the following reduction processes : Al³? + 3e? ? Al(s), E° = -1.66 V Fe³? + e? ? Fe²?, E° = +0.77 V Co³? + e? ? Co²?, E° = +1.81 V Cr³? + 3e? ? Cr(s), E° = -0.74 V The tendency to act as reducing agent decreases in the order : A: Al > Fe²? > Cr > Co²? B: Al > Cr > Co²? > Fe²? C: Cr > Fe²? > Al > Co²? D: Al > Cr > Fe²? > Co²? Answer: D Explanation: Reducing agent is the species that gets oxidised (donates electrons). In NCERT terms: More negative for a couple ? the reduced form is a stronger reducing agent (it will be more easily oxidised). Equivalently, higher ? stronger reducing agent. Now write oxidation potentials for the given reducing species: Now arrange reducing strength (decreasing ): +1.66 > +0.74 > -0.77 > -1.81 So, tendency to act as reducing agent decreases as: Al > Cr > Fe 2+ > Co 2+ Correct option: D Q4: For a closed circuit Daniell cell, which of the following plots is the accurate one at a given temperature? A: B: C: D: Answer: D Explanation: Standard cell potential does not change as time passes. Q5: A volume of x mL of 5 M NaHCO 3 solution was mixed with 10 mL of 2 M H 2 CO 3 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) 6 2- (0.5 M) | HSnO 2 - (0.05 M) | OH - | Bi 2 O 3 (s) | Bi(s) Consider up to one place of decimal for intermediate calculations Page 5 JEE Main Previous Year Questions (2021-2026): Electrochemistry (January 2026) Q1: Consider the above electrochemical cell where a metal electrode ( M ) is undergoing redox reaction by forming M + (M ? M + + e - ). The cation M + is present in two different concentrations c 1 and c 2 as shown above. Which of the following statement is correct for generating a positive cell potential? A: If c1 is present at anode, then c1 > c2. B: If c1 is present at cathode, then c1 > c2. C: If c1 is present at cathode, then $c1 < c2. D: If c1 is present at anode, then c1 = c2. Answer: B Explanation: (1) If c 1 is at anode ? cell reaction Q2: In the given electrochemical cell, Ag(s) | AgCl(s) | FeCl2(aq), FeCl3(aq) | Pt(s) at 298 K, the cell potential (E cell ) will increase when: A. Concentration of Fe 2+ is increased. B. Concentration of Fe 3+ is decreased. C. Concentration of Fe 2+ is decreased. D. Concentration of Fe 3+ is increased. E. Concentration of Cl - is increased. Choose the correct answer from the options given below : A: C, D and E Only B: A and B Only C: B Only D: A and E Only Answer: A Explanation: Q3: Consider the following reduction processes : Al³? + 3e? ? Al(s), E° = -1.66 V Fe³? + e? ? Fe²?, E° = +0.77 V Co³? + e? ? Co²?, E° = +1.81 V Cr³? + 3e? ? Cr(s), E° = -0.74 V The tendency to act as reducing agent decreases in the order : A: Al > Fe²? > Cr > Co²? B: Al > Cr > Co²? > Fe²? C: Cr > Fe²? > Al > Co²? D: Al > Cr > Fe²? > Co²? Answer: D Explanation: Reducing agent is the species that gets oxidised (donates electrons). In NCERT terms: More negative for a couple ? the reduced form is a stronger reducing agent (it will be more easily oxidised). Equivalently, higher ? stronger reducing agent. Now write oxidation potentials for the given reducing species: Now arrange reducing strength (decreasing ): +1.66 > +0.74 > -0.77 > -1.81 So, tendency to act as reducing agent decreases as: Al > Cr > Fe 2+ > Co 2+ Correct option: D Q4: For a closed circuit Daniell cell, which of the following plots is the accurate one at a given temperature? A: B: C: D: Answer: D Explanation: Standard cell potential does not change as time passes. Q5: A volume of x mL of 5 M NaHCO 3 solution was mixed with 10 mL of 2 M H 2 CO 3 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) 6 2- (0.5 M) | HSnO 2 - (0.05 M) | OH - | Bi 2 O 3 (s) | Bi(s) Consider up to one place of decimal for intermediate calculations Answer: 78 Explanation: For the half-cells (25 °C): (1) Sn(IV)/Sn(II) couple (given E ° = -0.90V) Balanced reduction in basic medium:Read More
FAQs on Electrochemistry: JEE Main Previous Year Questions (2021-2026)
| 1. What is electrochemistry? |  |
Ans. Electrochemistry is the branch of chemistry that deals with the relationship between electrical energy and chemical change. It involves the study of redox (reduction-oxidation) reactions where electrons are transferred between substances, leading to the generation of electricity or the use of electricity to drive chemical reactions.
| 2. What are the main types of electrochemical cells? | |
Ans. The main types of electrochemical cells are galvanic (or voltaic) cells and electrolytic cells. Galvanic cells convert chemical energy into electrical energy through spontaneous redox reactions, while electrolytic cells use electrical energy to drive non-spontaneous chemical reactions.
| 3. How does a galvanic cell operate? | |
Ans. A galvanic cell operates by separating two half-cells, each containing an electrode and an electrolyte. The oxidation reaction occurs at the anode, releasing electrons, while the reduction reaction occurs at the cathode, consuming electrons. This flow of electrons from the anode to the cathode generates an electric current, which can be harnessed for work.
| 4. What is the significance of the Nernst equation in electrochemistry? | |
Ans. The Nernst equation is significant in electrochemistry as it relates the cell potential to the concentrations of the reactants and products in a redox reaction. It allows for the calculation of the electromotive force (EMF) of a cell under non-standard conditions, providing insights into the spontaneity and feasibility of electrochemical reactions.
| 5. What role do electrolytes play in electrochemical cells? | |
Ans. Electrolytes play a crucial role in electrochemical cells by facilitating the movement of ions between the electrodes. They are solutions that conduct electricity due to the presence of free ions, allowing for charge balance and maintaining the flow of current as oxidation and reduction reactions occur at the electrodes.
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