Electrochemistry Class 12 MCQ

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    Electrochemistry Class 12 MCQ. We covered all the Electrochemistry Class 12 MCQ in this post for free so that you can practice well for the exam.

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    MCQ on Electrochemistry for NEET Students

    The standard reduction potentials of metal ions X, Y, and Z are -0.52 V, -3.03 V, and -1.18 V respectively. Arrange the corresponding metals in the order of increasing reducing strength.

    (A) Y > Z > X

    (B) X > Y > Z

    (C) Z > Y > X

    (D) Z > X > Y

    Option a – Y > Z > X

    A solution of copper sulfate is electrolyzed with 5 faradays of electricity. What is the mass of copper collected at the cathode? (Atomic mass of Cu = 63.5)

    (A) 63.5 g

    (B) 95.25 g

    (C) 158.75 g

    (D) 317.5 g

    Option c – 158.75 g

    Choose the statement that is NOT correct.

    (A) Gaining electrons is defined as reduction.

    (B) A redox reaction involves electron transfer between species.

    (C) One Faraday equals the electric charge carried by one mole of electrons.

    (D) In electronic conductors, the flow of electricity involves transfer of matter.

    Option d – In electronic conductors, the flow of electricity involves transfer of matter.

    Which of the following elements is the most electropositive based on standard reduction potentials?

    (A) Ag (E° = +0.80 V)

    (B) Al (E° = -1.66 V)

    (C) Mg (E° = -2.37 V)

    (D) Ca (E° = -2.87 V)

    Option d – Ca (E° = -2.87 V)

    Consider the following two statements: Statement 1: Molar conductivity increases when electrolyte concentration decreases. Statement 2: Conductivity decreases as the concentration of an electrolyte decreases.
    Choose the correct option.

    (A) Only Statement 1 is true.

    (B) Only Statement 2 is true.

    (C) Both statements are false.

    (D) Both statements are true.

    Option d – Both statements are true.

    What are the products formed at the cathode and anode respectively during electrolysis of aqueous silver nitrate using platinum electrodes?

    (A) Ag(s), O₂(g)

    (B) Ag(s), NO₂(g)

    (C) H₂(g), Ag(s)

    (D) Ag(s), H₂(g)

    Option a – Ag(s), O₂(g)

    How long will it take to generate 0.10 mol of chlorine gas during electrolysis of molten NaCl using a 5-ampere current?

    (A) 0.50 hours

    (B) 0.85 hours

    (C) 1.07 hours

    (D) 6.43 hours

    Option c – 1.07 hours

    Which of the following statements best explains the concept of standard reduction potential?

    (A) A negative value indicates that the half-cell reaction tends to proceed in reverse.

    (B) Reversing a half-reaction changes the numerical value of its E°.

    (C) The sign of E° remains unchanged even if the half-reaction is reversed.

    (D) Doubling a half-reaction doubles its standard potential value.

    Option a – A negative value indicates that the half-cell reaction tends to proceed in reverse.

    During the electrolysis of water, 1.008 g of hydrogen gas is collected at the cathode. How much oxygen gas is released at the anode?

    (A) 32 g

    (B) 16 g

    (C) 8 g

    (D) 4 g

    Option c – 8 g

    Identify the INCORRECT statement about cathodic protection using magnesium for iron pipes.

    (A) Magnesium serves as the anode while iron becomes the cathode.

    (B) The entire iron pipe must be coated with magnesium to prevent rusting.

    (C) Moist soil works as an electrolyte in the protection setup.

    (D) Magnesium corrodes more easily than iron, offering protection to the pipe.

    Option b – The entire iron pipe must be coated with magnesium to prevent rusting.

    Which of the following statements about electrochemical cells is incorrect?

    (A) In dry cells, zinc acts as the anode and graphite as the cathode.

    (B) The lead storage battery operates as a galvanic cell during charging.

    (C) Alkaline dry cells use a basic electrolyte like NaOH or KOH.

    (D) Nickel-cadmium cells have a longer operational life than lead-acid batteries.

    Option b – The lead storage battery operates as a galvanic cell during charging.

    When 100 mL of 1 M solutions of NiSO₄, CrCl₃, and ZnSO₄ are completely electrolyzed, what is the ratio of electricity required?

    (A) 2 : 3 : 2

    (B) 2 : 3 : 1

    (C) 2 : 1 : 2

    (D) 1 : 3 : 1

    Option a – 2 : 3 : 2

    Assertion: Copper sulfate solution cannot be stored in a zinc container. Reason: Zinc is more reactive than copper. Choose the correct option.

    (A) Both Assertion and Reason are true, and Reason correctly explains the Assertion.

    (B) Both Assertion and Reason are true, but Reason does not explain the Assertion.

    (C) Assertion is true, but Reason is false.

    (D) Assertion is false, but Reason is true.

    Option a – Both Assertion and Reason are true, and Reason correctly explains the Assertion.

    What is the electrode potential of a hydrogen electrode in a solution with pH 10 and H₂ gas at 1 bar?

    (A) 0.4 V

    (B) -0.4 V

    (C) -0.59 V

    (D) 0.59 V

    Option c – -0.59 V

    One mole of aluminum is deposited by passing ‘Y’ coulombs through an aluminum nitrate solution. How many moles of silver will be deposited by the same quantity of charge from a silver nitrate solution?

    (A) 1

    (B) 2

    (C) 3

    (D) 4

    Option c – 3

    We covered all the electrochemistry class 12 MCQ above in this post for free so that you can practice well for the exam.

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