NEET Chemistry: Electrochemistry — MCQ Test 13

Q6. A current of 0.5 A deposits 0.3175 g of Cu from CuSO\(_4\) in 3860 s. What mass of Mg would be deposited from MgCl\(_2\) with the same charge? (Atomic masses: Cu = 63.5 g/mol, Mg = 24 g/mol, F = 96500 C/mol)

Q7. In a fuel cell operating at 298 K, the cell potential decreases from 1.23 V to 1.17 V when the \( [H^+] \) at the cathode increases from 0.1 M to 1 M. What is the number of electrons involved in the cathode reaction?

Q8. What is the emf of a cell \( Ni(s) | Ni^{2+}(0.1 \, M) || Cu^{2+}(0.001 \, M) | Cu(s) \) at 298 K? (Given: \( E^\circ_{Ni^{2+}/Ni} = -0.25 \, V \), \( E^\circ_{Cu^{2+}/Cu} = 0.34 \, V \))

Q9. What is the standard emf of a cell with the reaction \( 2Al(s) + 3Cd^{2+}(aq) \rightarrow 2Al^{3+}(aq) + 3Cd(s) \)? (Given: \( E^\circ_{Al^{3+}/Al} = -1.66 \, V \), \( E^\circ_{Cd^{2+}/Cd} = -0.40 \, V \))

Q10. The limiting molar conductivity of CsCl is 153.3 S cm\(^2\) mol\(^{-1}\). If \( \lambda^\circ_{Cs^+} = 77.0 \, S \, cm^2 \, mol^{-1} \), what is \( \lambda^\circ_{Cl^-} \)?

NEET Chemistry — Electrochemistry

Free MCQ Test 13 of 20

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1Question 1 of 10
Medium

The molar conductivity of a 0.005 M solution is 80 S cm2^2 mol−1^{-1}. What is the conductivity of the solution?

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About this NEET MCQ Test

This page provides a free online MCQ test for NEET Chemistry preparation, focusing specifically on the chapter Electrochemistry. It contains 10 carefully selected multiple-choice questions (MCQs) designed to test your conceptual understanding and exam readiness.

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Key concepts covered in this specific test include Conductivity, Solution, Standard, Reaction, Rightarrow, and Coulombs.

Taking these timed MCQ tests helps you simulate the real NEET exam environment. Detailed step-by-step explanations are provided for every question to help you learn from your mistakes and strengthen your fundamentals.

Preview of Questions in this Test

Q1.

The molar conductivity of a 0.005 M solution is 80 S cm2^2 mol−1^{-1}. What is the conductivity of the solution?

  • A.

    0.08 S cm−1^{-1}

  • B.

    0.004 S cm−1^{-1}

  • C.

    0.0004 S cm−1^{-1}

  • D.

    0.0008 S cm−1^{-1}

Q2.

What is the emf of the cell $ Mn(s)

Mn^{2+}(0.005 , M)
Hg^{2+}(0.02 , M)

Hg(l) at298K?(Given:at 298 K? (Given: E^\circ_{Mn^{2+}/Mn} = -1.18 , V ,, E^\circ_{Hg^{2+}/Hg} = 0.85 , V $)

  • A.

    2.03 V

  • B.

    2.05065 V

  • C.

    2.00935 V

  • D.

    2.10 V

Q3.

What is the standard emf of a cell with the reaction Cr(s)+3Ag+(aq)→Cr3+(aq)+3Ag(s)Cr(s) + 3Ag^+(aq) \rightarrow Cr^{3+}(aq) + 3Ag(s)? (Given: ECr3+/Cr∘=−0.74 VE^\circ_{Cr^{3+}/Cr} = -0.74 \, V, EAg+/Ag∘=0.80 VE^\circ_{Ag^+/Ag} = 0.80 \, V)

  • A.

    1.54 V

  • B.

    0.06 V

  • C.

    2.28 V

  • D.

    -1.54 V

Q4.

How many coulombs are required to deposit 108 g of silver from an AgNO3_3 solution? (Atomic mass of Ag = 108 g/mol, F = 96500 C/mol)

  • A.

    96500 C

  • B.

    193000 C

  • C.

    48250 C

  • D.

    289500 C

Q5.

A conductivity cell with cell constant 0.5 cm−1^{-1} shows a resistance of 200 \Omega with a 0.02 M KCl solution. What is the molar conductivity of the solution?

  • A.

    62.5 S cm2^2 mol−1^{-1}

  • B.

    250 S cm2^2 mol−1^{-1}

  • C.

    125 S cm2^2 mol−1^{-1}

  • D.

    50 S cm2^2 mol−1^{-1}

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