NEET Chemistry: Electrochemistry — MCQ Test 1

Q6. The emf of a cell \( Ni(s) | Ni^{2+}(0.001 \, M) || Ag^+(0.002 \, M) | Ag(s) \) at 298 K is (Given: \( E^\circ_{Ni^{2+}/Ni} = -0.25 \, V \), \( E^\circ_{Ag^+/Ag} = 0.80 \, V \))?

Q7. What is the emf of a cell with the reaction \( Mg(s) + 2Ag^+(aq) \rightarrow Mg^{2+}(aq) + 2Ag(s) \) at standard conditions, given \( E^\circ_{Mg^{2+}/Mg} = -2.36 \, V \) and \( E^\circ_{Ag^+/Ag} = 0.80 \, V \)?

Q8. The conductivity of a 0.025 M NaNO\(_3\) solution is 0.003 S cm\(^{-1}\), and its molar conductivity is 120 S cm\(^2\) mol\(^{-1}\). What is the degree of dissociation if \( \Lambda_m^\circ = 126.5 \, S \, cm^2 \, mol^{-1} \)?

Q9. The conductivity of a 0.01 M solution is 0.00141 S cm\(^{-1}\). What is its molar conductivity?

Q10. A current of 1 A deposits 0.635 g of Cu from CuSO\(_4\) in 1930 s. What is the time required to deposit 0.54 g of Al from Al\(_2\)(SO\(_4\))\(_3\) with the same current? (Atomic masses: Cu = 63.5 g/mol, Al = 27 g/mol, F = 96500 C/mol)

NEET Chemistry — Electrochemistry

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A current of 0.5 A is passed through a CuSO\(_4\) solution for 9650 s, and then the same current is passed through an AlCl\(_3\) solution for 6433.33 s. What is the total mass of metal deposited? (Atomic masses: Cu = 63.5 g/mol, Al = 27 g/mol, F = 96500 C/mol)

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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 Solution, Deposited, Limiting, Conductivity, Required, and Infinite.

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Preview of Questions in this Test

Q1. A current of 0.5 A is passed through a CuSO\(_4\) solution for 9650 s, and then the same current is passed through an AlCl\(_3\) solution for 6433.33 s. What is the total mass of metal deposited? (Atomic masses: Cu = 63.5 g/mol, Al = 27 g/mol, F = 96500 C/mol)

  • A. 1.8875 g
  • B. 1.5875 g
  • C. 2.1875 g
  • D. 1.2875 g

Q2. The limiting molar conductivity of CaCl\(_2\) is 258 S cm\(^2\) mol\(^{-1}\). If \( \lambda^\circ_{Ca^{2+}} = 119 \, S \, cm^2 \, mol^{-1} \), what is \( \lambda^\circ_{Cl^-} \)?

  • A. 69.5 S cm\(^2\) mol\(^{-1}\)
  • B. 119 S cm\(^2\) mol\(^{-1}\)
  • C. 139 S cm\(^2\) mol\(^{-1}\)
  • D. 258 S cm\(^2\) mol\(^{-1}\)

Q3. What is the time (in seconds) required to deposit 0.405 g of calcium from molten CaCl\(_2\) using a current of 1.5 A? (Atomic mass of Ca = 40.5 g/mol, F = 96500 C/mol)

  • A. 1286.67 s
  • B. 965 s
  • C. 1930 s
  • D. 2573.33 s

Q4. The molar conductivity of LiCl at infinite dilution is 115.0 S cm\(^2\) mol\(^{-1}\). If \( \lambda^\circ_{Li^+} = 38.7 \, S \, cm^2 \, mol^{-1} \), what is \( \lambda^\circ_{Cl^-} \)?

  • A. 76.3 S cm\(^2\) mol\(^{-1}\)
  • B. 38.7 S cm\(^2\) mol\(^{-1}\)
  • C. 115.0 S cm\(^2\) mol\(^{-1}\)
  • D. 19.3 S cm\(^2\) mol\(^{-1}\)

Q5. A cell \( Zn(s) | Zn^{2+}(0.001 \, M) || Br_2(l) | Br^-(0.002 \, M) | Pt(s) \) operates at 298 K. What is the cell potential? (Given: \( E^\circ_{Zn^{2+}/Zn} = -0.76 \, V \), \( E^\circ_{Br_2/Br^-} = 1.07 \, V \))

  • A. 1.83 V
  • B. 1.682 V
  • C. 2.10 V
  • D. 1.978 V

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