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JEE Main Unit 9B2: Cell EMF and Electrolytic Applications — practice questions

Explore 12 free Unit 9B2: Cell EMF and Electrolytic Applications questions in JEE Main Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Unit 9B2: Cell EMF and Electrolytic Applications questions and exercises with answers

Showing questions 1–12 of 12.

The standard EMF of a Zn|Zn²⁺||Cu²⁺|Cu cell (E°_Cu²⁺/Cu = +0.34 V; E°_Zn²⁺/Zn = −0.76 V) isRead the answer and worked solution →For the reaction Cu²⁺ + 2e⁻ → Cu with E° = +0.34 V, what is the cell potential when [Cu²⁺] = 0.01 M at 298 K?Read the answer and worked solution →One Faraday equals the charge onRead the answer and worked solution →The mass of copper deposited when a current of 5.0 A flows for 30 minutes through a solution of CuSO₄ (M_Cu = 63.5 g/mol, F = 96500 C) is approximatelyRead the answer and worked solution →For a Cu-Zn Daniell cell, the emf is measured to be 1.10 V under standard conditions. If [Cu²⁺] = 1 M and [Zn²⁺] = 0.01 M at 298 K, the cell EMF becomesRead the answer and worked solution →Molar conductivity of a strong electrolyte at concentration c is related to its limiting value Λ°_m by the Debye-Hückel-Onsager equationRead the answer and worked solution →The specific conductivity of a 0.1 M KCl solution is 1.29 × 10⁻² S/cm. The molar conductivity isRead the answer and worked solution →Fuel cells directly convertRead the answer and worked solution →Rusting of iron requires which two chemicals in contact with the metal?Read the answer and worked solution →The primary cell that cannot be reused after its EMF drops to zero is exemplified byRead the answer and worked solution →The overall cell reaction of the lead storage battery on discharge isRead the answer and worked solution →For an electrochemical cell operating spontaneously, ΔG° is related to E°_cell byRead the answer and worked solution →

Worked practice questions

The standard EMF of a Zn|Zn²⁺||Cu²⁺|Cu cell (E°_Cu²⁺/Cu = +0.34 V; E°_Zn²⁺/Zn = −0.76 V) is

  1. +1.10 V
  2. +0.42 V
  3. −1.10 V
  4. −0.42 V
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Correct answer: A. +1.10 V

1. Daniell cell: Zn (anode, oxidation), Cu (cathode, reduction). 2. E°_cell = E°_cathode − E°_anode = 0.34 − (−0.76) V. 3. E°_cell = 0.34 + 0.76 = +1.10 V. 4. Positive value means the reaction is spontaneous as written. _Source: syllabus Chemistry, Unit 3 "Electrochemistry", §3.2_

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For the reaction Cu²⁺ + 2e⁻ → Cu with E° = +0.34 V, what is the cell potential when [Cu²⁺] = 0.01 M at 298 K?

  1. +0.34 V
  2. +0.399 V
  3. +0.281 V
  4. +0.281 V (using log 100)
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Correct answer: C. +0.281 V

1. E = E° − (0.059/n) log (1/[Cu²⁺]) = E° + (0.059/n) log [Cu²⁺]. 2. n = 2. Substitute: E = 0.34 + (0.059/2) × log(0.01). 3. log(0.01) = −2. Term = (0.059/2) × (−2) = −0.059. 4. E = 0.34 − 0.059 = +0.281 V. _Source: syllabus Chemistry, Unit 3 "Electrochemistry", §3.3_

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One Faraday equals the charge on

  1. One gram of silver
  2. One coulomb
  3. One mole of hydrogen atoms
  4. One mole of electrons
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Correct answer: D. One mole of electrons

1. 1 F is the charge carried by 1 mole of electrons. 2. Numerically, 1 F ≈ 96500 C mol⁻¹. 3. This connects electrical (charge) and chemical (moles) quantities. 4. It appears throughout electrolysis, Nernst equation and battery calculations. _Source: syllabus Chemistry, Unit 3 "Electrochemistry", §3.4_

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