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Indian Navy Pilot Electrochemistry — practice questions

Explore 33 free Electrochemistry questions in Indian Navy Pilot Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Electrochemistry questions and exercises with answers

Showing questions 1–30 of 33.

The Nernst equation gives cell EMF at non-standard conditions. For a half-cell Mⁿ⁺ + ne⁻ → M, it is:Read the answer and worked solution →Relation between standard cell potential E°, ΔG°, and equilibrium constant K:Read the answer and worked solution →Equilibrium constant K of the Daniell cell at 25°C (E° = 1.10 V, n = 2):Read the answer and worked solution →Electrochemistry deals with:Read the answer and worked solution →How many coulombs are needed to deposit 1 mole of Cu from CuSO₄ (Cu²⁺ + 2e⁻ → Cu)?Read the answer and worked solution →Time to deposit 1.27 g of Cu from CuSO₄ solution at 2 A current (Cu atomic mass = 63.5):Read the answer and worked solution →Lead acid battery (used in cars) overall reaction:Read the answer and worked solution →The Daniell cell (Zn-Cu) has E°cell = +1.10 V. Calculate ΔG° (F = 96500 C/mol):Read the answer and worked solution →Galvanic cell or electrolytic cell?Read the answer and worked solution →Complete the standard cell potential relationRead the answer and worked solution →Order these electrodes by standard potential, lowest firstRead the answer and worked solution →Match each electrode to the potential your syllabus givesRead the answer and worked solution →True or false: conductivity on dilutionRead the answer and worked solution →Strong electrolyte or weak electrolyte?Read the answer and worked solution →Kohlrausch's lawRead the answer and worked solution →Match each relation to what it linksRead the answer and worked solution →True or false: cells and electrodesRead the answer and worked solution →Tap every statement true of a galvanic cellRead the answer and worked solution →Assertion and reasonRead the answer and worked solution →Two are true, one is notRead the answer and worked solution →Three of these are wrong. Find the one that holds.Read the answer and worked solution →Complete the thermodynamic linksRead the answer and worked solution →What the Nernst equation is forRead the answer and worked solution →Which quantity is being described?Read the answer and worked solution →True or false: batteries, fuel cells and corrosionRead the answer and worked solution →Order the steps: find a standard cell potentialRead the answer and worked solution →Flip and pair: symbol with meaningRead the answer and worked solution →Spot the one that does not belongRead the answer and worked solution →Tap every factor conductivity depends onRead the answer and worked solution →Assertion and reason: potentialsRead the answer and worked solution →

Worked practice questions

The Nernst equation gives cell EMF at non-standard conditions. For a half-cell Mⁿ⁺ + ne⁻ → M, it is:

  1. E = E°/n
  2. E = E° - (RT/nF) ln Q
  3. E = E° + (RT/nF) ln Q
  4. E = E° (no correction)
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Correct answer: B. E = E° - (RT/nF) ln Q

**Nernst equation:** E = E° - (RT/nF) ln Q where Q is reaction quotient. At 25°C: E = E° - (0.0591/n) log Q (with log base 10).

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Relation between standard cell potential E°, ΔG°, and equilibrium constant K:

  1. ΔG° = E°/n
  2. ΔG° = -RT/F
  3. ΔG° = -nFE° = -RT ln K
  4. ΔG° = nFE° = RT ln K
Show answer and solution

Correct answer: C. ΔG° = -nFE° = -RT ln K

ΔG° = -nFE° (relates ΔG° to electrochemistry) and ΔG° = -RT ln K (relates to thermodynamic equilibrium). **So nFE° = RT ln K. Useful for predicting spontaneity and K from cell potentials.**

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Equilibrium constant K of the Daniell cell at 25°C (E° = 1.10 V, n = 2):

  1. ≈ 10²⁰
  2. ≈ 10⁻²
  3. ≈ 10³⁷
  4. ≈ 10²
Show answer and solution

Correct answer: C. ≈ 10³⁷

**At equilibrium:** log K = nE°/0.0591 = 2 × 1.10/0.0591 ≈ 37.2. So K ≈ 10³⁷, very large. The forward reaction goes essentially to completion.

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