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For a redox reaction with E° = 0.45 V and n = 3, what is the maximum work (W) ob

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Question: For a redox reaction with E° = 0.45 V and n = 3, what is the maximum work (W) obtainable from the reaction if 1 mole of reactants is used?

Options:

  1. -135 kJ
  2. -150 kJ
  3. 135 kJ
  4. 150 kJ

Correct Answer: 135 kJ

Solution: 

W = -nFE° = -3 * 96485 C/mol * 0.45 V = -130.9 kJ.

For a redox reaction with E° = 0.45 V and n = 3, what is the maximum work (W) ob

Practice Questions

Q1
For a redox reaction with E° = 0.45 V and n = 3, what is the maximum work (W) obtainable from the reaction if 1 mole of reactants is used?
  1. -135 kJ
  2. -150 kJ
  3. 135 kJ
  4. 150 kJ

Questions & Step-by-Step Solutions

For a redox reaction with E° = 0.45 V and n = 3, what is the maximum work (W) obtainable from the reaction if 1 mole of reactants is used?
  • Step 1: Identify the values given in the problem. We have E° = 0.45 V and n = 3.
  • Step 2: Understand the formula for calculating maximum work (W) in a redox reaction: W = -nFE°.
  • Step 3: Identify the value of F, which is the Faraday constant. F = 96485 C/mol.
  • Step 4: Substitute the values into the formula: W = -3 * 96485 C/mol * 0.45 V.
  • Step 5: Calculate the product of n, F, and E°: 3 * 96485 = 289455 C*V/mol.
  • Step 6: Multiply the result by 0.45 V: 289455 * 0.45 = 130.2525 kJ.
  • Step 7: Since the formula gives a negative value for work, we write W = -130.2525 kJ.
  • Step 8: Round the answer to three significant figures: W = -130.9 kJ.
  • Electrochemistry – Understanding redox reactions and their relationship to electrical work and potential.
  • Gibbs Free Energy – Relating the maximum work obtainable from a reaction to the Gibbs free energy change.
  • Faraday's Law – Using Faraday's constant to calculate the charge involved in the reaction.
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