Ask Question
17 April, 06:09

The potential in an electrochemical cell, E, is related to the Gibb's free energy change (ΔG) for the overall cell redox reaction: (1) ΔG0 = - n F E0 where n is the number of electrons transferred during the redox reaction, F is Faraday's constant (96,500 C / mol), and the superscript 0 indicates standard conditions (1 atm, 1 M concentrations, and 25 °C). Thus, a measurement of the cell voltage at standard conditions can be used to determine ΔG0. As an example, the following cell reaction: Zn (s) + Cu2 + (aq) → Zn2 + (aq) + Cu (m) generates a cell voltage of + 1.10 V under standard conditions. Calculate and enter delta G degree (with 3 sig figs) for this reaction in kJ/mol.

+1
Answers (1)
  1. 17 April, 09:25
    0
    As an example, the following cell reaction: Zn (s) + Cu2 + (aq) → Zn2 + (aq) + Cu (m) generates a cell voltage of + 1.10 V under standard conditions. Calculate and enter delta G degree (with 3 sig figs) for this reaction in kJ/mol.

    Zn (s) + Cu2 + (aq) → Zn2 + (aq) + Cu (m)

    ΔG = ΔG° + RTInQ

    Q = 1

    ΔG = ΔG°

    ΔG = = nFE°

    n=no of electrons transfered.

    E° = 1.1v

    ΔG° = - 2 * 96500 * 1.10

    = - 212300J

    ΔG° = -212.3kJ/mol

    Therefore, the ΔG° = - 212.3kJ/mol
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “The potential in an electrochemical cell, E, is related to the Gibb's free energy change (ΔG) for the overall cell redox reaction: (1) ΔG0 ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers