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Electrochemistry · Class 12 · CBSE · Science Chemistry

The standard electrode potential (E^0) for the Daniell cell is 1.1text{ V}. What is the standard Gibbs energy change (Delta G^0) for the reaction? (F…

Practice question from Electrochemistry (Class 12 · CBSE · Science Chemistry), with the correct answer and a step-by-step solution.

medium · MCQ · Q-A1DEDF

The standard electrode potential (E0E^0) for the \Daniell\Daniell cell is 1.1 V1.1\text{ V}. What is the standard Gibbs energy change (ΔG0\Delta G^0) for the reaction? (F=96500 C mol−1F = 96500\text{ C mol}^{-1})

  1. A.−212.3 kJ mol−1-212.3\text{ kJ mol}^{-1}Correct answer
  2. B.−106.15 kJ mol−1-106.15\text{ kJ mol}^{-1}
  3. C.+212.3 kJ mol−1+212.3\text{ kJ mol}^{-1}
  4. D.+106.15 kJ mol−1+106.15\text{ kJ mol}^{-1}

Solution

The relation is ΔG0=−nFE0\Delta G^0 = -nFE^0. For the Daniell cell, n=2n = 2 electrons transferred. ΔG0=−2×96500 C mol−1×1.1 V=−212300 J mol−1=−212.3 kJ mol−1\Delta G^0 = -2 \times 96500\text{ C mol}^{-1} \times 1.1\text{ V} = -212300\text{ J mol}^{-1} = -212.3\text{ kJ mol}^{-1}.

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