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  2. Question
  3. Chemistry
  4. The value of Δ G (kJ mol-1) for the given cell is (take 1 F = 96500 C mol-1)

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Q. The value of $\Delta G (kJ\, mol^{-1})$ for the given cell is
(take $1\, F = 96500 \,C\,mol^{-1}$)

IIT JEEIIT JEE 2012Electrochemistry

Solution:

$\Delta G = - nEF=-\frac{2 \times 0.059 \times 96500}{1000}kJ=-11.4\, kJ$