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Electrochemistry question

2019 · Q85
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Electrochemistry question

2019 · Q85

NEETChemistryElectrochemistryMCQ+4 / −1
For the cell reaction
2Fe3+(aq) + 2I– (aq) →\to→ 2Fe2+(aq) + I2(aq)
EcellΘ{E_{cell}^\Theta }EcellΘ​ = 0.24 V at 298 K. The standard Gibbs energy (Δ\DeltaΔrGo) of the cell reaction is :
[Given that Faraday constant F = 96500 C mol–1]
  1. A
    46.32 kJ mol–1
  2. B
    23.16 kJ mol–1
  3. C
    –46.32 kJ mol–1
  4. D
    –23.16 kJ mol–1
View written solutionFree

Correct answer: C

Here, n = 2

Δ\Delta ΔGo = -nFEo

= – 2 × 96500 × 0.24

= – 46320 J mol–1

= – 46.32 KJ mol–1

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