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For the cell reaction 2Fe^3+(aq)+2I^-(aq)→ 2Fe^2+(aq)+I_2(aq) E_cell^0=0.24 V at 298 K. The standard Gibbs energy (Δ _ G^-) of the cell reaction is:…

NEET UG 2019 — Chemistry Physical Chemistry

2019mcqhard

For the cell reaction

2Fe3+(aq)+2I−(aq)→2Fe2+(aq)+I2(aq)2F{e}^{3+}(aq)+2{I}^{-}(aq)\rightarrow 2F{e}^{2+}(aq)+{I}_{2}(aq)2Fe3+(aq)+2I−(aq)→2Fe2+(aq)+I2​(aq)

Ecell0=0.24V{E}_{cell}^{0}=0.24 VEcell0​=0.24V at 298K.298 K.298K. The standard Gibbs energy (ΔrG−)({\Delta }_{r}{G}^{-})(Δr​G−) of the cell reaction is:

[Given that Faraday constant F=96500Cmol−1F=96500 Cmo{l}^{-1}F=96500Cmol−1 ]

Official previous-year question

Held on 30 Apr 2019 · Verified 9 Jul 2026.

Options

  1. A

    −46.32kJmol−1-46.32 kJ mo{l}^{-1}−46.32kJmol−1

  2. B

    −23.16kJmol−1-23.16 kJ mo{l}^{-1}−23.16kJmol−1

  3. C

    46.32kJmol−146.32 kJ mo{l}^{-1}46.32kJmol−1

  4. D

    23.16kJmol−123.16 kJ mo{l}^{-1}23.16kJmol−1

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