For the cell reaction 2 {Fe}^{3+}( {aq})+2 {I}^{-}( {aq}) \to 2 {Fe}^{2+}( {aq})+ {I}_{2}( {aq}) {{E}^{⊖}}_{ {cell}} = 0.24 V at 298 K. The standard Gibbs energy \\Delta_r (G^{⊖}) of the cell reaction is : [Given that Faraday constant F = 96500 C mol{^{–1}}] [NEET 2019]

Correct Answer is : – 46.32 kJ mol–1

NEET 2019 Physics and Chemistry

Question : 31 of 90

Marks: +1, -0

For the cell reaction
2Fe3+(aq)+2I−(aq) →2Fe2+(aq)+I2(aq)
E⊖cell = 0.24 V at 298 K. The standard Gibbs energy Δr(G⊖) of the cell reaction is :
[Given that Faraday constant F = 96500 C mol‌–1]

[NEET 2019]

– 23.16 kJ mol‌–1
46.32 kJ mol‌–1
23.16 kJ mol‌–1
– 46.32 kJ mol‌–1

Validate

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