Verified Solution • 2025–26 Session moderate

QNEET-2019-Ch-775: NEET 2019 Chemistry - Class 12 NEET-2019-Ch-775 Solution: For the cell reaction \(2Fe^{3+}(aq) + 2I^-(aq) 2Fe^{2+}(aq) +…

For the cell reaction

2Fe^{3+}(aq) + 2I^-(aq) \rightarrow 2Fe^{2+}(aq) + I_2(aq)

E_{cell}^\circ = 0.24\ \text{V}

at 298 K. The standard Gibbs energy (

\Delta_r G^\circ

) of the cell reaction is: [Given that Faraday constant F = 96500 C

mol^{-1}

] 46.32 kJ

mol^{-1}

23.16 kJ

mol^{-1}

-46.32 kJ

mol^{-1}

-23.16 kJ

mol^{-1}

Step-by-Step Verified Solution

Here, n = 2 _ G o = -nFE o = � 2 _ 96500 _ 0.24 = � 46320 J mol �1 = � 46.32 KJ mol �1