NEET 2019, Chemistry Q17: Electrochemical Cell And Nernst Equation

For the cell reaction

$2F{e}^{3+}\left(aq\right)+2I^{-}\left(aq\right)\to 2F{e}^{2+}\left(aq\right)+l_2\left(aq\right)$

$E_{cell}^{\Theta }=0.24V298K$ at 298 K. The standard Gibbs energy $\left({\Delta }_r{G}^{\Theta }\right)$of the cell reaction is :

[Given that Faraday constant F = 96500 C mol^–1]