ChemistryNEET 2019Electrochemical cells and Nernst equation

Electrochemistry

For the cell reaction $2 F e^{3 +} (aq) + 2 I^{-} (aq) \to 2F e^{2 +} (aq) + I_{2} (aq)$ , $E_{ce l l}^{⊖} = 0.24$ V at 298 K. The standard Gibbs energy ( $Δ_{r} G^{⊖}$ ) of the cell reaction is: (Given: Faraday constant $F = 96500 C mo l^{- 1}$ )

A. $- 46.32 kJ mo l^{- 1}$ ✓
B. $- 23.16 kJ mo l^{- 1}$
C. $46.32 kJ mo l^{- 1}$
D. $23.16 kJ mo l^{- 1}$

You have the answer. The worked solution — and why the other three were written — is part of a paid pack.

Electrochemistry

More from this chapter in past papers