For the cell reaction 2Fe3+ (aq) + 2I- (aq) → 2Fe2+ (aq) + I2 (aq) E°cell = 0.24 V at 298 K The standard Gibbs energy (ΔrG°) of the cell reaction is [Given that Faraday constant F = 96500 C mol-1]

Question

For the cell reaction 2Fe3+ (aq) + 2I- (aq) → 2Fe2+ (aq) + I2 (aq) E°cell = 0.24 V at 298 K The standard Gibbs energy (ΔrG°) of the cell reaction is [Given that Faraday constant F = 96500 C mol-1] (A) 46.32 kJ mol-1 (B) 23.16 kJ mol-1 (C) - 46.32 kJ mol-1 (D) - 23.16 kJ mol-1

Tardigrade Admin · Accepted Answer

Δ G ominus = - n F E ominuscell = - 2 × 96500 × 0.24 J mol-1 = - 46320 J mol-1 = - 46.32 kJ mol-1

Q. For the cell reaction
$2 F e^{3 +} (a q) + 2 I^{-} (a q) \to 2 F e^{2 +} (a q) + I_{2}$ (aq)
$E_{ce ll}^{\circ} = 0.24 V$ at $298 K$
The standard Gibbs energy ( $Δ_{r} G^{\circ}$ ) of the cell reaction is
[Given that Faraday constant $F = 96500 C m o l^{- 1}$ ]

$46.32 k J m o l^{- 1}$

$23.16 k J m o l^{- 1}$

$- 46.32 k J m o l^{- 1}$

$- 23.16 k J m o l^{- 1}$

$Δ G^{⊖} = - n F E_{ce ll}^{⊖}$
$= - 2 \times 96500 \times 0.24 J m o l^{- 1}$
= - 46320 J $m o l^{- 1}$
= - 46.32 kJ $m o l^{- 1}$

Q. For the cell reaction 2Fe3+(aq)+2I−(aq)→2Fe2+(aq)+I2​ (aq) Ecell∘​=0.24V at 298K The standard Gibbs energy (Δr​G∘) of the cell reaction is [Given that Faraday constant F=96500Cmol−1]

46.32kJmol−1

23.16kJmol−1

−46.32kJmol−1

−23.16kJmol−1