For the cell reaction 2Fe^3+(aq) + 2I-(aq) -> 2Fe^2+(aq) + I2(aq), E^ cell = 0.24 V at 298 K. The standard Gibbs energy ( _r G^°) of the cell reaction is:

Correct answer: (A) -46.32 kJ mol-1. Answer: (A) -46.32 kJ mol-1 Solution: The standard Gibbs energy of the cell reaction is _r G^° = -nFE^ cell. For 2Fe^3+ + 2I- -> 2Fe^2+ + I2, two electrons are transferred, so n = 2. _r G^° = -2 × 96500 × 0.24 = -46320 J mol-1 = -46.32 kJ mol-1.

NEET 2019 · ChemistryGalvanic & EMFPrevious Year Question

For the cell reaction $2 Fe X^{3 +} (aq) + 2 I X^{-} (aq) 2 Fe X^{2 +} (aq) + I X_{2} (aq)$ , $E_{ce l l}^{\circ} = 0.24$ V at $298$ K. The standard Gibbs energy ( $Δ_{r} G^{\circ}$ ) of the cell reaction is:

Answer: (A) $- 46.32$ kJ mol $^{- 1}$ . \textbf{Answer:} (A) $- 46.32$ kJ mol $^{- 1}$ \textbf{Solution:} The standard Gibbs energy of the cell reaction is $Δ_{r} G^{\circ} = - n F E_{ce l l}^{\circ} .$ For $2 Fe X^{3 +} + 2 I X^{-} 2 Fe X^{2 +} + I X_{2}$ , two electrons are transferred, so $n = 2$ .

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

Correct Answer

(A) $- 46.32$ kJ mol $^{- 1}$

Solution & Explanation

\textbf{Answer:} (A) $- 46.32$ kJ mol $^{- 1}$ \textbf{Solution:} The standard Gibbs energy of the cell reaction is $Δ_{r} G^{\circ} = - n F E_{ce l l}^{\circ} .$ For $2 Fe X^{3 +} + 2 I X^{-} 2 Fe X^{2 +} + I X_{2}$ , two electrons are transferred, so $n = 2$ . $Δ_{r} G^{\circ} = - 2 \times 96500 \times 0.24 = - 46320 J mol^{- 1} = - 46.32 kJ mol^{- 1} .$

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For the cell reaction 2FeX3+(aq)+2IX−(aq)​2FeX2+(aq)+IX2​(aq), Ecell∘​=0.24 V at 298 K. The standard Gibbs energy (Δr​G∘) of the cell reaction is:

Solution & Explanation

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For the cell reaction $2 Fe X^{3 +} (aq) + 2 I X^{-} (aq) 2 Fe X^{2 +} (aq) + I X_{2} (aq)$ , $E_{ce l l}^{\circ} = 0.24$ V at $298$ K. The standard Gibbs energy ( $Δ_{r} G^{\circ}$ ) of the cell reaction is: