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 $n = 2$ . $Δ_{r} G^{\circ} = - 2 \times 96500 \times 0.24 = - 46320 J mol^{- 1} = - 46.32 kJ mol^{- 1} .$

🎯

43,000+ questions in हिंदी & English · one-tap toggle

Practice NEET 2019 Chemistry — free, with instant solutions

43,000+ NEET questions solved step-by-step, chapter-wise, in the MedicNEET app.

Open →📚Practice all NEET Chemistry PYQs chapter-wise →💡Don't get it? Learn the Electrochemistry concepts →

← Chemistry Q31 Chemistry Q33 →

More NEET PYQ solutions

ChemThe correct value of cell potential (in volt) for the reaction that occurs when the following two half cells are connected is: Fe^2+(aq) + 2e- -> Fe(s), E^° = -0.44 V Cr2O7^2- + 14H+ + 6e- -> 2Cr^3+ + 7H2O, E^° = +1.33 V ChemThe E^° values are given as: E^ Al+/Al = +0.55 V and E^ Tl+/Tl = -0.34 V; E^ Al^3+/Al = -1.66 V and E^ Tl^3+/Tl = +1.26 V. Identify the incorrect statement.ChemThe correct option for a redox couple is ChemGiven below are the half-cell reactions: MnO4^- + 8H+ + 5e- -> Mn^2+ + 4H2O, E^ MnO4^-/Mn^2+ = -1.510 V 1/2 O2 + 2H+ + 2e- -> H2O, E^ O2/H2O = +1.223 V Will the permanganate ion, MnO4^-, liberate O2 from water in the presence of an acid?ChemAt 298 K, the standard electrode potentials of Cu^2+/Cu, Zn^2+/Zn, Fe^2+/Fe and Ag+/Ag are 0.34 V, -0.76 V, -0.44 V and 0.80 V, respectively. On the basis of standard electrode potential, predict which of the following reactions cannot occur?ChemThe standard electrode potential (E^°) values of Al^3+/Al, Ag+/Ag, K+/K and Cr^3+/Cr are -1.66 V, 0.80 V, -2.93 V and -0.74 V, respectively. The correct decreasing order of the reducing power of the metals is:ChemConsider the change in oxidation state of bromine corresponding to the standard reduction (electrode) potentials shown for each successive step: BrO4^- +1.82 V BrO3^- +1.50 V HBrO +1.595 V Br2 +1.0652 V Br^- Then the species undergoing disproportionation is ChemIf the E^ cell for a given reaction has a negative value, which of the following gives the correct relationships for the values of G^° and Keq?

More: All NEET 2019 Chemistry PYQs · NEET Chemistry PYQs · All NEET PYQs · Previous year papers

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

More NEET PYQ solutions

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: