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ChemistryElectrochemistryGalvanic cells/Nernst Equation/Concentration CellsMedium2 minPYQ_2016

ChemistryMediumsingle choice

If the $E_{c e l l}^{o}$ for a given reaction has a negative value, which of the following gives the correct relationship for the values of $∆ G^{o}$ and $K_{e q}$ ?NEET 2016 (Phase 2)

Options:

Answer:

Solution:

${ΔG}^{\circ} = - 2.303 RT \log k$

${ΔG}^{\circ} = - {nFE}^{o}$

$∵ E_{cell}^{o} = - ve (E_{cell}^{o} < 0)$ , then,

${ΔG}^{\circ} = - nF (- E^{o}) = + ve$

From the equation, ${ΔG}^{\circ} = - 2.303 RT \log k$

$∴ ∆ G^{\circ} = + v e$ & $K_{e q} = - v e$

i.e., $∆ G^{\circ} > 0$ & $K_{e q} < 1$ .

Stream:NEETSubject:ChemistryTopic:ElectrochemistrySubtopic:Galvanic cells/Nernst Equation/Concentration Cells

⏱ 2mℹ️ Source: PYQ_2016

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