For the cell reaction, Cu 2+ (C 1 ) (aq) + Zn(s) → Zn 2+ (C 2 ) (aq) + Cu(s), the change in free energy ( Δ G ) at a given temperature is a function of

ΔG = ΔG o + RT lnQ ΔG = ΔG o + RT ln Zn +2 Cu +2 ΔG = ΔG o + RT ln C 2 C 1 So, Δ G is function of l n ( C 2 / C 1 ) .

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ChemistryElectrochemistryGalvanic cells/Nernst Equation/Concentration CellsEasy2 minPYQ_2020

ChemistryEasysingle choice

For the cell reaction,
$\underset{{(C}_{1})}{{Cu}^{2+}} (aq) + Zn(s) \to \underset{{(C}_{2})}{{Zn}^{2+}} (aq) + Cu(s),$
the change in free energy $(Δ G)$ at a given temperature is a function of

Options:

Answer:

Solution:

$ΔG = {ΔG}^{o} + RT lnQ$
$ΔG = {ΔG}^{o} + RT ln \frac{[{Zn}^{+2}]}{[{Cu}^{+2}]}$
$ΔG = {ΔG}^{o} + RT ln \frac{C_{2}}{C_{1}}$
So, $Δ G$ is function of $l n (C_{2} / C_{1})$ .

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

⏱ 2mℹ️ Source: PYQ_2020

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