Calculate Δ G ∘ for the cell: Sn ( s ) Sn ( IM ) ++ Ag ( IM ) + Ag ( s ) at 2 5 ∘ C ( E cell ∘ = 0.90 V )

Δ G ∘ = − nF cell ∘ = − 2 × 96500 × 0.90 = − 173700 J = − 173.7 kJ

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ChemistryElectrochemistryGalvanic cells/Nernst Equation/Concentration CellsMedium2 minPYQ_2023

ChemistryMediumsingle choice

Calculate $Δ G^{\circ}$ for the cell: $Sn_{(s)} Sn_{(IM)}^{++} Ag_{(IM)}^{+} Ag_{(s)} at 2 5^{\circ} C (E_{cell}^{\circ} = 0.90 V)$

Answer:

Solution:

$Δ G^{\circ} = - nF_{cell}^{\circ} = - 2 \times 96500 \times 0.90 = - 173700 J = - 173.7 kJ$

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

⏱ 2mℹ️ Source: PYQ_2023

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