Calculate E cell ∘ for Cd ( s ) Cd ( IM ) ++ Ag ( MM ) + Ag ( s ) . [ E Cd ∘ = − 0.403 V ; E Ag ∘ = 0.799 V ]

For the given cell, anode is Cd and cathode is Ag. E cell ∘ = E cathode ∘ − E anode ∘ = 0.799 − ( − 0.403 ) = 1.202 V

Chemistry - Electrochemistry Question with Solution | TestHub

ChemistryElectrochemistryGalvanic cells/Nernst Equation/Concentration CellsEasy2 minPYQ_2023

ChemistryEasysingle choice

$Calculate E_{cell}^{\circ} for Cd_{(s)} Cd_{(IM)}^{++} Ag_{(MM)}^{+} Ag_{(s)} . [E_{Cd}^{\circ} = - 0.403 V; E_{Ag}^{\circ} = 0.799 V]$

Answer:

Solution:

For the given cell, anode is $Cd$ and cathode is Ag. $E_{cell}^{\circ} = E_{cathode}^{\circ} - E_{anode}^{\circ} = 0.799 - (- 0.403) = 1.202 V$

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

⏱ 2mℹ️ Source: PYQ_2023

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