For the electrochemical cell, M ∣ M + ∥ X − ∣ X , E ∘ ( M + ∣ M ) = 0.44 V and E ∘ ( X ∣ X − ) = 0.33 V . From this data one can deduce that

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Chemistry - Electrochemistry Question with Solution | TestHub

ChemistryElectrochemistryGalvanic cells/Nernst Equation/Concentration CellsEasy2 minPYQ_2010

ChemistryEasysingle choice

For the electrochemical cell, $M ∣ M^{+} ∥ X^{-} ∣ X$ , $E^{\circ} (M^{+} ∣ M) = 0.44 V$ and $E^{\circ} (X ∣ X^{-}) = 0.33 V$ . From this data one can deduce that

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Solution:

$M^{+} + X^{-} \to M + X$ is spontaneous because for the cell represented by $M ∣ M^{+} ∥ X ∣ X$ , the value of $E^{\circ}$ is positive i.e. $(0.44 - 0.33) V = 0.11 V$ .

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

⏱ 2mℹ️ Source: PYQ_2010

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