The standard reduction potential for Mg 2 + / Mg is − 2.37 V and for Cu 2 + / Cu is 0.337 . The E cell ∘ for the following reaction is Mg + Cu 2 + ⟶ Mg 2 + + Cu

E cell ∘ = E cathode ∘ − E anode ∘ = E ( Cu 2 + / Cu ) ∘ − E ( Mg 2 + / Mg ) ∘ = 0.337 − ( − 2.37 ) V = 2.7 V

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Chemistry - Electrochemistry Question with Solution | TestHub

ChemistryElectrochemistryGalvanic cells/Nernst Equation/Concentration CellsEasy2 minPYQ_2009

ChemistryEasysingle choice

The standard reduction potential for $Mg^{2 +} / Mg$ is $- 2.37 V$ and for $Cu^{2 +} / Cu$ is $0.337$ . The $E_{cell}^{\circ}$ for the following reaction is $Mg + Cu^{2 +} ⟶ Mg^{2 +} + Cu$

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Answer:

Solution:

$E_{cell}^{\circ} = E_{cathode}^{\circ} - E_{anode}^{\circ}$ $= E_{(Cu^{2 +} / Cu)}^{\circ} - E_{(Mg^{2 +} / Mg)}^{\circ} = 0.337 - (- 2.37) V = 2.7 V$

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

⏱ 2mℹ️ Source: PYQ_2009

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