Two metals 'A' and 'B' have E red ∘ value equal to 0.36 V and 1.23 V . What will be the correct cell equation?

From E red ∘ . values, it is clear that A is more electropositive than B (as it has lesser E ∘ red ), hence it can replace B from its salt solution and act as anode in galvanic cell. Hence, correct cell equation will be: A + B 2 + ⟶ A 2 + + B

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Chemistry - Electrochemistry Question with Solution | TestHub

ChemistryElectrochemistryCommercial Cells/Fuel cellMedium2 minPYQ_2004

ChemistryMediumsingle choice

Two metals 'A' and 'B' have $E_{red}^{\circ}$ value equal to 0.36 V and 1.23 V . What will be the correct cell equation?

Options:

Answer:

Solution:

From $E_{red}^{\circ}$ . values, it is clear that $A$ is more electropositive than $B$ (as it has lesser $E^{\circ}_{red}$ ), hence it can replace $B$ from its salt solution and act as anode in galvanic cell. Hence, correct cell equation will be: $A + B^{2 +} ⟶ A^{2 +} + B$

Stream:JIPMERSubject:ChemistryTopic:ElectrochemistrySubtopic:Commercial Cells/Fuel cell

⏱ 2mℹ️ Source: PYQ_2004

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