Which of the following statement is correct? If E C u 2 + ∣ C u ∘ = + 0.337 V and E S n 2 + ∣ S n ∘ = − 0.136 V .

Standard reduction potential of H⁺: ( E H + ∣ H 2 ∘ ) = 0 . E ∘ ( C u 2 + ∣ C u ) = 0.337 V . E ∘ ( S n 2 + ∣ S n ) = − 0.136 V . Since E C u 2 + ∣ C u ∘ is higher than that of H⁺, Cu²⁺ can be reduced by H₂. Also, since E S n 2 + ∣ S n ∘ is lower than that of H⁺, Sn²⁺ cannot be reduced by H₂.

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ChemistryElectrochemistryRelationship between Eº, DGº & KeqMedium2 minQB

ChemistryMediumstatement

Which of the following statement is correct?

If $E_{C u^{2 +} ∣ C u}^{\circ} = + 0.337 V$ and $E_{S n^{2 +} ∣ S n}^{\circ} = - 0.136 V$ .

Options:

Answer:

Solution:

Standard reduction potential of H⁺: $(E_{H^{+} ∣ H_{2}}^{\circ}) = 0$ .

$E^{\circ} (C u^{2 +} ∣ C u) = 0.337 V$ .

$E^{\circ} (S n^{2 +} ∣ S n) = - 0.136 V$ .

Since $E_{C u^{2 +} ∣ C u}^{\circ}$ is higher than that of H⁺, Cu²⁺ can be reduced by H₂. Also, since $E_{S n^{2 +} ∣ S n}^{\circ}$ is lower than that of H⁺, Sn²⁺ cannot be reduced by H₂.

Stream:JEESubject:ChemistryTopic:ElectrochemistrySubtopic:Relationship between Eº, DGº & Keq

⏱ 2mℹ️ Source: QB

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