The Gibbs change (in J) for the given reaction at [Cu²⁺] = [Sn²⁺] = 1 M and 298K is: Cu(s) + Sn²⁺(aq.) → Cu²⁺(aq.) + Sn(s); (E_ S n²⁺ |Sn ⁰ = - 0.16 V, E_ C u²⁺ |Cu ⁰ = 0.34 V) Take F = 96500 C mol^–1)

Redox Reactions and Electrochemistry: JEE Main 2020 Chemistry question

JEE Main 2020 · 2 Sep, Morning shift · Q6

JEE Main 20202 Sep, Morning shiftChemistryMediumRedox Reactions and Electrochemistry138× since 2002

The Gibbs change (in J) for the given reaction at [Cu²⁺] = [Sn²⁺] = 1 M and 298K is : Cu(s) + Sn²⁺(aq.)

\to

Cu²⁺(aq.) + Sn(s); (

E_{S{n^{2 + }}|Sn}^0 = - 0.16\,V

E_{C{u^{2 + }}|Cu}^0 = 0.34\,V

) Take F = 96500 C mol^–1)

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JEE Main 2020 Redox Reactions and Electrochemistry Question with Answer (2 Sep Morning shift, Q6) | JEE Arc