The standard electrode potential for an electrochemical cell is 2.2V. Calculate the standard Gibbs energy change for reaction: X(s)+Y2+(aq)→X2+(aq)+Y(s) (Given, 1F=96500Cmol−1) (correct answer +1, wrong answer -0.25)
A
554.632kJ/mol
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B
384.786kJ/mol
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C
−424.6kJ/mol
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D
−384.123kJ/mol
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Solution
The correct option is C−424.6kJ/mol X(s)+Y2+(aq)→X2+(aq)+Y(s) ΔGo=−nFEo(cell) n=2 F=96500Cmol−1Eocell=2.2V ⇒ΔGo=−2×2.2V×96500Cmol−1 ⇒ΔGo=−424600CVmol−1 1CV=1Joule ⇒ΔGo=−424.600kJmol−1