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JEE Main & Advanced Chemistry Electrochemistry / विद्युत् रसायन Question Bank Electrode potential Ecell Nernst equation and ECS

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    Calculate standard free energy change for the reaction \[\frac{1}{2}Cu(s)+\frac{1}{2}C{{l}_{2}}(g)\]⇌\[\frac{1}{2}C{{u}^{2+}}+C{{l}^{-}}\] taking place at \[{{25}^{o}}C\] in a cell whose standard e.m.f. is 1.02 volts           [MP PMT 1997]

    A)                 ? 98430 J             

    B)                 98430 J

    C)                 96500 J 

    D)                 ? 49215 J

    Correct Answer: A

    Solution :

               \[\Delta G=-nF{{E}^{o}}\]                                 \[\Delta G=-1\times 96500\times 1.02\];               \[\Delta G=-98430\].


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