ChemistryAll the energy released from the reaction X Y , Δ r G ° = – 193 kJ mol – 1 is used for oxidizing M + as M + M 3 + + 2 e – , E° = –0.25 V Under standard conditions, find the number of moles of M + oxidized when one mole of X is converted to Y [F = 96500 C mol – 1 ]

All the energy released from the reaction XY,ΔrG°=-193 kJ mol-1 is used for oxidizing M+ as M+ M 3+ + 2e-,
E° = –0.25 V
Under standard conditions, find the number of moles of M+ oxidized when one mole of X is converted to Y
[F = 96500 C mol-1]

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    Solution:

    XY;ΔG°=-193 kJ mol-1

    M+M3++2e-  E°=-0.25 V

    Hence G° for oxidation will be G° = - nFE°

    =-2×96500×(-0.25)=48250 J=48.25 kJ

    48.25 kJ energy oxidises one mole M+

    193 kJ energyoxidises 19348.25 mole M+=4 mole M+

     

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