chemistry

the quantity of electricity required to reduce 12.3g of nitrobenzene to aniline assuming 50% current efficiency is
1. 115800 C
2. 57900 C
3. 231600 C
4. 28950 C

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asked by hriday
  1. You multiply 12.3 by .50 to get 6.15 so none of those are the answer. simple!

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  2. Check my thinking on this.
    C6H5NO2 ==> C6H5NH2
    molar mass C6H5NO2 = 123

    Change of electrons is 6, N going from +5 oxidation state to -1 oxidation state or gain of 6 electrons.

    Therefore, 1 Faraday or 96,485 coulombs will reduce 123/6 = 20.5 g C6H5NO2. But since the efficiency is only 50%, it will reduce only half that amount or 20.5/2 = 10.25 g or 10.25/123 = 0.08333 mole.

    How many moles do we have? That is 12.3/123 = 0.1; therefore,
    # coulombs = 96,485 C x (0.1/0.08333)= ??
    Check my work.

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    posted by DrBob222
  3. 57900

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  4. Change in o.s=6
    Now 6 F is req'd to reduce 1 mole
    Therefore for 12.3/123=0.1 mole we need
    0.1*6=0.6 F
    But since current is 50℅ efficient..
    Therefore for 0.6 we need 0.6*2=1.2 F
    1.2*96500=115800 C

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  5. Mole=6×12.3/123=0.6
    Charge= 0.6×96500
    As 50% efficiency
    So, 2×0.6×96500=115800 C

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  6. mishra

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    posted by ayush
  7. Change in o.s=6e=6f
    123g req.6f
    But efficiency is half 50%so
    123g req 12f so,
    12.3g req 12*12.3/123
    =1.2f
    In coulomb 1.2*96500=115800

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