Posted by **hriday** on Monday, March 2, 2009 at 5:45am.

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

- chemistry -
**Madeleine**, Monday, March 2, 2009 at 12:23pm
You multiply 12.3 by .50 to get 6.15 so none of those are the answer. simple!

- chemistry -
**DrBob222**, Monday, March 2, 2009 at 2:08pm
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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