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April 20, 2014

April 20, 2014

Posted by **DAN** on Saturday, April 14, 2012 at 2:27pm.

Cu+(aq) + e− -> Cu(s)

I2(s) + 2 e− -> 2 I−(aq)

The cell is operated at 298 K with [Cu+ ] = 2.7 M and [I− ] = 2.7 M.

(a) Determine E for the cell at these concentrations.

(b) If [Cu+ ] was equal to 1.2 M, at what concentration of I− would the cell have zero potential?

- AP CHEMISTRY -
**DrBob222**, Saturday, April 14, 2012 at 3:04pmWhen you post problems that depend upon numbers you would do well to post the numbers in your text because texts change over the years and those constants change. The E value I looked up for I is =0.535 and the E value for Cu is +0.521.

Step 1 is to use the reduction ernst equation, substitute 2.7M and calculate E for I. I get +.509 but your values may be different. Do the same for Cu and I obtained 0.469; again your numbers may be different.

Then write the equation.

I2 ==> 2I^- E = +0.509v

Cu + e ==> Cu E = -0.469v

----------------------

I2 + 2Cu ==> 2Cu^+ + 2I^- Ecell = sum of E values.

To do b I would use the overall equation.

Ecell = EoCell - (0.0592/2)logQ

log Q = (I^-)^2(Cu^+)^2/((Cu)(I2) and solve for I^-

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