AP CHEMISTRY

A voltaic cell is constructed that uses the following half-cell reactions.
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?

asked by DAN
  1. When 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^-

    posted by DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. AP CHEMISTRY

    A voltaic cell is constructed that uses the following half-cell reactions. 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)
  2. AP Chemistry

    A voltaic cell is constructed that uses the following half-cell reactions. Cu+(aq) + e- Cu(s) I2(s) + 2 e- 2 I -(aq) The cell is operated at 298 K with [Cu+ ] = 2.3 M and [I - ] = 3.3 M. (a) Determine E for the cell at these
  3. AP Chemistry

    A voltaic cell is constructed that uses the following half-cell reactions. Cu+(aq) + e- Cu(s) I2(s) + 2 e- 2 I -(aq) The cell is operated at 298 K with [Cu+ ] = 2.3 M and [I - ] = 3.3 M. (a) Determine E for the cell at these
  4. chemistry 2

    A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb2+ half-cell. Measurement shows that thesilver electrode is positive. -Write balanced half-reactions and the overall spontaneous reaction.
  5. AP CHEMISTRY

    A voltaic cell is constructed that is based on the following reaction. Sn2+(aq) + Pb(s) -> Sn(s) + Pb2+(aq) (a) If the concentration of Sn2+ in the cathode half-cell is 1.80 M and the cell generates an emf of +0.219 V, what is
  6. Chemistry

    One half-cell in a voltaic cell is constructed from a silver wire electrode in a .25 M solution of AgNO3 . The other half-cell consists of a zinc electrode in a .001 M solution of Zn(NO3)2. Calculate the cell potential I have no
  7. Chemistry

    Consider a chromium-silver voltaic cell that is constructed such that one half-cell consists of the chromium, Cr, electrode immersed in a Cr(NO3)3 solution, and the other half-cell consists of the silver, Ag, electrode immersed in
  8. Chemistry

    A voltaic cell consists of a Pb /Pb^2+ half-cell and a Cu/Cu^2 half-cell at 298K. The initial concentrations of Pb^2+ and Cu^2 are 5.20×10−2 M and 1.40 M, respectively.
  9. chem 2

    Consider a chromium-silver voltaic cell that is constructed such that one half-cell consists of the chromium, Cr, electrode immersed in a Cr(NO3)3 solution, and the other half-cell consists of the silver, Ag, electrode immersed in
  10. Chemistry again

    Two voltaic cells are to be joined so that one will run the other as an electrolytic cell. In the first cell, one half-cell has Au foil in 1.00M Au(NO3)3, and the other half-cell has a Cr bar in 1.00M Cr(NO3)3. In the second cell,

More Similar Questions