Chemistry - 1st Yr College Level

The corrosion of iron can be thought of as an electrochemical cell reaction. Calculate the voltage difference between two points of corroding iron differing only in their partial pressures of oxygen: 0.20 atm of oxygen at one point and 0.0010 atm of oxygen at the other. The reaction is: H2O + Fe (s) + 1/2 O2 (g) --> Fe(OH)2 (s)

  1. 👍 0
  2. 👎 0
  3. 👁 105
asked by Anne
  1. Ecell = Eocell - (0.0592/n)*log (more dilute soln/more concd soln).

    Eocell = 0 since the two electrodes are the same; i.e, this is a concentration cell.
    I would plug in 0.001 for more dilute solution and 0.20 for the more concentrated solution and calculate E. I believe n=2.
    Check my thinking.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. college chemistry - answer check ASAP!

    The corrosion of iron can be thought of as an electrochemical cell reaction. Calculate the voltage difference between two points of corroding iron differing only in their partial pressures of oxygen: 0.20 atm of oxygen at one

    asked by anne on March 13, 2010
  2. Chemistry

    the corrosion of iron is similar to the reactions that occur in an electrochemical cell. Oxidation and reduction occur at separate places on the metal and the circuit is completed by an electrolyte in solution one possible

    asked by ryan on November 30, 2011
  3. Chemistry

    The reaction below shows the corrosion process of iron. Calculate E°cell for the corrosion process and state whether you would predict that this is a spontaneous or nonspontaneous process. 2 Fe (s) + O2 (g) + 4 H+ (aq) → 2 Fe2+

    asked by Allie on August 8, 2010
  4. chemistry

    The voltage of an electrochemical cell depends on the redox reaction occurring in the cell. Given a redox reaction below: Zn(s) + Pb2+(aq) --> Zn2+(aq) + Pb(s) Pb2+(aq) + 2 e--->Pb(s)Eº = -0.13V Zn2+(aq) + 2 e--->Zn(s)Eº =

    asked by bliss on March 9, 2016
  5. c

    The voltage of an electrochemical cell depends on the redox reaction occurring in the cell. Given a redox reaction below: Zn(s) + Pb2+(aq) --> Zn2+(aq) + Pb(s) Pb2+(aq) + 2 e--->Pb(s)Eº = -0.13V Zn2+(aq) + 2 e--->Zn(s)Eº =

    asked by bliss on March 9, 2016
  6. chemistry

    2. The voltage of an electrochemical cell depends on the redox reaction occurring in the cell. Given a redox reaction below: Zn(s) + Pb2+(aq) --> Zn2+(aq) + Pb(s) Pb2+(aq) + 2 e--->Pb(s)Eº = -0.13V Zn2+(aq) + 2 e--->Zn(s)Eº =

    asked by bliss on March 9, 2016
  7. chemistry

    The reaction described by the equation Zn + Hg2Cl2 2Hg +Zn+2 + 2Cl is run on electrochemical cell. The E^0 of the cell at 25 degrees C is 1.03V. In the same cell, [Cl-]=.10 M and [Zn+2] is unknown, and the measured cell voltage is

    asked by Dylan on April 12, 2012
  8. chemistry (electrochemistry)

    1) For the following electrochemical cell Cu(s)|Cu2 (aq, 0.0155 M)||Ag (aq, 1.50 M)|Ag(s) write the net cell equation. Calculate the following values using standard potentials as needed. Eo cell and dGo for each

    asked by Andrew on April 15, 2013
  9. Chemistry

    Calculate the electrical voltage of an electrochemical cell using Pb(s) and Co(s) as electrodes along with their appropriate solutions. Co2+(aq) + 2e- --> Co(s) -0.28 V Pb2+(aq) + 2e- --> Pb(s) -0.13 V The oxidation reaction is

    asked by Melissa on March 18, 2010
  10. Chemistry

    Electrochemisry. Candy Chemist wishes to determine the concentration of CrO4^2- by electrochemical means in solution, and subsequently the Ksp of Ag2CrO4. She sets up one half-cell comprised of the Ag+|Ag couple (E=+0.799V) and a

    asked by KRH on April 28, 2016

More Similar Questions