Chemistry DR BOB

Under standard conditions of 1 atm and 298.15K, the half-cell reduction potential E,zero for the anode in a voltaic cell is 0.37V. The half-cell reduction potential E,zero for the cathode of the cell is 0.67V. The number of moles, n, of electrons transferred in the redox reaction is 3. Calculate the equilibrium constant K for this reaction at 25degC. Enter your answer in exponential notation with two decimal places.

  1. 👍 0
  2. 👎 0
  3. 👁 213
  1. I assume you mean the reaction in which electrons flow from the anode to the cathode spontaneously.
    Anode is on the left, it is oxidized; therefore, Eo oxidation = -0.37
    Cathode is on the right so it receives the electrons and it is reduced so Eo redn = 0.67.
    EoCell = Eox + Ered = ?
    Then nFEo = RTlnK.
    You know n, Eo and F (96,485), R(8.314) and T. Solve for K.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry- electrochemical cell

    What makes this an oxidation-reaction? 3Ag2S+2Al(s) -> Al2S3+6 Ag(s)? Write the half-reactions showing the oxidation and reduction reactions. Identify which is the oxidation reaction and which is the reduction reason. What is

    asked by princess on March 25, 2012
  2. chemistry

    Complete the two reduction half reactions for the cell shown at the right, and show the line notation for the cell by dragging labels to the correct position. (The electrode on the left is the anode, and the one on the right is

    asked by shanonn on May 5, 2013
  3. Chemistry

    Consider the following cell: Pt|H2(g, 0.460 atm)|H (aq, ? M)||Ag (aq, 1.00 M)|Ag(s) If the measured cell potential is 1.00 V at 25 °C and the standard reduction potential of the Ag /Ag half-reaction couple is 0.80 V, calculate

    asked by Daisy on March 19, 2012
  4. Chemistry

    For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g) + O2(g) --> 2NO2(g) the standard change in Gibbs free energy is ΔG° = -69.0 kJ/mol. What is ΔG for

    asked by Janavi on March 23, 2014
  5. Electrochemistry

    In lab, we did an experiment with electrochemical cells with solutions of ZnSO4, CuSO4, Al2(SO4)3 and MgSO4 and their respective metal electrodes. There are a couple of post-lab questions that I'm not sure about: (1) Summarize

    asked by Donna on May 16, 2008
  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) Determine E for the cell at

    asked by DAN on April 14, 2012
  2. Chemistry

    Constants The following values may be useful when solving this tutorial. Constant Value E∘Cu 0.337 V E∘Fe -0.440 V R 8.314 J⋅mol−1⋅K−1 F 96,485 C/mol T 298 K Part A In the activity, click on the E∘cell and Keq

    asked by Jasper on March 28, 2018
  3. 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 the

    asked by DAN on April 6, 2012
  4. chemistry

    Consider the cell: (Pt) H2/H+ || (Pt) H+/H2. In the anode half-cell, hydrogen gas at 1.0 atm is bubbled over a platinum electrode dipping into a solution that has a pH of 7.0. The other half-cell is identical to the first except

    asked by Anonymous on March 27, 2012
  5. Chemistry

    The standard reduction potential for Cr3+(aq) is −0.74 V. The half-reaction for the reduction of Cr3+(aq) is the following. Cr3+(aq) + 3 e− → Cr(s) The standard reduction potential for Ni2+(aq) is −0.26 V. The

    asked by Anonymous on April 12, 2018
  6. chem

    Q: Calculate ℰ° values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in the Standard Reduction Potentials table.

    asked by . on May 7, 2019

You can view more similar questions or ask a new question.