Voltaic Cells Under Non-Standard Conditions Step 1-2 Identify the reduction half-reaction. E° for this reaction is E°cathode- Step 3-4 Identify the oxidation half-reaction. E° for this reaction is E°anode- Step 5 Determine the number of electrons transferred in the process. Step 6 Calculate E° cell- E°cell = E°cathode - E°anode Step 7 Identify the form of the reaction quotient, Q. This is of the same form as the equilibrium constant expression for the system being studied. Step 8 Calculate the numerical value of Q. Step 9 Use the Nernst equation to calculate the cell potential. Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.025 M at 25 °C. 2 Fe (aq) + H,O2(aq) + 2 H¨(aq) → 2 Fe¯(aq) + 2 H,O(t) Acidic Solution Standard Electrode Potential, E(volts)

Voltaic Cells Under Non-Standard Conditions Step 1-2 Identify the reduction half-reaction. E° for this reaction is E°cathode- Step 3-4 Identify the oxidation half-reaction. E° for this reaction is E°anode- Step 5 Determine the number of electrons transferred in the process. Step 6 Calculate E° cell- E°cell = E°cathode - E°anode Step 7 Identify the form of the reaction quotient, Q. This is of the same form as the equilibrium constant expression for the system being studied. Step 8 Calculate the numerical value of Q. Step 9 Use the Nernst equation to calculate the cell potential. Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.025 M at 25 °C. 2 Fe (aq) + H,O2(aq) + 2 H¨(aq) → 2 Fe¯(aq) + 2 H,O(t) Acidic Solution Standard Electrode Potential, E(volts)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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