3. Standard reduction potentials are listed for reactions under standard conditions. Standard conditions are 1 M concentrations of ions, I atm (or 1 bar) partial pressures for gases, and a temperature of 298 K. In Part I. you were asked to compare your measured cell potential to a calculated standard cell potential. The cell potential you measured was for a galvanic cell you prepared using 0.10 M solutions of Pb²* and Cu, not 1.0 M solutions, Write out the balanced equation for this cell, then give the Nernst equation for this cell. From the Nernst equation, explain why the cell potential under these nonstandard conditions should be equal to the standard cell potential for this particular reaction. a.

3. Standard reduction potentials are listed for reactions under standard conditions. Standard conditions are 1 M concentrations of ions, I atm (or 1 bar) partial pressures for gases, and a temperature of 298 K. In Part I. you were asked to compare your measured cell potential to a calculated standard cell potential. The cell potential you measured was for a galvanic cell you prepared using 0.10 M solutions of Pb²* and Cu, not 1.0 M solutions, Write out the balanced equation for this cell, then give the Nernst equation for this cell. From the Nernst equation, explain why the cell potential under these nonstandard conditions should be equal to the standard cell potential for this particular reaction. a.

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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Question

3. Standard reduction potentials are listed for reactions under standard conditions. Standard conditions
are 1 M concentrations of ions, I atm (or I bar) partial pressures for gases, and a temperature of 298 K:
In Part I, you were asked to compare your measured cell potential to a calculated standard cell
potential. The cell potential you measured was for a galvanic cell you prepared using 0.10 M
solutions of Pb2 and Cu, not 1.0 M solutions. Write out the balanced equation for this cell, then
give the Nernst equation for this cell. From the Nernst equation, explain why the cell potential
under these nonstandard conditions should be equal to the standard cell potential for this
particular reaction.
a.

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A certain half-reaction has a standard reduction potential -0 red = = +0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.70 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. ロ→ロ 0 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a minimum. ☐v red If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. no minimum Ś ? 0 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a maximum. Ov red If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. no maximum E E = = X
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell AG K E A 77. kJ/mol -14 3.24 x 10 0.80 V 119. kJ/mol 20 7.05 x 10 -1.23 V 60. kJ/mol -11 3.08 x 10 -0.62 V
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