The last reaction of the citric acid cycle is the conversion of malate to oxaloacetate, catalyzed by malate dehydrogenase. The standard reduction potential for oxaloacetate malate is -0. 166 V. 1. What is the difference in the standard reduction potential for the whole redoxreaction and what is the standard free energy change for the full reaction? To calculate this, look up the standard reduction potential for the correct redox-active cofactor in the lecture notes (table 15-1). Faraday's constant F = 96485 J mol Note: In an exam, you will be given the standard reduction potential and the constants. O A) Ae" = -0.481 V AG= 192.82 kJ/mol A 0.481 V B) AG = +4.52 k/mol !3! C Ae=-0.149 V AG = +28.75 kJ/mol D) Ac = -0.149 V AG 28.75 kl/mol E) Ar +0.149 V AG--28.75 kl/mol

The last reaction of the citric acid cycle is the conversion of malate to oxaloacetate, catalyzed by malate dehydrogenase. The standard reduction potential for oxaloacetate malate is -0. 166 V. 1. What is the difference in the standard reduction potential for the whole redoxreaction and what is the standard free energy change for the full reaction? To calculate this, look up the standard reduction potential for the correct redox-active cofactor in the lecture notes (table 15-1). Faraday's constant F = 96485 J mol Note: In an exam, you will be given the standard reduction potential and the constants. O A) Ae" = -0.481 V AG= 192.82 kJ/mol A 0.481 V B) AG = +4.52 k/mol !3! C Ae=-0.149 V AG = +28.75 kJ/mol D) Ac = -0.149 V AG 28.75 kl/mol E) Ar +0.149 V AG--28.75 kl/mol

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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A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGº. • 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 n aG K E -21 1.42 x 10 A 1 119. kJ/mol O 1.23 V -- В - 51. kJ/mol 1.16 X 10 -0.53 V -11 2.06 X 10 1 -61. kJ/mol 0.63 V
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