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...

See similar textbooks

Similar questions

Determine K for each of the following reactions Determine AGan for each of the following reactions cell Determine the nonstandard cell potential, Eat, using the Nernst Equation and the stated conditions 3. Cu2 + S2042 Cu(s) + SO32 (base) pH = 8.9, concentration of Cu is 0.331 M, and the other concentrations are standard concentrations
Using these metal ion/metal standard reduction potentials: Cd2+ (aq)| Cd(s): -0.38 V; Zn2+ (aq) Zn(s): -0.78 V; Ni2+ (aq) |Ni (s): -0.29 V; Cu2+ (aq)| Cu(s): 0.30 V. Calculate the standard cell potential in V for the cell reaction Cu²+ (aq) + Cd(s)→Cd²+ (aq) + Cu(s) Report your answer with 2 places past the decimal point. Do not put unit in your answer. Type your answer...
Calculate the AG° (in kJ) for the reaction of elemental chlorine with the bromide ion at 298K. Refer to | the standard cell potentials on the last page of the note packet. Selected Answer: -54 A Calculate the AG° (in kJ) for the reaction of elemental chlorine with the bromide ion at 298K. Refer to the standard X cell potentials on the last page of the note packet. Selected Answer: 27.0
Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.5M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.19 volts. Your Answer:
Give a clear explanation handwritten answer ...
1
A certain half-reaction has a standard reduction potential Ered = -1.01 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.00 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. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? 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. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? 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. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used…
Calculate biological standard potential of the NAD+/NADH couple at 25°C.The reduction half-reaction is:NAD+(aq) + H+(aq) + 2e → NADH (aq)E° = -0.11 V (standard reduction potential ((pchem standard state)) Calculate potential for the redox couple above at pH=1 under standard biological conditions assuming that NAD+ and NADH are in unimolar concentrations.
Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? 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. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? 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. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the anode of this cell. Note: write the half reaction as it would actually occur at the anode. Oyes, there is a minimum. no minimum yes, there is a maximum. no maximum 0 E 0V red 0 E red = = ☐v
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 2. cell n A B U 2 2 2 calculated quantities (Check the box next to any that are wrong.) AGⓇ 64, kJ/mol O -160, kJ/mol -228. kJ/mol O O K -12 6.13 X 10 O -29 9.32 × 10 O 1.14 X 10 40 O 0 E 0.33 V 0.83 V 1.18 V O O G o
Give typed explanation not a single word hand written otherwise leave it the answer is 0.03295 please help me understand how that is the answer
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.