3. Consider the following coupled reaction: Isocitrate + NAD+ à a-Ketoglutarate + CO2 + NADH First write the two standard half reactions written in reduction form for each with their std half reaction reduction potentials. Next calculate the AEo' for the reaction written above. Finally, based on the calculation convert this to the AGº

3. Consider the following coupled reaction: Isocitrate + NAD+ à a-Ketoglutarate + CO2 + NADH First write the two standard half reactions written in reduction form for each with their std half reaction reduction potentials. Next calculate the AEo' for the reaction written above. Finally, based on the calculation convert this to the AGº

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.44QE: For each of the reactions, calculate E from the table of standard potentials, and state whether the...

See similar textbooks

Similar questions

Consider the following half reactions in the attached image and their corresponding standard reduction potentials: 1. Consider the overall reaction wherein a pair of electrons passes from lactate to oxaloacetate. a. The overall net potential (ΔE°) (report up to two decimal places) for this reaction is _________ V. b. The standard Gibbs free energy for this reaction (report up to two decimal places) is ________ kJ/mol. c. The equilibrium constant (Keq) for this reaction (up to two decimal places) is ____________ .
Given the standard reduction potentials (Eo’) for ubiquinone (Q) and NADP+provided below, consider the following questions.Q + 2H+ + 2e- ---> QH2 Eo’ = 0.04 VNADP+ + H+ + 2e- ---> NADPH Eo’ = -0.32 V - Calculate the standard ΔEo’ for the oxidation of NADPH by Q. From the reactantsin your derived redox reaction, indicate the oxidant and reductant.- Calculate the standard free energy of the redox reaction in part (a) and indicate if thereaction is exergonic or endergonic.
Oxidation of lactate by cytochrome C (represented as cytochrome C (Fe3 +)) to pyruvate is an important biological reaction.Below are the reduction reactions and standard reduction potentials (E °) at pH = 7 and 25 ° C.Pyruvate + 2H + + 2e- = Lactate - (E ° = -0.185 V)Cytochrome C (Fe3 +) + e - = Cytochrome C (Fe2 +) (E ° = 0.254 V) Considering the Gibss free energy and Nernst equations, calculate the following equilibrium ratio (K) at 25 ° C, pH = 7.
Although the hydrogen electrode may be conceptually the simplest electrode and is the basis for the choice of reference potential in electrochemical systems, it is cumbersome to use. Therefore, several substitutes for it have been devised. One of these alternatives is the quinhydrone electrode (quinhydrone, Q ⋅ QH2, is a complex of quinone, C6H4O2 = Q, and hydroquinone, C6H4O2H2 = QH2), where the concentrations of Q ⋅ QH2 and QH2 are equal to each other. The electrode half-reaction is Q(aq) + 2 H+(aq) + 2 e− → QH2(aq), E⦵ = +0.6994 V. If the cell Hg(s)|Hg2Cl2(s)|HCl(aq)|Q ⋅ QH2|Au(s) is prepared, and the measured cell potential is +0.190 V, what is the pH of the HCl solution?
Ozone (O3) and chlorine dioxide (ClO2) are both strong oxidizing agents. Given the half reactions for these species as follow: O3 + 2H+ + 2e- = O2 + H2O, E0 = 2.07 V vs. SHE ClO2 + e- = ClO2-, E0 = 1.15 V vs. SHE Write and balance the overall reaction that occurs when O3 is mixed with NaClO2 in aqueous solution. What is the standard Gibbs free energy for the overall reaction?
Calculate the emf at 298.15 K generated by the oxidation of Fe2+ by O2 in acidic solution, according to the following reaction: O2(g) + 4H+(aq) + 4Fe2+(aq) ⟶ 4Fe3+(aq) + 2H2O(l) when [H+] = 0.003 M, [Fe3+] = 2.5 x 10 – 4 M, and [Fe2+] = 0.18 M. Also, write the complete (oxidation/reduction) half-reactions.
Given the following data: Cathode= AuNO3 (0.01 M) Anode: Hydrogen (1.01 M) In the attached photo, it shows how the cell potential (V) changes as the temperature (K) is varied. 1. determine the slope and y-intercept 2. Calculate delta S and delta H Thank you.
Arsenic(III) sulfide is oxidized with concentrated nitric acid into arsenic acid and sulfuric acid, with release of nitrogen dioxide gas. Compile the balanced chemical eqn for this reaction using oxidation-reduction electron-ion half reaction method (must show explicitly your work). The sum of all stochiometric coefficients in this chemical eqn is: A 30 B 50 C 70 D None of those is correct. If so, what is your value?
In a electrochemical cell are the molarity of the electrolyte CdCl2=0.10 kg/mole. Calculate the cellpotential at 25 degrees celcius when the activity coefficient for the proces are 0.10 mol/kg, CdCl2-solvent are decided to be 0.228, and the standard cell-potential are 0.624 V. Please answer very soon will give rating surely Show your work
For the following electrode, obtain the equation that relates the potential it develops as a function of pY. How is that electrode classified? Pb / PbY2-(0.15M), Y4-(0.12M)
Use the half reaction for pyruvate oxidation to compute the following at 25 °C. CH,COCOO-(pyruvate) + 4H₂O→ 2CO₂+HCO3 + 10H++ 10e a. Compute AG in kJ/mole pyruvate. b. Compute AG in kJ/mole pyruvate. Please answer only part b.
Write the relevant half-reactions, then combine them into a full reaction, for Fe2+ oxidation to Fe3+ by O2 going to H2O