Consider the two half-reactions below and their standard reduction potentials.NAD+ + H+ + 2e → NADHElo= -0.32 Va-Ketoglutarate + CO₂ + 2H+ + 2e → Isocitrate E' = -0.38 V(a) What is AE" for the spontaneous redox reaction that is, the reaction that actuallyoccurs under standard biochemical conditions (pH 7)?(b) Which of the following statements are correct under standard biochemical conditions?i. The concentration of H+ is 1.0 M.ii. The reaction NAD+ + Isocitrate → NADH + H+ + a-Ketoglutarate + CO₂ is favor-able.iii. NAD+ accepts electrons from isocitrate.iv. The NAD → NADH reaction actually occurs in reverse. The a-ketoglutarate →isocitrate reaction occurs as written.(c) Calculate AG" for the reaction in (a). (pH 7, 25°C, pressure, 1 atm.)(d) Suppose that the actual conditions are T = 25°C, pH = 7, CO₂ = 1 atm, [a-Ketoglutarate]10 mM, [NAD+] = 2.5 mM, and [NADH] = 0.5 mM.PAR= 2 mM, [Isocitrate]DEWhat is the value of AG under those conditions?(Hints: pH 7 is already included in AG". Similarly, 1 atm is the standard pressure ofCO2, which is also taken into account in AG.)

∆G'0 = -nF∆E'0 here; ∆G'0 is the change in standard Gibbs free energy. 'n' is the number of…

Answered: Consider the two half-reactions below…

Biochemistry

6th Edition

ISBN:9781305577206

Author:Reginald H. Garrett, Charles M. Grisham

Publisher:Reginald H. Garrett, Charles M. Grisham

Chapter27: Metabolic Integration And Organ Specialization

Section: Chapter Questions

Problem 4P

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