Standard redox potentials E' for some common compounds in biochemistry: Eo' (Volt) + 0,81 12 O2 + 2 H+ + 2 e NO3 + 2 H+ + 2 e 2 cyt c (ox) + 2 e 2 cyt b (ox) + 2 e Pyruvate + 2 H+ + 2 e NAD + 2 H+ + 2 e Acétoacétate + 2 H+ + 2 e (2) acétoacétate + NADH+H* H₂O NO₂ + H₂O 2 cyt c (red) 2 cyt b (red) Lactate (3) 2 cyt c (ox) + 2 cyt b (red) NADH + H* B-hydroxybutyrate +0,42 + 0,25 + 0,08 - 0,19 -0,32 With the help of the above table, determine the spontaneous direction of the following reactions in the standard conditions. Justify your answers by calculating the Gibbs (free) energy of reaction in each case. (1) pyruvate + B-hydroxybutyrate - 0,35 lactate + acétoacétate B-hydroxybutyrate + NAD+ 2 cyt c (red) + 2 cyt b (ox)
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- Consider the two half-reactions below and their standard reduction potentials. NAD+ + H+ + 2e → NADH Elo= -0.32 V a-Ketoglutarate + CO₂ + 2H+ + 2e → Isocitrate E' = -0.38 V (a) What is AE" for the spontaneous redox reaction that is, the reaction that actually occurs 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] DE What is the value of AG under those conditions? (Hints: pH 7 is already…Begining with 1 M concentrations of each reactant and product at pH=7 and 25.0 degrees C, calculate the K'eq of the reaction Pyruvate + NADH Lactate + NADH+H+. Note the temperature of this reaction will not affect the standard reducton potential delta E° in the table 13-7b.Begining with 1 M concentrations of each reactant and product at pH=7 and 25.0 degrees C, calculate the K'eq of the reaction Pyruvate + NADH Lactate + NADH+H+. Note the temperature of this reaction will not affect the standard reducton potential
- Begining with 1 M concentrations of each reactant and product at pH=7 and 25.0 degrees C, calculate the K'eq (to one decimal point) of the reaction Pyruvate + NADH+H+ <=> Lactate + NAD+.Note the temperature of this reaction will not affect the standard reducton potential delta E'o in the table 13-7b. please provide a comprehensive explanation with each step taken.Consider the following equilibrium at 25ºC :Glucose-1-Phosphate Glucose-6-PhophateUsing the equilibrium concentrations of [Glucose-1-Phosphate] = 0.35 M and [Glucose-6-Phosphate] = 1.65 M, calculate BOTH K′eqand Gº′ for this reaction. Is this reaction exergonicor endergonic? R = 8.314 J/K·molCalculate AG for this reaction under the following conditions: 37°C, pH 7, [Pyruvate] = [CO₂] = 4.0 mM, [OAA] = 2.0 mM, [ATP] = 3.5 mM, [P;] = 5.0 mM, and [ADP] = 1.8 mM. Use 2 signficant figures. AG= i kJ.mol-1 Under these conditions, the reaction is (Tolerance is +/- 2%)
- The standard reduction potential for ubiquione (A or coenzyme Q) is .045 V, and the standard reduciton potential (E) for FAD is -0.219 V. Using these values, show that the oxidation for FADH2 by ubiquinone theoretically liberates enough energy to drive the synthesis of ATP. Faraday constant =96.48KJ/Vol delta G' standard for ATP Synthesis is +30.5 KJ/mol R=8.314 J/mol K=1.987 cal/mol KAcetyl CoA + 2H* + 2e = pyruvate + COASH E = -0.48 V Ubiquinone + 2H* + 2e = Ubiquinol E" = +0.04 V Consider the redox rxn wherein a pair of e passes from pyruvate to ubiquinone. Calculate the change in standard Gibbs free energy (kJ/mol). Report answer to two decimal places.The reactionPyruvate-(aq) + NADH(aq) + H+(aq) → lactate-(aq) + NAD+(aq)where NAD+ is the oxidized form of nicotinamide adenine dinucleotide, occurs in muscle cells deprived of oxygen during strenuous exercise and can lead to cramp. Calculate the biological standard Gibbs energy, ΔrG⊕, for the reaction at 310 K given that the thermodynamic standard reaction Gibbsenergy ΔrGΘ = -66.6 kJ mol-1.
- If a 0.1 M solution of glucose 1- phosphate at 25 °C is incubated with a catalytic amount of phosphoglucomutase, the glucose 1-phosphate is transformed to glucose 6-phosphate. At equilibrium, the concentrations of the reaction components are Calculate Keq and ΔG′° for this reaction.Given the following coupled reactions: phosphoenolpyruvate + H2O → pyruvate + Pi ΔG°'= -61.9 kJ/mol ATP + H2O → ADP + Pi ΔG°'= -30.5 kJ/mol write the overall reaction, calculate the ΔG°’, and determine if the reaction is exergonic or endergonic. The overall reaction is ______ + _______ → _______ + _________ The overall ΔG°’ is ________ kJ/mol. Therefore, the reaction is _______(exergonic/endergonic)Explain why the glycogen phosphorylase reaction (ΔG°′= 3.1 kJ · mol−1) is exergonic in the cell.