Calculate 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= ikJ.mol-1Under these conditions, the reaction is(Tolerance is +/- 2%)

The thermodynamic function called Gibbs free energy (G), named after Josiah Willard Gibbs, best…

Answered: Calculate AG for this reaction under…

Biochemistry

9th Edition

ISBN:9781319114671

Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Chapter1: Biochemistry: An Evolving Science

Section: Chapter Questions

Problem 1P

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For part (b) of this problem, use the following standard reduction potentials, free energies, and nonequilibrium concentrations of reactants and products: Consider the last two steps in the alcoholic fermentation of glucose by brewer’s yeast: pyruvate + NADH + 2H+ → ethanol + NAD+ + CO2 (a) Do you predict that ∆S° for this reaction is > 0 or < 0? (b) Calculate the nonequilibrium concentration of ethanol in yeast cells, if ∆G = -38.3 kJ/mol for this reaction at pH = 7.4 and 37 °C when the reactants and products are at the concentrations given above. (c) How would a drop in pH affect ∆G for the reaction described in part (b)? (d) How would an increase in intracellular CO2 levels affect ∆G for the reaction in part (b)? (e) How would an increase in intracellular CO2 levels affect ∆G°′ for the reaction in part (b)?
Question 4 Glucose + Pi -> glucose-6-phosphate + H20 deltaG"= -6 kJ/mol ATP + H2O-> ADP + Pi deltaG= -22 kJ/moi What is deltaG" for this reaction ATP + glucose -> ADP + glucose-6-phosphate deltaG"= ? O a. 28 kJ/mol O b. 22 kJimoi Oc 20 kJimrol Od-22 kimol A Ma
Write the coupled reaction that would occur spontaneously for the following pairs of molecules under standard condition: Oxaloaxcetate and NAD+
Derive an Equation that explains the realtionship between kE and kN with respect to the equilibrium constants provided in the reaction scheme provided below. Assume that the enzyme must bind with A before it binds with B. The two reactions are related by the following reaction scheme:provided below.
The reaction quotient is Q=1.6×10-26 Part B What pH is needed to produce this value of Q if the concentration and pressure values are [Br2]=2.50×10−4M , [Br−]=11.65M, [SO42−]=9.50M, and PSO2=3.50×10−5atm ? Express your answer numerically to two decimal places.
What is the Keq of Reaction #3? Show your work & clearly label your answer. Is Reaction #3 favorable under mammalian cellular conditions when the concentration of dGTP is 0.2 M, dCMP is 20 mM, dGMP-dCMP is 7 mM, and PPi is 10 mM? Use △G to support your answer.
P2.5
Complete the balanced equation for the overall reaction by selecting an answer choice in the brackets. Sucrose + [2 Pi, 4Pi]+[4 ADP, 2 ADP, 4 ATP, 2ATP]+[2 NAD+, 4 NAD+, 6 NAD+]+[H2O, 5 H2O, 3 H2O] --> [2 cirate, 2 oxaloacetate, 2 pyruvate, 2 acetyl-coA]+[4 ADP, 2 ADP, 4 ATP, 2ATP] + [2 NAD+, 4 NAD+, 6 NAD+] + [2H+, 8H+, 6 H+, 4 H+, 10 H+] Does the commercial process require aerated culture medium—that is, is this a fermentation or an aerobic process? A. a fermentation process, because A. niger cells must use O2O2 to continuously regenerate NAD+ B. an aerobic process, because A. niger cells must use O2O2 to continuously regenerate NAD+ C. a fermentation process, because A. niger cells cannot use O2O2 to continuously regenerate NAD+ D. an aerobic process, because A. niger cells cannot use O2O2 to continuously regenerate NAD+
Consider the following reaction at 25°C with the ΔG°’ = +1800 J/mol for the forward reaction.The molar concentrations at the beginning of the reaction were [A] = 19 mM and [B] = 10 mM.After 1 hour, the concentrations were [A] = 16 mM and [B] = 13 mM. Calculate the ΔG of the reaction at the 1 hour timepoint. Please round to 1 decimal point.Gas constant = 8.315 J/mol K
The formation constants at 25°C for Fe(CN)4-6 and Fe(EDTA)2– are 1.00 x 1037 and 2.10 x 1014, respectively. Answer the questions below. 1) Calculate K under standard conditions for the reaction Fe(EDTA)2−(aq) + 6CN−(aq) ----> Fe(CN)4−6(aq) + EDTA4−(aq) 2) Calculate ΔG° for the reaction. (kJ/mol)
Determine whether the following reactions will be spontaneous under standard biochemical conditions. Include calculations for Delta G in your answer. Use Table 13-7 in your textbook to help you.a) 2NADH + 2H+ + O2 --> 2NAD+ + 2H2Ob) Malate + FAD --> Oxaloacetate + FADH2c) Pyruvate + H2S --> Lactate + S
Calculate the standard free-energy change, deltaG'o, for the reaction in which acetaldehyde is reduced by the biological electron carrier NADH in the reaction acetaldehyde + NADH + H+ → ethanol + NAD+. Then calculate the actual free-energy change, deltaG, when the acetaldehyde is 1.51 M, the NADH is 1.02 M, the ethanol is 0.13 M and the NAD+ is 0.19 M, at 33.35oC and pH = 7. Give the actual free-energy change in kJ/mol to one decimal place. See Table 13-7b for the E'o values. please provide comprehensive explaination with each step.

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Calculate 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