Wheeler and Mathews (J. Biol. Chem. 287:31218–31222 (2012)) reportedthe NAD+ and NADH concentrations in yeast mitochondria as 20 mM and0.3 mM, respectively. Consider the malate dehydrogenase reaction, which is part of the citric acid cycle:malate + NAD+ → oxaloacetate + NADH + H+ ΔG∘' = +29.7 kJ/molIf malate concentration in yeast mitochondria is 0.4 mM, what is the maximum concentration of oxaloacetate needed to make the reaction exergonic at pH 7.0 and 37°C?

Wheeler and Mathews (J. Biol. Chem. 287:31218–31222 (2012)) reportedthe NAD+ and NADH concentrations in yeast mitochondria as 20 mM and0.3 mM, respectively. Consider the malate dehydrogenase reaction, which is part of the citric acid cycle:malate + NAD+ → oxaloacetate + NADH + H+ ΔG∘' = +29.7 kJ/molIf malate concentration in yeast mitochondria is 0.4 mM, what is the maximum concentration of oxaloacetate needed to make the reaction exergonic at pH 7.0 and 37°C?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 78QAP

See similar textbooks

Similar questions

Aerobic respiration links the oxidation of glucose with the production of ATP form ADP.Given the following thermodynamic data, C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) ΔrH° = −2803 kJ/mol-rxn ATP + H2O(l) → ADP + HPO42-(aq) ΔrH° ≈ −24 kJ/mol-rxn calculate the enthalpy of reaction for the aerobic production of 25 ATP shown below.C6H12O6(s) + 6O2(g) + 25ADP + 25HPO42-(aq)→ 6CO2(g) + 25ATP + 31H2O(l) ΔrH° = ?
The efficiency of striated muscle is typically 37%, that is, the muscle converts 37% of the chemical energy reaching it (in the form of glucose) into mechanical work, converts the remainder into waste heat. Your biceps muscle performs mechanical work at the rate of 50 W. (a) What is the rate at which it consumes chemical energy? (b) What is the rate at which it produces waste heat? (c) Given that the oxidation of glucose yields 3.70 103 kcal/kg, what is the rate at which this muscle consumes glucose?
Consider the reaction in the attached image: a. The standard Gibbs free energy (ΔfG˚) for this reaction (up to two decimal places) is ____________ kJ/mol. b. If the concentration of AMP is adjusted to 1.5M and that of adenosine and phosphate is adjusted to 0.50M, the actual free energy change (ΔG) (up to two decimal places) is equal to ___________ kJ/mol.
Glycolysis is the process by which glucose is metabolized to lactic acid according to the equation C6H12O6(aq)2C3H6O3(aq) G=198 kJ at pH 7.0 and 25°C Glycolysis is the source of energy in human red blood cells. In these cells, the concentration of glucose is 5.0103 M, while that of lactic acid is 2.9103 M. Calculate AG for glycolysis in human blood cells under these conditions. Use the equation G=G+RT In Q, where Q is the concentration quotient, analogous to K.
1.) Calculate ΔG'° for a reaction proceeding under biochemical standard conditions with a K'eq of 2.32. Give your answer in units of kJ/mol, but do not include the units as part of your answer (give the number only) 2.) What is the ΔG in kJ/mol for the reaction characterized in the previous question if the temperature is increased to 30°C and Q = 3.1? Again, please only give the numerical answer, do not include units.
In liver cells the usual concentrations of some solutes are: [ATP] = 3.4 mM; [ADP] = 1.3 mM and [Pi] = 5 mM. Calculate the real variation of energy free by hydrolyzing ATP in the liver into ADP and Pi. a) at 25ºC b) at 37ºC (ΔGº’ ATP hydrolysis = -30.5 kJ / mol)
The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is q of rxn?
Calculate the equilibrium constant at 37oC for the reactionGlucose + 6O2 + 36ADP + 36Phospate → 6CO2+ 42H2O +36ATP ... ... ...Entropy change of Go= − 423 kcal/mole of Glucose
Would you expect the entropy of 1.0 M C12H22O11(aq) to be greater than, less than or equal to the entropyof 10.0 M C12H22O11(aq)? Explain your reasoning.
What is the entropy at SATP of a reaction where ∆Hºrxn=12.5 kJ and Keq=32.1?
Explain the difference between Kf and Ksp.
Use bond enthalpies and mean bond enthalpies to estimate (a) the enthalpy of the anaerobic breakdown of glucose to lactic acid in cells that are starved of O2, C6H12O6(aq) → 2 CH3CH(OH) COOH(aq), and (b) the enthalpy of combustion of glucose (Ignore the contributions of enthalpies of fusion and vaporization). NOTE: When using bond enthalpies alone to estimate reaction enthalpies, it is not possible to include condensed phase interactions, so the estimates are for gas-phase reactions.