3. Consider the following reactions: ATP + H20 --> ADP + Pi AGO' = -30.5 kJ/mol 1,3-biphosphoglycerate + H20 ----> phosphoglycerate + Pi AGO' = -49.4 kJ/mol a. How many moles of ATP could be produced under standard conditions from the oxidation of one mole of 1,3-biphosphoglycerate assuming 27.3% efficiency? b. Calculate the AGO' for the reaction: phosphoglycerate + ATP ----> 1,3-biphosphoglycerate + ADP

3. Consider the following reactions: ATP + H20 --> ADP + Pi AGO' = -30.5 kJ/mol 1,3-biphosphoglycerate + H20 ----> phosphoglycerate + Pi AGO' = -49.4 kJ/mol a. How many moles of ATP could be produced under standard conditions from the oxidation of one mole of 1,3-biphosphoglycerate assuming 27.3% efficiency? b. Calculate the AGO' for the reaction: phosphoglycerate + ATP ----> 1,3-biphosphoglycerate + ADP

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter23: Organic Polymers, Natural And Synthetic

Section: Chapter Questions

Problem 46QAP: Glycolysis is the process by which glucose is metabolized to lactic acid according to the equation...

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The G° for the conversion of glucose 6-phosphate (G6P) to fructose 6-phosphate (F6P) is +1.7 kJ/mole. In a particular human cell the concentration G6P is 8.0 µM and the concentration F6P is 1.0 µM. Calculate the G of the reaction as it occurs in this cell at 37°C?
Assume that in a certain cell, the ratio of products/reactants or Keq = 614.9 (Keq is dimensionless) for the reaction Glucose + ATP <> Glucose-6-P + ADP, at a particular instant, the concentrations of each compound were Glucose =4.3M, ATP =10.5M, ADP =17.3M and G-6-P =23.5M. Calculate the difference (dimensionless) between Keq and the ratio of products/ractants at this instance, in this cell, to five significant figures.
Dependence of ΔG on pH, he free energy released by the hydrolysis of ATP under standard conditions at pH 7.0 is -30.5 kJ/mol. If ATP is hydrolyzed under standard conditions but at pH 5.0, is more or less free energy released? Explain
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?
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° = ?
Suppose you determined experimentally that a cellular transport system for glucose, driven by symport of Na+, could accumulate glucose to concentrations 25 times greater than in the external medium, while the external [Na+] was only 10 times greater than the intracellular [Na+]. Would this violate the laws of thermodynamics? If not, how could you explain this observation?
Q26-C (i) Explain pyrolysis process.
Energy from ATP hydrolysis drives many nonspontaneouscell reactions:AT P⁴⁻(aq) +H₂O(l) ⇌ADP³⁻(aq) +HPO₄²⁻(aq) +H(aq) ΔG°'=-30.5 kJ Energy for the reverse process comes ultimately from glucose metabolism:C₆H₁₂O₆(s)+ 6O₂g) →6CO₂(g) +6H₂O(l)(a) Find K for the hydrolysis of ATP at 37°C.(b) Find ΔG'°ᵣₙₓ for metabolism of 1 mol of glucose. (c) How many moles of ATP can be produced by metabolism of1 mol of glucose? (d) If 36 mol of ATP is formed, what is the actual yield?
This is a thermodynamically unfavorable process, with ΔG°' = +13.7 kJ/mol. In a liver cell at 37°C the concentrations of both phosphate and glucose are normally maintained at about 6.2 mM each, while the glucose-6-phosphate is around 2.1 mM . Calcaulate the Gibb's Free Energy (ΔG) of this reaction occuring in the liver
Double-helix-formation entropy. For double-helix forma- tion, DG can be measured to be 254 kJ mol?1 (213 kcal mol?1) at pH 7.0 in 1 M NaCl at 258C (298 K). The heat released indicates an enthalpy change of 2251 kJ mol?1 (260 kcal mol?1). For this process, calculate the entropy change for the system and the entropy change for the surroundings.
The Caloric Value of carbohydrates in 1g is: 4 5 1 9
At a steady state in the living cell, (ATP) = 10-3M and (ADP) = 10-4 M. The maximum(equilibrium) value of the ratio (glycerol-1-P)/(glycerol) is observed to be 770 at 25 Cand pH=7.a. Calculate K and rG for the reaction.b. Using the value of rG for the reaction ADP + Pi →ATP + H2O, together with the answer topart (a), calculate rG and K for the reaction: glycerol + phosphate→ glycerol-1-phosphate+ H2O