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In glycolysis, the reaction of glucose (Glu) to form glucose-6-phosphate (G6P) requires ATP to be present as described by the following equation:
In this process, ATP becomes ADP summarized by the following equation:
Determine the standard free energy change for the following reaction, and explain why ATP is necessary to drive this process:
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Chapter 12 Solutions
Chemistry: Atoms First
- Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.arrow_forwardIn glycolysis, the reaction of glucose (Glu) to form glucose-6-phosphate (G6P) requires ATP to be present as described by the following equation:Glu + ATP⟶G6P + ADP ΔG°298 = −17 kJIn this process, ATP becomes ADP summarized by the following equation:ATP⟶ADP ΔG°298 = −30 kJDetermine the standard free energy change for the following reaction, and explain why ATP is necessary to drive this process:Glu⟶G6P ΔG°298 = ?arrow_forwarda) As stated in question 5a, glucose (C6H12O6(s)) is a source of cellular energy. Calculate the standard free energy for the metabolism of glucose: Given ΔG°C6H12O6(s) = -911kJ/mol; ΔG°O2(g) = 0kJ/mol; ΔG°CO2 = -394kJ/mol; ΔG°H2O(l) = -237kJ/molC6H12O6(s) + 6O2(g) ➝ 6CO2(g) + 6H2O(l) b) Cells couple the hydrolysis of adenosine triphosphate (ATP) into adenosine diphosphate (ADP) andinorganic phosphate (PO43–) to drive chemical reactions (i.e. as a source of chemical energy). The reaction is: ATP(aq) + H2O(l) ➝ ADP(aq) + PO43–(aq) Calculate K for this reaction if ΔG° = –30.5 kJ/mole. c) If all of the energy from glucose metabolism went into ATP synthesis from ADP and inorganicphosphate, how many molecules of ATP could be generated from each molecule of glucose?arrow_forward
- Given that the reaction of 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 3 H20 (g) ΔΗ - - 906 kJ What would AH for NO (g) + ? H20 (g) → NH3 (g) + O2 (g) be? 2. 906 kJ 226.5 kJ -226.5kJ 453 kJarrow_forwardIn glycolysis, glucose is broken down to yield energy. If the equilibrium constant of the isomerization of glucose-6-phosphate to fructose-6-phosphate is 0.5, would this reaction proceed in the forward or reverse direction? What is the free energy of the reaction? Using standard conditions (1 M) as an initial state, what are the equilibrium concentrations?arrow_forwardATP → ADP + Pi (ΔG°’ = -30.5 kJ/mol) In cells, the [ATP] is 0.5 mM, the [ADP] is 4.5 mM, and the [Pi] is 0.65 mM. Calculate the free energy change for ATP hydrolysis under cellular conditions. Enter the numerical value in units of kJ/mol and round to the nearest tenths place.arrow_forward
- Please answer this question. For the aqueous reaction: dihydroxyacetone phosphate ↽−−⇀ glyceraldehyde−3−phosphatedihydroxyacetone phosphate the standard change in Gibbs free energy is Δ?°′=7.53 kJ/molΔG°′=7.53 kJ/mol. Calculate ΔG for this reaction at 298K when [dihydroxyacetone phosphate]=0.100 M and [glyceraldehyde-3-phosphate]=0.00200arrow_forwardThe Keq for the isomerization of glucose-6-phosphate to fructose-6-phosphate is 0.504. What is the ΔG for the reaction if the concentration of glucose-6-phosphate is 0.01 M and the concentration of fructose-6-phosphate is 0.05 M? This reaction is in the cell (this is your temperature = 30 degree celcius ). the answer should be 0.588 kcal/mol - please show all steps I am not sure how to get that answerarrow_forwardGiven that S(g) + O2(g) → SO2(g) A,G° = -300.1 kJ/mol-rxn 2 S(g) + 3 O2(g) → 2 SO3(g) A,G° = -742.1 kJ/mol-rxn calculate AG° of the following reaction: SO2(g) + 1/2 O2(g) → SO3(g) O -1042.2 kJ/mol-rxn O -71.0 kJ/mol-rxn O +2.47 kJ/mol-rxn +1042.2 kJ/mol-rxn O +71.0 kJ/mol-rxnarrow_forward
- a 75 kg adult requires a calorie intake of 2000 Cal of food every 24 hours. The food is metabolized, and the free energy is used to synthesis ATP for useful work. {each Calorie listed on food labels corresponds to 1.0 Cal in biochemical terms}. Assuming that the efficiency of converting food energy into ATP is 50%. Calculate the weight of ATP used by this human in 24 hours and the percentage of the person’s body weight that this represents. {the formula mass of ATP is 505 g/mol and each mole of ATP is equivalence to 7.30 Cal}arrow_forwardThe standard free energy variation, at 25 ºC, for equilibrium: Glucose-6-phosphate (G-6-P) Glucose-1-phosphate (G-1-P) is ΔGº '= + 7280 J / mol. Calculate a) The equilibrium constant of the reaction. b) The real change in free energy when one mole of G-6-P is transformed into G-1-P, both concentrations remaining constant and equal to 10mM and 2 mM respectively.arrow_forwardWhat is the relationship between free-energy change for a reaction and it's equilibrium constant?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
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