Chemistry Atoms First2e
2nd Edition
ISBN: 9781947172647
Author: OpenStax
Publisher: OpenStax College
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Chapter 12, Problem 47E
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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In 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°=−17 kJ
In this process, ATP becomes ADP summarized by the following equation:ATP⟶ADP ΔG°=−30 kJ
Determine the standard free energy change for the following reaction, and explain why ATP is necessary to drive this process:Glu⟶G6P ΔG°=?
In 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 = ?
a) 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?
Chapter 12 Solutions
Chemistry Atoms First2e
Ch. 12 - What is a spontaneous reaction?Ch. 12 - What is a nonspontaneous reaction?Ch. 12 - Indicate whether the following processes are...Ch. 12 - A helium-filled balloon spontaneously deflates...Ch. 12 - Many plastic materials are organic polymers that...Ch. 12 - In Figure 12.8 all possible distributions and...Ch. 12 - In Figure 12.8 all possible distributions and...Ch. 12 - How does the process described in the previous...Ch. 12 - Consider a system similar to the one in Figure...Ch. 12 - Consider the system shown in Figure 12.9. What is...
Ch. 12 - Consider the system shown in Figure 12.9. What is...Ch. 12 - Arrange the following sets of systems in order of...Ch. 12 - At room temperature, the entropy of the halogens...Ch. 12 - Consider two processes: sublimation of I2(s) and...Ch. 12 - Indicate which substance in the given pairs has...Ch. 12 - Predict the sign of the entropy change for the...Ch. 12 - Predict the sign of the entropy change for the...Ch. 12 - Write the balanced chemical equation for the...Ch. 12 - Write the balanced chemical equation for the...Ch. 12 - What is the difference between S and S for a...Ch. 12 - Calculate S for the following changes. (a)...Ch. 12 - Determine the entropy change for the combustion of...Ch. 12 - Determine the entropy change for the combustion of...Ch. 12 - Thermite reactions have been used for welding...Ch. 12 - Using the relevant S values listed in Appendix G,...Ch. 12 - From the following information, determine S for...Ch. 12 - By calculating Suniv, at each temperature,...Ch. 12 - Use the standard entropy data in Appendix G to...Ch. 12 - Use the standard entropy data in Appendix G to...Ch. 12 - What is the difference between G and G for a...Ch. 12 - A reaction has H=100kJ/mol and S=250J/mol.K . Is...Ch. 12 - Explain what happens as a reaction starts with G0...Ch. 12 - Use the standard free energy of formation data in...Ch. 12 - Use the standard free energy data in Appendix G to...Ch. 12 - Given: P4(s)+5O2(g)P4O10(s) G=2697.0kJ/mol...Ch. 12 - Is the formation of ozone (O3(g)) from oxygen...Ch. 12 - Consider the decomposition of red mercury(II)...Ch. 12 - Among other things, an ideal fuel for the control...Ch. 12 - Calculate G for each of the following reactions...Ch. 12 - Calculate G for each of the following reactions...Ch. 12 - Calculate the equilibrium constant at 25 C for...Ch. 12 - Determine G for the following reactions. (a)...Ch. 12 - Given that the Gf for Pb2+(aq) and Cl-(aq) is...Ch. 12 - Determine the standard free energy change, Gf, for...Ch. 12 - Determine the standard enthalpy change, entropy...Ch. 12 - The evaporation of one mole of water at 298 K has...Ch. 12 - In glycolysis, the reaction of glucose (Glu) to...Ch. 12 - One of the important reactions in the biochemical...Ch. 12 - Without doing a numerical calculation, determine...Ch. 12 - When ammonium chloride is added to water and...Ch. 12 - An important source of copper is from the copper...Ch. 12 - What happens to G (becomes more negative or more...
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- 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_forwardThe free energy of formation of one mole of compound refers to a particular chemical equation. For each of the following, write that equation. a MgO(s) b COCl2(g) c CF4(g) d PCl5(g)arrow_forwardcells use the hydrolysis of adenosine triphosphate, abbreviated as ATP, as a source of energy. Symbolically, this reaction can be written as ATP(aq) + H2O(l)--> ADP(aq) + H2PO4-(aq). where ADP represent adenosine diphosphate. For this reaction, ΔG∘=-30.5kj/mol. a. If all the free energy from the metabolism of glucose goes into forming ATP from ADP, how many ATP molecules can be produced for every molecule of glucose? C6H12O6 + 6O2 → 6CO2 + 6H2Oarrow_forward
- Cells use the hydrolysis of adenosine triphosphate (ATP) as a source of energy. The conversion of ATP to ADP has a standard free-energy change of -30.5 kJ>mol. If all the free energy from the metabolism of glucose, C6H12O61s2 + 6 O21g2 ¡ 6 CO21g2 + 6 H2O1l2 goes into the conversion of ADP to ATP, how many moles of ATP can be produced for each mole of glucose?arrow_forwardCells use the hydrolysis of adenosine triphosphate (ATP) asa source of energy. The conversion of ATP toADP has a standard free-energy change of -30.5 kJ/mol. Ifall the free energy from the metabolism of glucose, C6H12O6(s) + 6 O2(g)---->6 CO2(g)- + 6 H2O(l) goes into the conversion of ADP to ATP, how many moles ofATP can be produced for each mole of glucose?arrow_forwardAerobic 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° = ?arrow_forward
- 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?arrow_forward1. Describe how you would calculate ∆G0′ for the reaction: glucose+ 6 O2 = 6 CO2 + 6 H2O. If you were told that this reaction is highlyexergonic, what would be the arithmetic sign (negative or positive)of the ∆G0′ you would expect for this reaction?arrow_forwardThe equilibrium constant for a chemical reaction is Kc = 902 at 25°C. What is the standard free energy change, ∆G⁰ for this reaction?arrow_forward
- How and why can virtually all organisms-plants, animals, and bacteria- use the exact same energy molecule, ATP?arrow_forwardConsider the following reaction at 25 °C: 3 Ni(s) + N₂(g) + 3 H₂O(g) → 3 NiO(s) + 2 NH₃(g) If ∆H° = -85.7 kJ/mol and ∆S° = -348.3 J/mol•K, determine the standard free energy for the reaction at 25 °C.arrow_forwardHow do I answer these questions? 1. For a reaction that has ∆H of -30 kJ and ∆S of -62 J/K, estimate at what temperature will the reaction change from spontaneous to non-spontaneous reaction? 2. For a reaction glutamate + NH3 → glutamine + H2O that occurred at 20⁰C, calculate the Gibbs free energy change of the reaction. Given the change in enthalpy of 3103 cal and change of entropy of 3.4 cal/K. 3. For a reaction of conversion of ATP into ADP at 20⁰C, calculate the reaction Gibbs free energy. Given the change in enthalpy is 20.27 Kcal and the change in entropy is 85 cal/Kelvin.arrow_forward
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