Concept explainers
Interpretation:
The feasibility of the dimerization of protein at
Concept introduction:
The spontaneity of areaction is determined by Gibbs free energy. The mathematical equation is expressed as follows:
Here,
If
If
If
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Chemistry
- 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_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_forwardThe enzyme aldolase catalyzes the conversion of fructose-1,6-diphosphate (FDP) to dihydroxyacetone phosphate (DHAP) and glyceraldehyde-3-phosphate (G3P). The reaction is FDP → DHAP + G3P with A,G°(298.15 K) = 23.8 kJ mol In red blood cells, the concentrations of these species are [FDP] = 35 µM, [DHAP] = %3D 130 µM, and [G3P] = 15 µM. Remember that 1.0 µM 1.0 x 10-6 mol L-1. The standard state for reactions in solution can be taken to be 1.0 mol L-1. (a) Calculate A,G in a red blood cell at 25°C. (Note: A,G is not the same as A,Gº, as the substances in the blood cell are not in standard condi- tions). (b) Will the reaction occur spontaneously in the blood cell at this temperature?arrow_forward
- The 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_forwardA student determines the value of the equilibrium constant to be 3.67×10-18 for the following reaction. Fe3O4(s) + 4H₂(g) →→→3Fe(s) + 4H₂O(g) Based on this value of Keq: AGO for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 1.67 moles of Fe3O4(s) at standard conditions at 298K. AGᵒrxn KJarrow_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→G6) + ADP AG° = - 17KJ In this process, ATP becomes ADP summarized by the following equation: ATP→ ADP A G° =- 30 kJ What is the standard free energy change for the following reaction: Glu →G6P AG° =? A 17 k) B) -13 k) c) 13 kJ -17 kJarrow_forward
- Which of the following reactions corresponds to the reaction corresponding to a free energy of formation, ΔGfo? Group of answer choices.... 6 C(l) + 11 H2(g) + 11 O(g) → C6H22O11(s) P(g) + 4 H(g) + Br(g) → PH4Br(l) 6 C(s) + 6 H(g) → C6H6(l) 1/2 N2(g) + O2(g) → NO2(g) 2 N2(g) + 4 H2(g) + 3 O2(g) → 2 NH4NO3(s)arrow_forwardFrom the reaction below, calculate the free energy of formation for CH4(g) at 25°C, if ΔGfo(C3H6(g)) is 104.514 kJ/mol.3CH4(g) ↔ C3H6(g) + 3H2(g) ΔGo = 256.883 kJ/mol ΔGo = -50.790 kJ ΔGo = -152.369 kJ ΔGo = 50.790 kJ ΔGo = 152.369 kJarrow_forwardPlease 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_forward
- 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 = ?arrow_forward9. For the reaction: 2 CH,OH(g) + H2(g) - C2H(g) + 2 H2O(g) a) Calculate AG° for this reaction using free energy values in your text book. b) Calculate AG at standard temperature when the pressure of CH3OH is 4.97 atm, H2 is 3.56 atm, C2H6 is 4.85 atm, and H20 is 2.18 atm. c) Calculate Kp for this reactionarrow_forwardCalculate the free-energy change for the following reaction using the ΔGf° values in the appendix:C12H22O11 (s) + 12 O2 (g) → 12 CO2 (g) + 11 H2O (l)arrow_forward
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