4. The reaction shown below is part of the glycolytic pathway. The standard free energy change for this reaction is +0.4 kcal/mol. Glucose-6-phosphate (G6P) → Fructose-6-phosphate (F6P) C) Steady-state concentrations of these compounds in the cell (at 25°C) are 0.675 mM G6P and 0.0969 mM F6P. In which direction is this reaction allowed to proceed in the cell? (show calculations)

4. The reaction shown below is part of the glycolytic pathway. The standard free energy change for this reaction is +0.4 kcal/mol. Glucose-6-phosphate (G6P) → Fructose-6-phosphate (F6P) C) Steady-state concentrations of these compounds in the cell (at 25°C) are 0.675 mM G6P and 0.0969 mM F6P. In which direction is this reaction allowed to proceed in the cell? (show calculations)

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter13: Fundamental Equilibrium Concepts

Section: Chapter Questions

Problem 31E: The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what...

See similar textbooks

Similar questions

Why are enzymes important? For example, what is the importance of the enzyme carbonic anhydrase in the body?
The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?
Consider these three reactions as the elementary steps in the mechanism for a chemical reaction.(i) Cl2 (g) + Pt (s) à 2Cl (g) + Pt (s) Ea = 1550 kJ ∆H = – 950 kJ(ii) Cl (g)+ CO (g) + Pt (s) à ClCO (g) + Pt (s) Ea = 2240 kJ ∆H = 575 kJ(iii) Cl (g) + ClCO (g) à Cl2CO (g) Ea = 2350 kJ ∆H = – 825 kJ e. Which reaction intermediate would be considered a catalyst (if any) and why?f. If you were to add 2700kJ of activation energy to the reaction, would you be able to make thereaction reverse itself (i.e. have the products become reactants)? Justify your answer.g. If you were to added a positive catalyst to step (iii) what would the end result be? Justify yourprediction.h. Your friend is looking at your graph and states that she believes that step (ii) is the ratedetermining step. Do you agree with her? Justify your reasoning.
Consider these three reactions as the elementary steps in the mechanism for a chemical reaction.(i) Cl2 (g) + Pt (s) à 2Cl (g) + Pt (s) Ea = 1550 kJ ∆H = – 950 kJ(ii) Cl (g)+ CO (g) + Pt (s) à ClCO (g) + Pt (s) Ea = 2240 kJ ∆H = 575 kJ(iii) Cl (g) + ClCO (g) à Cl2CO (g) Ea = 2350 kJ ∆H = – 825 kJ e. Which reaction intermediate would be considered a catalyst (if any) and why?f. If you were to add 2700kJ of activation energy to the reaction, would you be able to make thereaction reverse itself (i.e. have the products become reactants)? Justify your answer.g. If you were to added a positive catalyst to step (iii) what would the end result be? Justify yourprediction. h. Your friend is looking at your graph and states that she believes that step (ii) is the ratedetermining step. Do you agree with her? Justify your reasoning.
The balanced chemical equation for cellular respiration (oxidation of glucose) is: C6H12O6 + 6O2 → 6CO2 + 6H2O + 38 ATP a. Write the equation for the relationshipbetween the rate of disappearance ofglucose and the rate of formation of ATP. b. Write the equation for the relationshipbetween the rate of formation of carbondioxide and the rate of disappearance of glucose c. In an experiment, 8.8 x1020 molecules of ATP are formed each 6.0 x 10-6s.i. What is the rate of glucose consumption, in molecules/s, during that time? Rate = ii. What is the rate of formation of carbon dioxide, in molecules/s, during that time? Rate=
Draw the reaction coordinate of catalyzed and uncatalyzed reactions. Indicate the substrate (S), product (P), activation energy (∆G+), transition state (T), and free energy change (∆G°).
10. Consider the reaction 2A + B + 24.0 kJ ------ 2 C + D with energy of activation of 55.0 kJ. What is the energy of activation for the reaction 2 C + D --- 2 A + B? A. – 55.0 kJ B. – 31.0 kJ C. 79.0 kJ D. 31.0 kJ E. 24.0 kJ
If you add enzyme to a solution containing only the product(s) of a reaction, would you expect any substrate to form? No, because the enzyme lowers the transition state energy barrier. Yes, because the reaction proceeds backwards until reaching equilibrium. Yes, because the enzyme reduces the standard free energy change for the reaction. No, because enzymes catalyze only the forward reaction. No, because the product inhibits the enzyme.
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 answer
2. For the decomposition of hydrogen peroxide, shown below, the free energy change at 25oC is - 28 kcal/mole. The activation energy is 18 kcal/mole. H2O2 (l) ⟶ 2 H2O (l) + O2 (g) Δ G = - 28 kcal/mole Draw the free energy diagram for the reaction. In addition to labels for the diagram, label the activation energy and the free energy change. The diagram does not need to be precisely proportional, estimates are fine. On the free energy diagram, show how the diagram would change if a catalyst were used (using a dashed line, -----). Is this reaction exergonic or endergonic? Briefly explain.
Reaction 25.1 Sucrose (aq) + H2O (l) ⇄ Glucose (aq) + Fructose (aq) While Reaction 25.1 is spontaneous, it is very slow. Use this information to sketch a reaction diagram for Reaction 25.1. Clearly label the x axis, y axis, products, reactants, and activation energy.
Which of the following is not an example of heterogeneous catalysis? a) 2O3(g) → 3O2(g) has a catalyst of Cl(g) b) CO(g) + 3H2(g) → CH4(g)+H2O(g) has a catalyst of Co(s) c) C2H4(g) + H2(g) → C2H6(g) has a catalyst of Ni(s) d) 2CO(g) + 2NO(g) → 2CO2(g)+N2(g) has a catalyst Rh(s)