Chemistryneed some guidance with this question please. 5). A). Calculate the delta G for the hydrolysis of ATP (reactant) to ADP and inorganicphosphate (Pi) (both products), knowing that the Go for this reaction is -7.3 kcal/mol,and assuming a temperature of 28 °C, and concentrations of ATP, ADP and Pi each equalto 10 mM. B). What would the value for G be at equilibrium? R= 1.99 cal/molI

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5). A). Calculate the delta G for the hydrolysis of ATP (reactant) to ADP and inorganic phosphate (Pi) (both products), knowing that the G" for this reaction is -7.3 kcal/mol, and assuming a temperature of 28 °C, and concentrations of ATP, ADP and Pi each equal to 10 mM. B). What would the value for G be at equilibrium? R= 1.99 cal/mol

5). A). Calculate the delta G for the hydrolysis of ATP (reactant) to ADP and inorganic phosphate (Pi) (both products), knowing that the G" for this reaction is -7.3 kcal/mol, and assuming a temperature of 28 °C, and concentrations of ATP, ADP and Pi each equal to 10 mM. B). What would the value for G be at equilibrium? R= 1.99 cal/mol

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 90QAP: Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of...

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The following reaction occurs in pure water: H2O(l)+H2O(l)H3O+(aq)+OH-(aq) which is often abbreviated as H2O(l)H+(aq)+OH-(aq) For this reaction, G = 79.9 kJ/mol at 25C. Calculate the value of G for this reaction at 25C when [OH] = 0.15 M and [H+] = 0.71 M.
9.96 Most first aid "cold packs" are based on the endothermic dissolution of ammonium nitrate in water: NH4NO3(s)NH4+(aq)+NO3(aq) H= 25.69 kJ A particular cold pack contains 50.0 g of NH4NO3 and 125.0 g of water. When the pack is squeezed, the NH4NO3dissolves in the water. If the pack and its contents are initially at 24.0°C, what is the lowest temperature that this bag could reach? (Assume that the ammonium nitrate solution has a specific heat of 4.25J g-l K-l, and that the heat capacity of the bag itself is small enough to be neglected.)
Wet limestone is used to scrub SO2 gas from the exhaust gases of power plants. One possible reaction gives hydrated calcium sulfite: CaCO3(s) + SO2(g) + H2O() CaSO3 H2O(s) + CO2(g) Another reaction gives hydrated calcium sulfate: CaCO3(s) + SO2(g) + H2O() + O2(g) CaSO4 H2O(s) + CO2(g) (a) Which reaction is more product-favored at equilibrium? Use the data in the table below and any other information needed in Appendix L to calculate rG for each reaction at 25 C. (b) Calculate rG for the reaction CaSO3 H2O(s) + O2(g) CaSO4 H2O(s) Is this reaction product- or reactant-favored at equilibrium?
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Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
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2. The intracellular concentration of glucose-6-phosphate and fructose-6-phosphate are measured inside the cell of a patient and the following values were obtained: (glucose-6-phosphate] = 8 x 10-5 M [fructose-6-phosphate] = 1.5 x 10-5 M %3D %3D Is this reaction at equilibrium? What is the value of Q?. What do you predict the sign for AG will be? Calculate AG for this reaction.
The hydrolysis of ATP to form ADP requires energy to break the bonds initially, but releases moreenergy as bond are remade making the reaction exothermic overall. The Gibbs free energy for thisreaction is -30.5 kJ/mole, meaning that it is also exergonic (ΔG=-). This energy can be used by otherbiological systems if this reaction is coupled with another less favorable one. In this case, the creation ofglucose-6-phosphate, C6H10O9P, this is a pivotal intermediate in many biochemical pathways. PO43- + C6H12O6 ⇌ H2O + C6H10O9P ΔG° = +13.8 kJ/moleATP + H2O ⇌ ADP + PO43- ΔG° = -30.5 kJ/mole A) What is the overall reaction that takes place? B) Calculate the ΔG° for this reaction C) Will this be a successful coupled reaction?
3. For the reaction A B at 300 K and AG°' is -1.2 kcal/mol, in which direction will the reaction go if: a) There is ten times more B than A? b) There is equal amounts of B and A? c) There is ten times more A than B? d) There is 100 times more A than B? e) What is the ratio of B/A at equilibrium? f) If AG is 2.4 kcal/mol, and the concentration of B is 0.5 mM, what is the minimum concentration of A required to make the reaction favorable? g) Overall, what does this question tell us about the concentration of reactants and products as it relates to whether the reaction will go forward or backwards? h) How would the addition of enzyme impact your answers to (a) — (f)?