pls show complete solution 1. The phosphorylation of glucose in the cell is coupled to the hydrolysis of ATP; that is, part ofthe free energy of ATP hydrolysis is used to phosphorylate glucose. The reactions involved areshown as follows:glucose + PiATP + H2Oglucose 6-phosphate + H₂OADP + PiAGº' = 13.8 kJ/molAG-30.5 kJ/molSum: glucose + ATPglucose 6-phosphate + ADPCalculate the Keq for the overall reaction of glucose phosphorylation.2. Consider the oxidation of malate to oxaloacetate:malate + NAD+ -oxaloacetate + NADH + H+Would you expect this reaction to proceed under standard condition and assuming that theappropriate enzyme is present? Support your answer with calculation. Hint: The followingreactions are involved in this conversion:oxaloacetate + 2H + + 2e*NAD++ H+ + 2emalateE°' = -0.166 VNADHE°' = -0.320 V

Approach to solving the question: Detailed explanation:1.given reactions: Glucose + Pi -->…

Answered: 1. The phosphorylation of glucose in…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 53QRT

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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.)
The overall reaction that occurs when sugar is metabolized is C12H22O11(s)+12O2(g)12CO2(g)+11H2O(l) For this reaction, H° is -5650 kJ and G° is -5790 kJ at 25°C. (a) If 25% of the free energy change is actually converted to useful work, how many kilojoules of work are obtained when one gram of sugar is metabolized at body temperature, 37°C? (b) How many grams of sugar would a 120-lb woman have to eat to get the energy to climb the Jungfrau in the Alps, which is 4158 m high? ( w=9.79103mh, where w= work in kilojoules, m is body mass in kilograms, and h is height in meters.)
Explain in your own words what is meant by the term entropy. Explain how both matter spread and energy spread are related to the concept of entropy.
Define the standard enthalpy of formation. What are standard states for elements and for compounds? Using Hess's law, illustrate why the formula Hreaction=npHf(products)nfHf(reactants) works to calculate H for a reaction.
Given the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g) Substance Hf(kJ/mol) S(J/molK) A(g) 191 244 B(g) 70.8 300 C(g) 197 164 a 956 kJ b 956 kJ c 346 kJ d 346 kJ e 1.03 103 kJ
Consider the following reactions at 25°C: C6H12O6(aq)+6O2(g)6CO2(g)+6H2O G=2870kJ ADP(aq)+HPO42(aq)+2H+(aq)ATP(aq)+H2OG=31kJ Write an equation for a coupled reaction between glucose, C6H12O6, and ADP in which G=390kJ .
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
Use standard entropies and heats of formation to calculate G f at 25C for (a) cadmium(II) chloride (s). (b) methyl alcohol, CH3OH(l). (c) copper(I) sulfide (s).
When glucose, C6H12O11, is metabolized to CO2 and H2O in living systems, the first step is the conversion of glucose to glucose-6-phosphate. glucose+H3PO4glucose-6-phosphate+H2OG=13.4kJ This nonspontaneous reaction can be made to proceed by coupling it with the hydrolysis of ATP. ATP+H2OADP+H3PO4G=31.0kJ (a) Write an equation for the coupled reaction and calculate G°. (b) Estimate the number of moles of ATP required to convert glucose to glucose-6-phosphate.
Given that H f for HF(aq) is -320.1 kJ/mol and S for HF(aq) is 88.7 J/mol K, find Ka for HF at 25C.
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
When ammonium chloride is added to water and stirred, it dissolves spontaneously and the resulting solution feels cold. Without doing any calculations, deduce the signs of G, H, and S for this process, and justify your choices.

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