Use the following information corresponding to 1 Molar concentrations of reactants and products for Questions 7-12. Glycerol + ATP ADP+ 3-Phosphoglycerate: AH = -63.39 kJ/mol and AS = -0.1255 kJ/molk. At 25 °C, calculate the standard free energy change for the reaction as written. Type your answer...

The 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)

Use the following information corresponding to 1 Molar concentrations of reactants and products for Questions 7 -12.  Glycerol + ATP  → ADP + 3-Phosphoglycerate: ΔHo’ = -63.39 kJ/mol and   ΔS o’ = -0.1255  kJ/molK.  At what temperature (if any) is this reaction  endergonic?  Report your answer in Kelvin using inequality signs with out and extra spaces added in. For example T=100.00K T>100.00K T<100.00K T</=100.00K  less than or equal to T>/=100.00K   greater than or equal to

Use the following information corresponding to 1 Molar concentrations of reactants and products for Questions 7 -12.  Glycerol + ATP  → ADP + 3-Phosphoglycerate: ΔH = -63.39 kJ/mol and   ΔS = -0.1255  kJ/molK.  Based on the information given above, Which of the following statements regarding this folding process are correct?   Use the following information corresponding to 1 Molar concentrations of reactants and products for Questions 7 -12.  Glycerol + ATP  → ADP + 3-Phosphoglycerate: ΔH = -63.39 kJ/mol and   ΔS = -0.1255  kJ/molK.  Based on the information given above, Which of the following statements regarding this folding process are correct?   endothermic exothermic Enthapically driven Entropically driven Enthalpically opposed Entropically opposed at equilibrium Exergonic for all temperatures Endergonic for all temperatures

Use the following information corresponding to 1 Molar concentrations of reactants and products for Questions 7 -12.  Glycerol + ATP  → ADP + 3-Phosphoglycerate: Δ = -63.39 kJ/mol and   ΔS  = -0.1255  kJ/molK.  At 37 oC, calculate the standard free energy change for the reaction as written.

Use the following information corresponding to 1 Molar concentrations of reactants and products for Questions 7 -12.  Glycerol + ATP  → ADP + 3-Phosphoglycerate: ΔH = -63.39 kJ/mol and   ΔS  = -0.1255  kJ/molK.  At what temperature is this reaction at equilibrium? Report your answer in Kelvin.

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?

At 25 oC, calculate the standard free energy change for the reaction as written.  1,3-Bisphosphoglycerate + ADP →ATP + 3-Phosphoglycerate + H+: ΔH = 41.02 kJ/mol and   ΔS  = 0.3030  kJ/molK.  All answers should be in units of kJ/mol

For the triose phosphate catalyzed reaction: dihydroxyacetone phosphate <--> glyceraldehyde-3-phosphate the standard change in Gibbs free energy is ΔG'º=7.53 kJ/mol. Calculate the ΔG for this reaction at 298K when the concentration of dihydroxyacetone phosphate is 0.161 M and the concentration of glyceraldehyde-3-phosphate is 0.00163 M.

I need help with calculating  You wish to determine if a certain biochemical reaction will be spontaneous. You have determined the following for this reaction: G(products) = 48 kCal/mole G(reactants) = 12 kCal/mole You have also determined that there are 4 molecules of ATP that can be used in this reaction (ΔG for one ATP = -7.3 kCal). What the ΔG for this biochemical reaction using this level of ATP hydrolysis?  ....     kCal/mol Will this reaction proceed spontaneously with this level of ATP hydrolysis?   ....