Calcium ions bind to a Ca2+-ATPase which has two identical calcium sites, in two stages with apparent equilibrium constants of K, = 3.5 x 10° and K2 = 2 x 106. Determine t for this binding. %3D
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- In liver cells the usual concentrations of some solutes are: [ATP] = 3.4 mM; [ADP] = 1.3 mM and [Pi] = 5 mM. Calculate the real variation of energy free by hydrolyzing ATP in the liver into ADP and Pi. a) at 25ºC b) at 37ºC (ΔGº’ ATP hydrolysis = -30.5 kJ / mol)Calculate the equilibrium constant at 37oC for the reactionGlucose + 6O2 + 36ADP + 36Phospate → 6CO2+ 42H2O +36ATP ... ... ...Entropy change of Go= − 423 kcal/mole of GlucoseThe 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.
- In glycolysis, glucose is broken down to yield energy. If the equilibrium constant of the isomerization of glucose-6-phosphate to fructose-6-phosphate is 0.5, would this reaction proceed in the forward or reverse direction? What is the free energy of the reaction? Using standard conditions (1 M) as an initial state, what are the equilibrium concentrations?The value of ΔG° for the phosphorylation of glucose in glycolysis is 13.8 kJ/mol. What is the value of the equilibrium constant for the reaction at 25.0°C?What is the correct Ksp expression for Lead(II) Chloride dissolving in water?
- The equilibrium constant Kc for the reaction fructose-1,6-diphosphate ⇋ glyceraldehyde-3-phosphate + dihydroxyacetone phosphate is 8.9 x 10-5 M at 250C and the behavior is assumed to be ideal?The standard state free energy of hydrolysis of acetyl phosphate is ΔGo= -42.3 KJ/mol. T=20 degrees C Calculate the free energy change for the acetyl phosphate hydrolysis in a solution of 3.5 mM acetate, 3.5mM phosphate (Pi), and 4.00 nM acetyl phosphate.Concentration of ATP: 5.0*10-3 Concentration of ADP: 5.0*10-4 Concentration of Phosphate (Pi): 1.0*10-3 ∆G ̊= -31 kJ/mol at 298 K for the hydrolysis of ATP. Calculate the Q and ∆G for ATP hydrolysis.
- Consider the reaction CO (g) + 2 H2 (g) = CH3OH (l)Thermodynamic Quantities for Substances at 25°C delta H°f (kJ/mol) delta G°f (kJ/mol) S°(J/mol*K) CO (g) -110.5 -137.2 197.5 H2 (g) 0 0 130.6 CH3OH -201.2 -161.9 238 17(a) Use the data above to calculate deltaH° and delta S° at 25°C. (17b) What is K at 25°C? (17c) What is delta G° at 1000°C?The standard free energy change for the reaction catalyzed by phosphoglucomutase is -7.1kJ/mol, (a) Calculate the equilibrium constant for the reaction, (b) Calculate ΔG at 37°C when the concentration of glucose-1-phosphate is 1-mM and the concentration of glucose-6-phosphate is 25-mM, (c) Is the reaction spontaneous under these conditions?2c2hh6g+7O2g arrows 4co2g+6h2og symbolic expression for the eqilibrium for reaction