Calculate AG for this reaction under the following conditions: 37°C, pH 7, [Pyruvate] = [CO₂] = 4.0 mM, [OAA] = 2.0 mM, [ATP] = 3.5 mM, [P;] = 5.0 mM, and [ADP] = 1.8 mM. Use 2 signficant figures. AG = i kJ.mol-¹ Under these conditions, the reaction is
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- The phosphoryl group transfer potentials for glucose-1-phosphate and glucose-6-phosphate are 20.9 kJ/mol and 13.8 kJ/mol, respectively. (a) What is the equilibrium constant for the reaction shown below at 25 °C? (b) If a mixture was prepared containing 1 m glucose-6-phosphate and 1 x 10-3 M glucose-1-phosphate, what would be the thermodynamically favored direction for the reaction?Given the following information, calculate the physiological ΔG of the isocitrate dehydrogenase reaction at 25°C and pH 7.0: [NAD+]/[NADH] = 8, [α-ketoglutarate] = 0.1 mM, and [isocitrate] = 0.02 mM. Assume standard conditions for CO2 (ΔG°′ is given in Table). Is this reaction a likely site for metabolic control?Calculate the standard free-energy change of the reaction catalyzed by theenzyme phosphoglucomutase, given that, starting with 20 mM glucose 1-phosphate and no glucose 6- phosphate, the final equilibrium mixture at 25 °C and pH 7.0 contains 1.0 mM glucose 1-phosphate and 19 mM glucose 6-phosphate. Does the reaction in the direction of glucose 6-phosphate formation proceed with a loss or a gain of free energy?
- If the hydrolysis of 1 M glucose 6-phosphate catalyzed by glucose 6-phosphatase has a ΔG′∘ of −11.386 kJ/mol at 25 °C, what percentage of substrate remains once the reaction reaches equilibrium assuming no product was initially present? (Round answer to the nearest whole number)The standard free energy change for the reaction catalyzed by phosphoglucomutase is -7.1kJ/mol, (a) 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, (b) Is the reaction spontaneous under these conditions?If a 0.1 M solution of glucose 1- phosphate at 25 °C is incubated with a catalytic amount of phosphoglucomutase, the glucose 1-phosphate is transformed to glucose 6-phosphate. At equilibrium, the concentrations of the reaction components are Calculate Keq and ΔG′° for this reaction.
- Given the following coupled reactions: phosphoenolpyruvate + H2O → pyruvate + Pi ΔG°'= -61.9 kJ/mol ATP + H2O → ADP + Pi ΔG°'= -30.5 kJ/mol write the overall reaction, calculate the ΔG°’, and determine if the reaction is exergonic or endergonic. The overall reaction is ______ + _______ → _______ + _________ The overall ΔG°’ is ________ kJ/mol. Therefore, the reaction is _______(exergonic/endergonic)The conversion of glucose-1-phosphate to glucose-6-phosphate by the enzyme phosphoglucomutase has a △G°' of -7.6 kJ/mol. Calculate the equilibrium constant for this reaction at 298 K and a pH of 7. (R = 8.315 J/K-mol) A. 0.003 B. 0.047 C. 1.00 D. 21The Keq (25C) of the reaction below is 635.67. Fructose 1,6-biphosphate <-->fructose -6-phosphate + Pi. a) What is the standard Gibbs free energy change for this reaction? b) if the concentrationof fructose 1,6 biphosphate is adjusted to 0.85 M and that of fructose 6 phosphate and phosphate adjusted to 0.055 M, what is the actual free energy change
- Calculate the ΔG for Malate dehydrogenase reaction of CAC if the concentration of oxaloacetate is 1x 10-8 M, malate is 0.2 mM, NAD+ is 10 mM and NADH is 0.1 mM in rat liver mitochondria. ΔGo’ for this reaction is 30 kJ/mole. Please write the units of the final answer and the formula you are using to solve. R = 0.008314kJ/K*mol, T = 298KCalculate the equilibrium concentration of H2O for the following esterification reaction performed in ethanol(C2H5OH) C2H5OH + CH3CO2H ⇌CH3CO2C2H5 + H2O KC= 4.0 At equilibrium: [CH3CO2H] = 0.75 M; [CH3CO2C2H5 ]= 2.2 MAssume that the reaction Arabinose +Pi <> Arabinose-6-P has a delta G of +13.0 kJ/mol and the reaction XTP <> XDP + Pi has a delta G of -25.7 kJ/mol. Calculate the delta G for the combined reaction Arabinose + XTP <> Arabinose-6-P + ADP, in kJ/mol to four significant figures.