Interpretation:
Concept Introduction:
Hydrolysis of ATP produces ADP and phosphate. The standard free energy chain for this hydrolysis reaction is known. If the concentrations of the reactants and products are known, the
Answer to Problem 25.19P
Explanation of Solution
The hydrolysis reaction of ATP is as follows:
The
To calculate the
The concentrations of ATP, ADP, and phosphate are all 1 mM, which is equal to
The value of
Substituting all these values in the equation,
The
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Chapter 25 Solutions
EBK ORGANIC CHEMISTRY
- Glycolysis is the process by which glucose is metabolized to lactic acid according to the equation C6H12O6(aq)2C3H6O3(aq) G=198 kJ at pH 7.0 and 25°C Glycolysis is the source of energy in human red blood cells. In these cells, the concentration of glucose is 5.0103 M, while that of lactic acid is 2.9103 M. Calculate AG for glycolysis in human blood cells under these conditions. Use the equation G=G+RT In Q, where Q is the concentration quotient, analogous to K.arrow_forwardIf glucose, phosphate, and glucose-6-phosphate are combined in concentrations of 4.8, 4.8, and 0.25 mM, respectively, what is the equilibrium constant for the hydrolysis of glucose-6- phosphate at a temperature of 25oC?arrow_forwardCalcium ions bind to a Ca2+-ATPase which has two identical calcium sites, in two stages with apparent equilibrium constants of K, = 3.5 x 105 and K2 = 2 x 106. Determinet for this binding.arrow_forward
- The Keq for the isomerization of glucose-6-phosphate to fructose-6-phosphate is 0.504. What is the ΔG for the reaction if the concentration of glucose-6-phosphate is 0.01 M and the concentration of fructose-6-phosphate is 0.05 M? This reaction is in the cell (this is your temperature = 30 degree celcius ). the answer should be 0.588 kcal/mol - please show all steps I am not sure how to get that answerarrow_forwardFree energy changes under intracellular conditions differ markedly from those determined under standard conditions. ΔG°′ = -32.2 kJ>mol for ATP hydrolysis to ADP and Pi . Calculate ΔG for ATP hydrolysis in a cell at 37 °C that contains [ATP] = 3 mM, [ADP] = 1 mM, and [Pi] = 1 mM.arrow_forwardCalcium ions bind to a Ca2+-ATPase which has two identical calcium sites, in two stages with apparer equilibrium constants of K, = 3.5 x 105 and K2 = 2 x 106. Determine t for this binding. O 2.0 0.5 11 22 1.0arrow_forward
- The value of ΔG° for the conversion of dihydroxyacetone phosphate to glyceraldehyde-3-phosphate (GAP) is 7.53 kJ/mol. If the concentration of dihydroxyacetone phosphate at equilibrium is 2.85 mM, what is the concentration of glyceraldehyde-3-phosphate?Assume a temperature of 25.0 °C.[GAP] = ???? mMarrow_forwardCalculate the equilibrium constant for the phosphorylation of glucose to glucose 6-phosphate at 37.0 °C. 4.74 x10¬3 M-1 eq In the rat hepatocyte, the physiological concentrations of glucose and P; are maintained at approximately 4.8 mM. What is the equilibrium concentration of glucose 6-phosphate (G6P) obtained by the direct phosphorylation of glucose by P;? 8.75 x10-8 [G6P] = M Incorrectarrow_forwardThe equilibrium constant, Keq , for the following reaction is 2 × 105 M: ATP->ADP +HPO2-4 If the measured cellular concentrations are [ATP] = 5 mM, [ADP] = 0.5 mM,and [Pi ] = 5 mM, is this reaction at equilibrium in living cells?arrow_forward
- 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.arrow_forwardAs a result of an experiment following measurements were obtained from a cell: ATP concentration of 0.5 mM, ADP concentration of 0.1 mM, inorganic phosphate (Pi) concentration of 2 mM. Under these conditions calculate the actual free energy (ΔG) of the reaction of hydrolysis of ATP to ADP and Pi. (The standard energy (ΔG°) of ATP = −31 kJ/mol; RT = 2.58 kJ/mol)arrow_forwardFormation of glycerol 3-phosphate is a model reaction for many metabolic processes. The ΔG˚’ for phosphorylating glycerol is +9.2 kJ/mol. Calculate the equilibrium constant for the phosphorylation of glycerol.arrow_forward
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