14 The concentrations of ATP, ADP, and P; differ with cell type. Consequently, the release of free energy from ATP hydrolysisvaries with cell type. Use the table to calculate the free energy change, AG, of ATP hydrolysis in liver, muscle, and brain cells.Cell typelivermusclebrainATP (MM) ADP (MM)ΟΟ3.58.02.6AG of ATP hydrolysis in liver cells:Oliverbrainmuscle1.80.90.7AG of ATP hydrolysis in muscle cells:AG of ATP hydrolysis in brain cells:The expression for free energy change isAG = AG" + RT In (Q)The standard free energy, AG", of ATP hydrolysis is -30.5 kJ · mol¯¹.The product of the gas constant and temperature, RT, is 2.47 kJ - mol¯¹.P₁ (MM)5.08.02.7In which cell type does ATP hydrolysis release the most energy?kJ. mol-1kJ. mol-¹kJ. mol-1

Since conditions inside the cell are different than standard temperature and pressure, biochemists…

Answered: The concentrations of ATP, ADP, and P;…

Biochemistry

9th Edition

ISBN:9781319114671

Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Chapter1: Biochemistry: An Evolving Science

Section: Chapter Questions

Problem 1P

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The pH values of the different compartments are shown below: matrix Intermembrane space Cytosol pH 7.8 – 8.0 pH ~ 7.0pH 7.0 – 7.4 Proton flow through ATP synthase leads to the formation of ATP, a process defined as the binding-change mechanism that was initially proposed by Boyer. Briefly explain Boyer’s binding change mechanism for the ATP synthase.
Free energy changes under intracellular conditions differ markedly from those determined under standard conditions. AG" =-30.5 kJ/mol for ATP hydrolysis to ADP and P,. Calculate AG for ATP hydrolysis in a cell at 37 °C that contains [ATP] =3 mM, [ADP] =1mM, and [P] =1 mM.
Explain the difference between ΔG°’ and ΔG and calculate the free energy (delta G) of hydrolysis of ATP in a rat liver cell in which the ATP, ADP, and Pi concentrations are 3.4, 1.3, and 4.8 mM.
Free 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 3Pi4 = 1 mM.
Assume that in a certain cell, the ratio of products/reactants or Keg = 809.5 (Keq is dimensionless) for the reaction Glucose + 2ATP > Glucose-1,6-diP + 2ADP, at a particular instant, the concentrations of each compound were Glucose =2.4M, ATP =11.1M, ADP -12.8M and G-6-P -28.4M. Calculate the difference (dimensionless) between Keq and the ratio of products/ractants at this instance, in this cell, to five decimal places
Coupled reactions occur where a nonspontaneous reaction is enabled by coupling it to a spontaneous reaction. This approach is common in biological settings. Determine if ATP could be generated by this biochemical reaction. You have calculated that cell potential is +0.637V. An example of a coupled reaction is the first step of glycolysis, the phosphorylation of glucose to form glucose-6-phosphate shown below. kJ/mol The net AG° for this reaction is 1 2 3 н он H. H- H- H H H H 4 6. H. glucose phosphate anion glucose-6-phosphate AG = +14.0 kJ/mol 7 8 9. АТР ADP phosphate anion AG = -30.5 kJ/mol +/- LO
Calculate the actual, physiological ΔG for the reaction at 37 °C, as it occurs in the cytosol of neurons, with phosphocreatine at 4.7 mM, creatine at 1.0 mM, ADP at 0.73 mM, and ATP at 2.6 mM.
In a living cell, this reaction is coupled with the hydrolysis of ATP. Symbolically, this reaction can be represented as ATP(aq) + H2O(l) → ADP(aq) + H2PO4−(aq) (ΔG° = −30.5 kJ/mol) Calculate ΔG° and K at 25°C for the following reaction. glutamic acid(aq) + ATP(aq) + NH3(aq) glutamine(aq) + ADP(aq) + H2PO4−(aq) find ΔG° in kJ and K
In the third step of glycolysis, the given reactions are coupled. reaction 1: fructose-6-phosphate + Pi ⟶ fructose-1,6-bisphosphate + H2O (Δ? = −28 kJ/mol) reaction 2: ATP + H2O ⟶ ADP + Pi (Δ? = +13.8 kJ/mol) Calculate the overall ΔG (kJ/mol) for the coupled reaction.
Suppose the physiological concentrations of ATP, ADP and Pi are as follows in human liver cells. ATP = 3.0 mM ADP = 1.5 mM PO4- = 2.0 mM AG" for ATP hydrolysis is -30.5 kJoules/mole R = 0.008314kJ/K/mol T= 298K How much free energy will be released during ATP hydrolysis of ATP in this condition? Please write the formula you will be using to calculate.
If the DGo for ATP hydrolysis into ADP + inorganic phosphate is -7.3 kcal/mole, and the DGo for sucrose synthesis from glucose + fructose is +5.5 kcal/mole, calculate standard free energy change for the combined reaction of ATP + glucose + fructose g ADP + sucrose + inorganic phosphate. DGo = -12.8 kcal/mole DGo = -1.8 kcal/mole DGo = 0 kcal/mole DGo = +1.8 kcal/mole DGo = +12.8 kcal/mole
The standard free energy change, ΔGº‘ , for the phosphorylation of glucose to glucose-6-phosphate (glucose + Pi yields glucose-6-P) is +3.3 kcal/mol. The standard free energy change, ΔGº‘ , for the hydrolysis of ATP (ATP yields ADP + Pi) is -7.4 kcal/mol. What is the cellular free energy change, ΔG, if the concentration of glucose is 0.005 M, the concentration of ATP is 0.005M, the concentration of glucose-6-phosphate is 0.001M and the concentration of ADP is 0.001M? Cellular temperature = 37 C Gas constant = 0.00198 kilocalories/mol K Temperature = C + Kelvin (C + 273.15) the answer is supposed to be -6.1 kcal/mol but I am not sure how to get there - please show all steps

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