Question 2, continued In a typical muscle cell at rest the following concentrations are observed Metabolite Equilibrium Concentration mM ATP 8.0 ADP 0.02 3.0 Creatine 3.0 Creatine Phosphate 26.0 c)Calculate the AG for creatine phosphate formation in these cells at 37%C. Show all work. Under the above cellular conditions, is the synthesis of creatine phosphate spontaneous? R=1.987×103 kcal mork T=273+37=310K △G=△G°+RTm/ roducts reactants △G=2.0cm:+1.987×103klmk-×310Kxby20.022601 [3080] AG=-0.36 kcal/mol Under the above cellular conditions, the synthesis of creatine phosphate is spontaneous d) Briefly explain why the AG you calculated is different from the AG given for the reaction under standard conditions AG describes the free energy of the reaction under standard conditions when the concentrations of the reactants and products are 1M. AG is different from AG, because the reaction is not being carried out under standard conditions e)What would happen to the spontaneity of the reaction if the equilibrium [ADP] was raised by an order of magnitude, i. e from 0.02mM to 0.2mM? What does this suggest about the importance of maintaining a high ratio of atP to ADP in the cell? If the equilibrium concentration of ADP were to increase in the cell by an order of magnitude, the synthesis of creatine phosphate would becoine non-spontaneous as the AG would be positive. This illustrates the importance of maintaining the proper balance of various metabolites within the cell, as small changes in concentration of just a few metabolites can have a significant impact upon the behavior and function of the cell 7012Fall20037.012 Fall 2003 Question 2, continued In a typical muscle cell at rest the following concentrations are observed: Metabolite Equilibrium Concentration (mM) ATP 8.0 ADP 0.02 Pi 3.0 Creatine 3.0 Creatine Phosphate 26.0 c) Calculate the ΔG for creatine phosphate formation in these cells at 37°C. Show all work. Under the above cellular conditions, is the synthesis of creatine phosphate spontaneous? R = 1.987×10-3 kcal mol-1 K-1 T = 273 + 37 = 310 K € ΔG = ΔGo + RT ln [products] [reactants]       ΔG = kcalmol 2.0 −1 +1.987 ×10−3 kcalmol−1 K−1 × 310K × ln [0.02][26.0] [3.0][8.0]       ΔG = -0.36 kcal/mol Under the above cellular conditions, the synthesis of creatine phosphate is spontaneous. d) Briefly explain why the ΔG you calculated is different from the ΔG° given for the reaction under standard conditions. ΔG° describes the free energy of the reaction under standard conditions when the concentrations of the reactants and products are 1M. ΔG is different from ΔG°, because the reaction is not being carried out under standard conditions. e) What would happen to the spontaneity of the reaction if the equilibrium [ADP] was raised by an order of magnitude, i.e. from 0.02mM to 0.2mM? What does this suggest about the importance of maintaining a high ratio of ATP to ADP in the cell? If the equilibrium concentration of ADP were to increase in the cell by an order of magnitude, the synthesis of creatine phosphate would become non-spontaneous as the ΔG would be positive. This illustrates the importance of maintaining the proper balance of various metabolites within the cell, as small changes in concentration of just a few metabolites can have a significant impact upon the behavior and function of the cell