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3. A muscle can be thought of as a fuel cell, producing work from the metabolism of glucose: C6H12O6+6O26CO2+6H2O. We can calculate changes in enthalpy H , entropy S, and Gibbs free energy G for this reaction using the measured data presented in the table (all data correspond to 1mol of the substance at 298K and 105Pa ). a. If we start with 1mol of glucose, how many moles of O2 are required, and how many moles of CO2 and H2O are produced? b. "Formation" refers to the change in enthalpy or Gibbs free energy when creating 1 mol of the substance from its constituent atoms (here, O2 is considered an "atom"). If the change in enthalpy when "forming" 1mol of glucose is 1273kJ, what is the change in enthalpy when breaking apart 1mol of glucose into its constituent elements? c. Determine the value of H for this reaction for 1mol of glucose. d. What is the total entropy of the reactants? What is the total entropy of the products? Calculate the change in entropy S for the reaction. Has entropy increased or decreased? e. Using H and S, calculate G=HTS for this reaction. Verify that it matches G for the reaction as determined from the values of G in the table. What does your answer indicate about the metabolism of glucose? The maximum amount of work, Wmax, that a muscle can perform (assuming ideal operation according to the laws of thermodynamics) for each mole of glucose that is consumed is given by the value of G calculated in part e. In a real muscle, the metabolism of a glucose molecule results in the synthesis of 38 molecules of ATP; each one of these ATP molecules causes a muscle filament to contract with an average force of about 4pN=41012N acting over a distance of about 11nm=11109m. f. Calculate the actual work done in a real muscle from the metabolism of 1 mol of glucose molecules, Wreal. Then calculate the efficiency of a muscle, Wreal/Wmax, the ratio of the actual work done to the maximum work that is possible