Part 1 In the overall reaction in aerobic metabolism of glucose (from the H1-Q10
ID: 3505888 • Letter: P
Question
Part 1
In the overall reaction in aerobic metabolism of glucose (from the H1-Q10), 36 mol of ATP is produced from ADP for every 1 mol of glucose oxidized.
a. Calculate the standard state free energy change for the overall reaction when glucose oxidation is coupled to the production of ATP (in kJ/mol).
b. For the capture of the energy released by glycolysis, what is the efficiency of the reaction in terms of the percentage of available free energy captured in ATP? (answer in percentage)
note:- delta G'° for ATP hydrolysis is -30.5 kJ/mol. Please show all work in your response.
Two biochemical reactions have the same Keq (5 x 10^-8 at 25°C). Reaction 1 has a delta H'° of -28 kJ/mol and Reaction 2 has a delta H'° of +28 kJ/mol. The two reactions utilize the same reactants. Your lab partner proposed that you can get more reactants to proceed via Reaction 2 rather than Reaction 1 by lowering the temperature of the reaction.
a. Will this strategy work? Why or why not?
b. How much would the temperature have to be raised or lowered to increase the ratio of the Keqs from 1 to 10?
Explanation / Answer
a.ans.standard state free energy change for the overall reaction when glucose oxidation is coupled to the production of ATP (in kJ/mol).
Now, 36 mol of ATP is produced from ADP for every 1 mol of glucose oxidized.
31 kJ/mol of energy to make each ATP
Thus energy needed to make 36 mol of ATP = 36 * 31 kJ/mol = + 1116 kJ/mol.
b.ans: delta G'° for ATP hydrolysis is -30.5 kJ/mol
Thus G for the overall reaction when glucose oxidation is coupled to the formation of ATP:
(1116 + (-)30.5 KJ/mol=1085.5 kJ/mol
Efficiency (in percentage) = [Energy required]/[Energy available]* 100%
=1,116/-30.5 X 100=-36.59%