Cells use the hydrolysis of ATP as a source of energy. The conversion of ATP to ADP has a standard free energy change of -30.5 kJ/mol. If all the free energy from the metabolism of glucose.
C6H12O6(s)+6O2(g)�¨6CO2(g)+6H2O(l)
goes into the conversion of ADP to ATP, how many moles of ATP can be produced for each mole of glucose?
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G=6(-394)+6(-237)-(-911)= -2875/30,5
Answer. 94,3 mol ATP/mol glucose
You will have to compute the heat of reaction for the reaction using Hess'Law. Then, divide it by 20.5kJ.
You may find the heat of reaction listed under heat of combustion tables.
To determine the number of moles of ATP that can be produced from the metabolism of glucose, we need to first calculate the amount of energy that can be obtained from the metabolism of glucose and then use the standard free energy change of ATP to ADP to convert the energy obtained into moles of ATP.
The balanced chemical equation for the metabolism of glucose is:
C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)
To calculate the energy obtained from the metabolism of glucose, we need to determine the standard free energy change for the balanced equation. This can be done by subtracting the sum of the standard free energy changes of the products from the sum of the standard free energy changes of the reactants.
In this case, we have:
ΔG° = ΣΔG°(products) - ΣΔG°(reactants)
ΔG° = (6ΔG°f(CO2) + 6ΔG°f(H2O)) - (ΔG°f(C6H12O6) + 6ΔG°f(O2))
Where:
ΔG°f is the standard free energy change of formation of each compound.
From standard free energy tables, we can find the following values at 298 K:
ΔG°f(CO2) = -394 kJ/mol
ΔG°f(H2O) = -286 kJ/mol
ΔG°f(C6H12O6) = -1274 kJ/mol
ΔG°f(O2) = 0 kJ/mol (by convention)
Substituting these values into the equation, we have:
ΔG° = (6(-394 kJ/mol) + 6(-286 kJ/mol)) - (-1274 kJ/mol + 6(0 kJ/mol))
ΔG° = (-2904 kJ/mol) - (-1274 kJ/mol)
ΔG° = -2904 kJ/mol + 1274 kJ/mol
ΔG° = -1630 kJ/mol
Now that we have the energy obtained from the metabolism of glucose, we can calculate the number of moles of ATP produced from the conversion of ADP to ATP. The standard free energy change for this reaction is given as -30.5 kJ/mol.
The energy obtained from the metabolism of glucose can be converted to moles of ATP using the following relationship:
ΔG° = ΔG°(ATP to ADP) * n
Where:
ΔG° is the energy obtained from the metabolism of glucose (-1630 kJ/mol)
ΔG°(ATP to ADP) is the standard free energy change for the conversion of ATP to ADP (-30.5 kJ/mol)
n is the number of moles of ATP
Rearranging this equation to solve for n, we have:
n = ΔG° / ΔG°(ATP to ADP)
Substituting the values, we get:
n = -1630 kJ/mol / -30.5 kJ/mol
Calculating the value, we have:
n ≈ 53.44
Therefore, approximately 53.44 moles of ATP can be produced for each mole of glucose metabolized.
A freshman studying medicine at an Ivy League College is a part of his class crew team and exercises regularly. After a particularly strenuous exercise session, he experiences severe cramps in his thighs and pain in his biceps.
Explain the chemical process that occurred in his muscle cells to cause this discomfort.
Explain the chemical reactions that have possibly taken place in his body after the exercise.
Discuss possible treatments for the freshman and how the treatment works chemically.