How Many Moles of ATP Can Be Produced from One Mole of Glucose?

[grumpyasian]

Homework Statement

assuming that all the energy released by the oxidation of one mole of glucose to carbon dioxide and water can be stored in the form of ATP, how many moles of ATP can be theoretically produced from ADP at 37 C? Use delta G since it tells you how much work a reaction could do or requires. ( P is a phosphate group, ADP is adenosine dephosphate, ATP is adenosine triphosphate)

Homework Equations

ADP ^-3 + H ^+ + P--> ATP ^-4 + H20 delta G= 31.4 KJ/mol

The Attempt at a Solution

I don't know how to start solving it, help

 

[Borek]

You will need delta G for glucose oxidation. Not knowing the circumstances it is hard to tell if you are expected to find it in tables or calculate from some other data.

 

[grumpyasian]

delta G is -916 kj/mol for Glucose. i don't know where to start or how to...help?

 

[Borek]

Now it is a simple energy balance - amount of energy produced from glucose oxidation can't be higher than amount of energy stored in ATP.

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[DeeNos]

!

As a scientist, it is important to understand the fundamental principles and equations involved in a problem before attempting to solve it. In this case, we are looking at the theoretical production of ATP from the oxidation of glucose. The equation for this reaction is:

C6H12O6 + 6O2 → 6CO2 + 6H2O + energy (as ATP)

From this equation, we can see that for every mole of glucose oxidized, 6 moles of ATP are produced. However, the question also mentions using the delta G value, which is the change in free energy during a reaction. The equation given is for the conversion of ADP to ATP, so it is not directly related to the oxidation of glucose.

To calculate the maximum number of moles of ATP produced from ADP, we need to use the equation:

ΔG = -nFE

where ΔG is the change in free energy, n is the number of moles of electrons transferred, F is Faraday's constant (96,485 C/mol), and E is the potential difference in volts. In this case, we are interested in the potential difference for the conversion of ADP to ATP, which can be found in a table of standard electrode potentials. The value for this reaction is -31.4 kJ/mol, as given in the problem statement.

Now, we need to determine the number of moles of electrons transferred in this reaction. Looking at the equation given, we can see that for each ATP molecule produced, one phosphate group (P) is added to ADP, and one H+ ion is consumed. This means that n = 2 moles of electrons transferred.

Plugging in all the values into the equation, we get:

-31.4 kJ/mol = -2 mol x 96,485 C/mol x E
E = 0.000162 V

This value represents the potential difference at standard conditions (25°C, 1 atm pressure, 1 M concentration). To calculate the potential difference at 37°C, we can use the Nernst equation:

E = E° - (RT/nF)ln(Q)

where E is the potential difference at a given temperature, E° is the standard potential difference, R is the gas constant (8.314 J/mol·K), T is the temperature in Kelvin, n is the number of moles of electrons transferred, F is Faraday