The standard free energy change for the hydrolysis of ATP was given in Problem 91. In a
Question:
The standard free energy change for the hydrolysis of ATP was given in Problem 91. In a particular cell, the concentrations of ATP, ADP, and Pi are 0.0031 M, 0.0014 M, and 0.0048 M, respectively.
Calculate the free energy change for the hydrolysis of ATP under these conditions.
Problem 91
Living organisms use energy from the metabolism of food to create an energy-rich molecule called adenosine triphosphate (ATP). The ATP acts as an energy source for a variety of reactions that the living organism must carry out to survive. ATP provides energy through its hydrolysis, which can be symbolized as follows:
where ADP represents adenosine diphosphate and Pi represents an inorganic phosphate group (such as HPO42–).
Calculate the equilibrium constant, K, for the given reaction at 298 K.
The free energy obtained from the oxidation (reaction with oxygen) of glucose (C6H12O6) to form carbon dioxide and water can be used to re-form ATP by driving the given reaction in reverse. Calculate the standard free energy change for the oxidation of glucose and estimate the maximum number of moles of ATP that can be formed by the oxidation of one mole of glucose.
Transcribed Image Text:
ATP(aq) + H₂O (1)
ADP(aq) + P(aq) AGxn=-30.5 kJ
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