Respuesta :
Comment can be made on how this hydrolysis would compare to that of ATP as When ΔG is more negative, the reaction tends to progress toward products.
The following two forces have an impact on both the hydrolysis of ATP and uridine diphosphate glucose (UDG): enthalpy and entropy, or to put it another way, the change in free energy, or delta G, is the net driving force for these reactions.
ΔG = ΔH - TΔS
The reaction has a tendency to progress toward products when ΔG is more negative.
The exothermic reaction of ATP hydrolysis, in which the high-energy phosphate bonds break and release energy, has a ΔG value of -35.7.
When UDG hydrolysis takes place, the phosphate-glucose bond is also broken, releasing a lot of energy with ΔG= -31.9.
A high GΔ indicates that the products of the reaction are much more stable than the reactants and will be more disordered, resulting in an increase in entropy.
Know more about ATP hydrolysis here: https://brainly.com/question/13056741
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(complete question)
In class, we discussed why ATP was considered a high-energy biomolecule. Its hydrolysis was favorable in terms of four factors: electrostatics, ionization, resonance, and entropy. This same logic can be used to analyze other biomolecules for energy transfer potential. Consider the hydrolysis of uridine phosphoglucose. Comment on how this hydrolysis would compare to that of ATP (consider both sign and magnitude of AG) and how each of the four factors contributes (if at all).
