In biological cells, the energy released by the oxidation of foods is stored in adenosine triphosphate (ATP or ATP). The essence of ATP's action is its ability to lose its terminal phosphate group by hydrolysis and to form adenosine diphosphate (ADP or ADP³-) ATP+ (aq) + H₂0 (1)→ ADP³- (aq) + HPO2(aq) + H₂O+ (aq) At physiological conditions, pH = 7 and T = 310K (blood temperature), the enthalpy and Gibbs energy of hydrolysis are A,H = -20 and 4₁G = -31, respectively. The hydrolysis of 1.00 mol of ATP, at these conditions, results in the extraction of 31 kJ of energy that can be used to do non-expansion work such as the synthesis of proteins or activation of neurons. mol Calculate the entropy of hydrolysis at pH = 7 and T = 310K
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Given=> pH= 7
Temperature(T) = 310 K
∆rH= -20 kJ/mol
∆rG= -31 kJ/mol
•Here we have to calculate entropy (∆S) of hydrolysis.
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