Respuesta :
Answer:
ΔG for overall reaction : -21.3 kJ
Explanation:
Reaction of the conversion of glycerol to glycerol-3-phosphate is unfavorable and thus is coupled with second reaction that involves the conversion of ATP to ADP which is highly energetically favorable.
Reaction 1: Glycerol + HPO₄²⁻ ⇒ Glycerol-3-phosphate + water
Reaction 2: ATP + H₂O ⇒ ADP + HPO₄²⁻ + H⁺
ΔG for reaction 1 : 9.2 kJ (non-spontaneous : Positive value)
ΔG for reaction 2 : -30.5 kJ (spontaneous : Negative value)
The overall coupled reaction is:
Glycerol + ATP ⇒ Glycerol-3-phosphate + ADP + H⁺
ΔG for overall reaction : 9.2 kJ + (-30.5 kJ) = -21.3 kJ
negative sign signifies that the overall reaction is spontaneous.
Gibbs free energy is the amount that gives the change in the enthalpy and its difference from the product to the temperature change and the entropy change. Gibbs free energy for the overall reaction is -21.3 kJ.
What is the Gibbs free energy of a reaction?
Gibbs free energy gives the amount of energy obtainable for the reactants to perform thermodynamic reactions.
The conversion of glycerol to glycerol-3-phosphate is unfavourable and hence, is associated with a second reaction that concerns ATP to ADP conversion.
The first reaction can be shown as:
[tex]\rm Glycerol + HPO_{4}^{2-} \rightarrow Glycerol-3-phosphate + water[/tex]
This will be non-spontaneous as the value of [tex]\rm \Delta G[/tex] (9.2 kJ) is positive.
Similarly, the second reaction will be:
[tex]\rm ATP + H_{2}O \rightarrow ADP + HPO_{4}^{2-} + H^{+}[/tex]
This will be spontaneous as the value of [tex]\rm \Delta G[/tex] (-3.5 kJ) is negative.
The overall reaction will be:
[tex]\rm Glycerol + ATP \rightarrow Glycerol-3-phosphate + ADP + H^{+}[/tex]
Gibbs free energy of the overall reaction will be:
[tex]\begin{aligned}\rm \Delta G &= 9.2 \;\rm kJ + (-30.5 \;\rm kJ) \\\\&= -21.3\;\rm kJ\end{aligned}[/tex]
Therefore, [tex]\rm \Delta G[/tex] for the overall reaction is -21.3 kJ and it will be spontaneous.
Learn more about Gibbs free energy here:
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