Respuesta :
Answer: The actual free-energy change for the reaction -8.64 kJ/mol.
Explanation:
The given reaction is as follows.
Fructose 1,6-bisphosphate [tex]\rightleftharpoons[/tex] Glyceraldehyde 3-phosphate + DHAP
For the given reaction, [tex]\Delta G^{o}[/tex] is 23.8 kJ/mol.
As we know that,
[tex]\Delta G = \Delta G^{o} + RT ln Q[/tex]
Here, R = 8.314 J/mol K, T = [tex]37^{o} C[/tex]
= (37 + 273) K
= 310.15 K
Fructose 1,6-bisphosphate = [tex]1.4 \times 10^{-5}[/tex] M
Glyceraldehyde 3-phosphate = [tex]3 \times 10^{-6}[/tex] M
DHAP = [tex]1.6 \times 10^{-5}[/tex] M
Expression for reaction quotient of this reaction is as follows.
Reaction quotient = [tex]\frac{[DHAP][\text{glyceraldehyde 3-phosphate}]}{[/text{Fructose 1,6-bisphosphate}]}[/tex]
Q = [tex]\frac{1.6 \times 10^{-5} \times 3 \times 10^{-6}}{1.4 \times 10^{-5}}[/tex]
= [tex]3.428 \times 10^{-6}[/tex]
Now, we will calculate the value of [tex]\Delta G[/tex] as follows.
[tex]\Delta G = \Delta G^{o} + RT ln Q[/tex]
= [tex]23800 + 8.314 \times 310.15 \times ln(3.428 \times 10^{-6})[/tex]
= -8647.73 J/mol
= -8.64 kJ/mol
Thus, we can conclude that the actual free-energy change for the reaction -8.64 kJ/mol.
