Consider these hypothetical chemical reactions: 1. A B, Delta G = 10.4 kJ/mol B
ID: 978336 • Letter: C
Question
Consider these hypothetical chemical reactions: 1. A B, Delta G = 10.4 kJ/mol B C, Delta G = -29.6 kJ/mol C D; Delta G = 8.30kJ/mol What is the free energy, Delta G, for the overall reaction. A D? Firefly luciferase is the enzyme that allows fireflies to illuminate their abdomens. Because this light generation is an ATP-requiring reaction, firefly luciferase can be used to test for the presence of ATP. In this way, luciferase can test for the presence of life. The coupled reactions are luciferin + O_2 oxyluciferin 4- light ATP AMP + PPi If the overall Delta G degree of the coupled reaction is -6.10 kJ/mol, what is the equilibrium constant, K, of the first reactions at 22 degree C ? The Delta G degree for the hydrolysis of ATP to AMP is -31.6 kJ/mol.Explanation / Answer
a)
sum of all gibbs free energy
= -10.9 kJ/mol
b) G=Go+RTln K
Go = -6.1 kJ/mol
G = -31.6 kJ/mol
T = 22C = 295.15K
R = 0.00831 kJ/molK
hence lnK= 25.5/(0.00831*295.15) =25.5/2.45145 = 10.402007
K = e^10.402007
K = 32925.6411676