Question

If the following two reactions were coupled, what would be the Delta G for the overall exergonic reaction? ATP + H2O -> ADP + Pi Delta G = -31 kJ/mol Glucose + Pi -> glucose-1-phosphate + H2O Delta G = 21 kJ/mol

a) -10 kJ/mol
b) -52 kJ/mol
c) 10 kJ/mol
d) 52 kJ/mol

Answer 1

The overall Delta G for the coupled reaction can be calculated by summing up the free energy changes of the individual reactions. The coupled reaction is exergonic, resulting in a negative Delta G of -10 kJ/mol. The option (A) is correct.

Step-by-step explanation:

The overall Delta G for the coupled reaction can be calculated by summing up the free energy changes of the two reactions.

The Delta G for the hydrolysis of ATP is -31 kJ/mol, and the Delta G for the formation of glucose-1-phosphate is 21 kJ/mol. Since the overall reaction is exergonic, the Delta G will be negative. In this case, the overall Delta G is -10 kJ/mol (Option a).