What does a net negative ΔG indicate about the reaction of glucose + ATP to glucose 6-phosphate + ADP?

A net negative ΔG, or change in Gibbs free energy, indicates that a reaction releases energy and can occur spontaneously under standard conditions. In the case of the reaction involving glucose and ATP to form glucose 6-phosphate and ADP, this negative ΔG suggests that the conversion is favorable and occurs without the need for additional energy input.

The spontaneity linked to a negative ΔG means that the products (glucose 6-phosphate and ADP) are at a lower free energy state than the reactants (glucose and ATP), making the reaction thermodynamically favorable. This doesn't imply that the reaction proceeds rapidly, but rather that it is thermodynamically predisposed to occur in the direction written.

In this context, a negative ΔG is a key factor in metabolic pathways, indicating that the reaction can proceed in the direction shown and is important in the regulation and flow of biochemical energy within the cell.