Calculate deltaG of reaction for:
glucose+ 2 ATP ----> 2 ADP + 2 G3P
For concentrations, glucose:
5.0 mM G3P:0.019 mM ATP: 1.85 mM ADP:0.14 mM
delta G for reaction under standard conditions = -1.97 kJ, assuming the temperature is 298 K.
Do I use delta G standard + RT ln K for this reaction?
What is T in this case?
Yes, the free energy relationship between standard state and the equilibrium product constant holds.
But lets look a bit closer at what you have. If an equilibrium is present the free energy is zero for the reaction i.e. nothing is driving it either way. I think the part that might be confusing is that in the case of non-zero free energy fot the reaction rather than a K which indicates equilibrium it is better to use the symbol Q for the equilibrium product ...