The free energy for ATP hydrolysis in vivo is actually greater than the standard free energy change of -30 kJ mol-1 because
A)it has stronger electrostatic repulsion.
B)of the actual concentrations of ATP and its hydrolysis products in cells.
C)it can easily be formed from other nucleotide triphosphates.
D)it can participate in phosphoryl group transfers.
E)All of the above.

Question

Quizplus · Accepted Answer

The actual concentrations of ATP and its hydrolysis products in cells affect the free energy for ATP hydrolysis in vivo. This is known as the standard free energy change of reaction and it takes into account the concentrations of reactants and products under standard conditions. In cells, the actual concentrations of ATP and its hydrolysis products may be different from the standard conditions, resulting in a change in the free energy of the reaction. This means that the actual free energy for ATP hydrolysis in vivo is greater than the standard free energy change of -30 kJ mol-1. Choices A, C, and D are not related to the actual free energy for ATP hydrolysis in vivo.

The Free Energy for ATP Hydrolysis in Vivo Is Actually