The final four reactions in glycolysis are given below. the δg of each reaction (under a standard set of conditions) is provided as well. 1,3-bisphosphoglycerate + adp → 3-phosphoglycerate + atp δg = 0.1 kj/mol 3-phosphoglycerate → 2-phosphoglycerate δg = 0.8 kj/mol 2-phosphoglycerate → phosphoenolpyruvate + h2o δg = 1.1 kj/mol phosphoenolpyruvate + adp + h+ → pyruvate + atp δg = -23 kj/mol what is the net change in free energy for the following reaction? 2-phosphoglycerate + adp + h+→ pyruvate + atp + h2o

ΔG = -21.9kJ/mol

Explanation:

It is possible to make an algebraic sum of the ΔG's of the semireactions to obtain ΔG of a reaction.

If semireactions are:

(1) 1,3-Bisphosphoglycerate + ADP → 3-Phosphoglycerate + ATP ΔG = 0.1 kJ/mol

(2) 3-Phosphoglycerate → 2-Phosphoglycerate ΔG = 0.8 kJ/mol

(3) 2-Phosphoglycerate → Phosphoenolpyruvate + H₂O ΔG = 1.1 kJ/mol

(4) Phosphoenolpyruvate + ADP + H⁺ → Pyruvate + ATP ΔG = -23 kJ/mol

The sum of (3) + (4) gives:

2-Phosphoglycerate + ADP + H⁺ → Pyruvate + ATP + H₂O

And the net change in free energy is:

ΔG = 1.1 kJ/mol + (-23kJ/mol) = -21.9kJ/mol

I hope it helps!

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

i think the answer is terrae but not 100 percent sure. ▓▬▬ §