If the δg° of the reaction a → b is –40 kj/mol, under standard conditions the reaction:

The value of Gibbs free energy of the reaction is negative which means that  reaction is spontaneous.

Explanation:

ΔG° = ΔH° - TΔG°

Where:

ΔG° = Change in Gibbs free energy at T temperature

ΔH° = Enthalpy of reaction at T temperature

ΔS° = Entropy change of reaction at T temperature

A → B ,ΔG° = -40

The value of Gibbs free energy of the reaction is negative which means that  reaction is spontaneous.

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.