Achemical reaction has an increase in entropy and a decrease in enthalpy. what is known about the spontaneity of the reaction?

Reaction is spontaneous at all temperatures.

Explanation:

According to Gibb's equation:

= Gibbs free energy

= enthalpy change

= entropy change

T = temperature in Kelvin

= +ve, reaction is non spontaneous

= -ve, reaction is spontaneous

= 0, reaction is in equilibrium

Thus when = -ve (decrease in enthalpy)

= +ve (increase in entropy)

Thus Reaction is spontaneous at all temperatures.

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.

the electrical  conductivity  of asolution  of an electrolyte is measured by determining the resistance of thesolution  between two flat or cylindrical electrodes separated by a fixed distance.