Which observation indicates that the kinetic-molecular theory has limited use for describing a certain gas? Gas particles are acting like tiny, solid spheres. Gas particles are obeying Newton’s laws of motion. Increasing pressure is reducing the volume of the gas. Increasing collisions of gas molecules will increase energy between them.

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.

there is none because earth is stationary and flat.