A 488.3 gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C. (heat capacity of solid = 2.96 J/g･°C; heat capacity of liquid = 1.75 J/g･°C; ∆Hfusion = 8.04 kJ/mol; Tfinal = 17.6 °C) A)How much energy (in kJ) is absorbed/released to heat the solid?
B)How much energy (in kJ) is absorbed/released to melt the solid?
C) How much energy (in kJ) is absorbed/released to heat the liquid?
D)What is the total amount of energy that must be absorbed/released for the entire process?

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.

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hurricanes form in warm water