Prove that for an ideal gas, U^ and H^ are related as H^ U^ RT, where R is the gas constant. Then: (a) Taking as given that the specific internal energy of an ideal gas is independent of the gas pressure, justify the claim that ΔH^ for a process in which an ideal gas goes from (T1, P1) to (T2, P2) equals ΔH^ for the same gas going from T1 to T2 at a constant pressure of P1. (b) Calculate ΔH(cal) for a process in which the temperature of 2.5 mol of an ideal gas is raised by 50°C, resulting in a specific internal energy change ΔU^ 3500 cal/mol.

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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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