Asample of gas has a mass of 827 mg . its volume is 0.270 l at a temperature of 88 ∘ c and a pressure of 975 mmhg . find its molar mass

Steps:

Mw = w * R * T / p * V

T = 88 + 273 => 361 K

p = 975 mmHg in atm :

1 atm  = 760 mmHg

975 mmg / 760 mmHg =>  1.28 atm

Therefore:

= 0.827 * 0.0821 * 361 /  1.28 * 0.270

=  24.51 / 0.3456

molar mass =  70.92 g/mol

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.