A sample of carbon dioxide occupies a volume of 3.50 L at 125 kPa pressure. What pressure
would the gas exert if the volume was decreased to 2.0 L?

218.75 kPa

Explanation:

Carbon dioxide is a gas with chemical formula CO2.

Original volume of CO2 (V1) = 3.50 L

Original pressure of CO2 (P1) = 125 kPa

New pressure of CO2 (P1) = ?

New Volume of CO2 (V2) = 2.0 L

Since pressure and volume are given while temperature is constant, apply the formula for Boyle's law

P1V1 = P2V2

3.50L X 125 kPa = P1 x 2.0L

437.5 L•kPa = 2.0L•P1

Divide both sides by 2.0L

437.5 L•kPa/2.0L = 2.0L•P1/2.0L

218.75 kPa = P1

Thus, the new pressure of carbon dioxide would be 218.75 kPa

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.