A sample of carbon dioxide occupies 2.77 L at a pressure of 18.1 psi and a temperature of 56ºC. What pressure will the carbon dioxide exert if the volume is increased to 4.81 L while the temperature is held constant?

10.4psi

Explanation:

Since the problem involves pressure and volume at constant temperature, Boyle's law is the appropriate formula to use.

Boyle's law States that at a constant temperature, the volume of a given mass of a bass is inversely proportional to its pressure.

Using Boyle's law

P1v1 = p2v2

P1 is 18.1psi

V1 is 2.77L

P2 =?

V2 is 4.81

Temperature is constant

P2 =P1v1/ v2

= 18.1 x 2.77 / 4.82

= 10.4psi

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.

you need to give more information