A gas occupies a volume of 8.60 L at 45C and 764 torr. What pressure would it occupy if the volume is adjusted to 13.3 L at 20C?

455 Torr

Explanation:

To get the correct answer, we employ the use of the General gas equation.

In its general form, the General gas equation can be written as:

P1V1/T1 = P2V2/T2

Defining the parameters;

P1 = 764 torr

V1 = 8.6L

T1 = 45 degrees Celsius = 273.15+ 45 = 318.15K

P2 = ?

V2 = 13.3L

T2 = 20 degrees Celsius = 273.15 + 20 = 293.15K

Rearranging the equation yields: P2 = P1V1T2/T1V2

Substituting the values:

P2 = (764 * 8.6 * 293.15)/(318.15 * 13.3)

P2= 455.2 Torr

whats the meaning of /

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.