Acyclopropane-oxygen mixture is used as an anesthetic. if the partial pressure of cyclopropane in the mixture is 334 mmhg and the partial pressure of the oxygen is 1.02 atm, what is the total pressure of the mixture in torr?

Total pressure = 1109.2 torr

Explanation:

Given data:

Partial pressure of cyclopropane = 334 mmHg

Partial pressure pressure of oxygen = 1.02 atm

Total pressure of mixture = ?

Solution:

Formula:

Total pressure = P of C₃H₆ + P of O₂

1 atm = 760 torr = 760 mmHg

1.02 atm × 760 torr / 1atm = 775.2 torr

Total pressure = P of C₃H₆ + P of O₂

Total pressure = 334 torr + 775.2 torr

Total pressure = 1109.2 torr

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.