The partial pressure of fluorine gas in a 2.00 L container is 0.85 atm while the partial pressure in that same 2.00L container of argon gas is 1350 torr. a) What is the total pressure, in atm? b) What is the mole fraction of argon in the container?

The total pressure, in atm is 2.62

b. The mole fraction of argon in the container is 0.67.

Explanation:

a) According to Dalton's law, the total pressure is the sum of individual pressures.

Given : =total pressure of gases = ?

= partial pressure of fluorine = 0.85 atm

= partial pressure of Argon = 1350 torr = 1.77 atm   ( 760 torr = 1atm)  

putting in the values we get:

b) According to Raoult's law, the partial pressure of a component at a given temperature is equal to the mole fraction of that component multiplied by the total pressure.

where, x = mole fraction

The mole fraction of argon in the container is 0.67.

a chemical reaction

explanation:

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.