In a mixture of he, ne, and xe gases with a total pressure of 925 atm, if there is 10.5 g of each gas in the mixture, what is the partial pressure of xe?

Partial pressure of Xe = 22.9 atm

Explanation:

Given:

Total pressure of gas mixture = 925 atm

Mass of He = Ne = Xe = 10.5 g

To determine:

Partial pressure of Xe

Explanation:

As per Dalton's Law in a mixture of gases the total pressure is the equal to the sum of partial pressures

In this case:

-------------(1)

Partial pressure of each gas can be expressed as:

-----(2)

where n(Xe) = moles of Xe

n(Total) = total moles

Therefore,

n(Total) = 0.080+2.625+0.525 = 3.23

Substituting for nXe, n(Total) and P(total) in equation (2)

answer: a chemical reaction

explanation:

im not wrong

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.