At a certain temperature, a mixture of 2 gases, 11.2 g of oxygen and 104.75 of krypton exert a total pressure of 4.25 atm. What is the partial pressure of each gas in mm Hg?

Pressure of O₂ = 0.93 atm

Pressure of krypton = 3.32 atm

Explanation:

This problem can be solved by using Dalton's Law of Partial Pressures, which states that the partial pressure of a component of a gaseous mixture depends on the mole ratio of said component and the total pressure of the gaseous mixture.

Pₐ = Xₐ * Ptotal

P ₐ - the partial pressure of component a

χ ₐ - its mole fraction in the mixture

P total - the total pressure of the mixture

The moles of the two gases are:

moles of O₂ = 11.2/32 = 0.35 moles

moles of krypton = 104.75/83.8 = 1.25 moles

Total moles = 1.25 + 0.35 = 1.6 moles

Xₐ = number of moles of a / total moles in mixture

Pressure of O₂ = 0.35/1.6 * 4.25 = 0.93 moles

Pressure of krypton = 1.25/1.6 * 4.25 = 3.32 moles