If a gaseous mixture is made by combining 3.17 g Ar 3.17 g Ar and 1.30 g Kr 1.30 g Kr in an evacuated 2.50 L container at 25.0 ∘ C, 25.0 ∘C, what are the partial pressures of each gas, P Ar PAr and P Kr , PKr, and what is the total pressure, P total , Ptotal, exerted by the gaseous mixture?

The partial pressures of argon is 0.77 atm and krypton is 0.16 atm.

The total pressure exerted by the gaseous mixture is 0.93 atm

Explanation:

Mass of argon gas  =

Mass of krypton gas  =

Mixture in terms of mole fractions:

Moles of argon gas =

Moles of krypton gas =

Mole fraction of argon gas =

=

Mole fraction of carbon dioxide gas =

=

Pressure of the exerted by the gaseous mixture= P

Temperature of the mixture = T = 25.0 °C =25.0+273K=298.0 K

Volume of the container in which mixture is kept =

Moles of gases,n =

PV=nRT

Partial pressure of argon gas =

Partial pressure of krypton gas =

The partial pressures of argon is 0.77 atm and krypton is 0.16 atm.

The total pressure exerted by the gaseous mixture is 0.93 atm

with this one i know the answer in craters one reason i looked it up and i learned about it there is my evidence