1.00 l mixture of He, ne, and Ar has a total pressure of 662 mmHg at 298k. if the pressure of he is 341 mmHg and Ne is 112 mmHg. the mass of Ar in the mixture is 0.44 g.
Given that :
total pressure = 662 mmHg
the partial pressure He = 341 mmHg
the partial pressure Ne= 112 mmHg298
according to Dalton's law of partial pressure :
Total pressure = pressure of He + pressure of Ne + Pressure of Ar
662 = 341 + 112 + partial pressure of Ar
Partial pressure of Ar = 209 mmHg = 0.27 atm
using ideal gas equation , we get:
P V = n RT
n = (0.27 atm× 1) / 0.082 × 298
n = 0.011 mol
mass of Ar = moles × molar mass
= 0.011 × 40
= 0.44 g
Thus, 1.00 l mixture of He, ne, and Ar has a total pressure of 662 mmHg at 298k. if the pressure of he is 341 mmHg and Ne is 112 mmHg. the mass of Ar in the mixture is 0.44 g.
To learn more about Dalton's law here
https://brainly.com/question/14119417
#SPJ4
