Answer:
The answers to the question are
Partial pressure of neon = 399.42
Partial pressure of xenon = 240 torr
Explanation:
From the universal gas equation
P×V = n × R × T
n = P × V÷(R×T)
= ((640 torr /(7.5×10^(-3))× 5/ L)÷(8.314×373.15))/1000
= 0.13751 moles
Therefore, if the mass of gas = x, we have
0.203×x mass of neon and
0.797×x mass of xenon
Molar mass of neon = 20.179 g/mol
Molar mass of xenon = 131.30 g/mol
Summing the moles of neon and xenon, we have
(0.203×x)/ (20.179) + 0.797×x/( 131.30) = 0.13751 moles
1.6×10^(-2)x= 0.13751
x = 8.5306 g
Number of moles of neon =
(0.203× 8.5306 )/ (20.179) = 8.58×10(-2) moles
Mole fraction of neon = (8.58×10(-2))/ 0.13751 = 0.624
Partial pressure of neon = (mole fraction)×(total pressure of gas) = 0.624× 640 torr = 399.42 torr
Partial pressure of xenon = 240 torr