Respuesta :
Answer:
Partial Pressure of Neon =384.128 torr
Partial Pressure of Xenon = 255.872 torr.
Explanation:
Mass of Neon = 20.3% = 0.203 gram
Mass of Xenon = 79.7% = 0.797 gram
Standard Molar mass of Neon = 20.1797
Standard Molar mass of Xenon = 131.293
Number of moles of Ne = [tex]\frac{mass}{molar mass}[/tex]
=[tex]\frac{0.203}{20.17974}[/tex]
=0.01006 moles of Ne
Number of moles of Xe = [tex]\frac{mass}{molar mass}[/tex]
=[tex]\frac{0.797}{131.293}[/tex]
= 0.00607 moles of Xe
Total number of moles of both gases;
= 0.01006 + 0.00607
= 0.01676 moles
The partial pressure of gases of each gas is directly proportional to their mole fraction. As such;
Mole fraction of Ne = [tex]\frac{number of moles of Ne }{Total moles}[/tex]
[tex]= \frac{0.01006}{0.01676}[/tex]
= 0.6002 moles
Mole fraction of Xe = 1 - mole fraction of Ne
= 1 - 0.6002
= 0.3998 moles
∴ Partial pressure of Neon = mole fraction of Neon × the total of 640 torr
= 0.6002 × 640
= 384.128 torr
Partial pressure of Xenon = mole fraction of Xenon × the total of 640 torr
= 0.3998 × 640
= 255.872 torr
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
