- #1

Chandasouk

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V = 6.0L

T=318.15K

P

_{total}=1.75atm

mole fraction: X

_{He}=0.25

X

_{Ar}=0.35

X

_{CH4}=0.40

Because mole fractions always add up to 1

Then I used Partial Pressure formula

Partial Pressure of CH4 = 0.40 X 1.75atm = 0.7atm

Then Ideal gas law

n=PV/RT

n=(0.7atm)(6L)/(.o8206)(318.15K) = 0.16087 moles of CH4

0.16087 moles of CH4 X 6.022 x 10

^{23}molecules = 9.69 X 10^22 molecules of methane?