1.1214 mL will a 0.205-mole sample of He occupy at 3.00 atm and 200 K.
The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).
Using equation PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.
Given data:
P= 3.00 atm
V= ?
n=0.205 mole
R= [tex]0.082057338 \;L \;atm \;K^{-1}mol^{-1}[/tex]
T=200 K
Putting value in the given equation:
[tex]\frac{nRT}{P} =V[/tex]
[tex]V= \frac{0.205 \;mole\;0.082057338 \;L \;atm \;K^{-1}mol^{-1} X 200}{3 \;atm}[/tex]
V= 1.1214 mL
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