Respuesta :
The density of a sample of nitrogen gas (N₂) that exerts a pressure of 5.30 atm in a 3.50-L container at 125°C is 4.54 gm/litre
What is the Ideal Gas Law ?
This law combines the relationships between p, V, T and mass, and gives a number to the constant.
The ideal gas law is:
pV = nRT
where n is the number of moles, and R is universal gas constant.
The value of R depends on the units involved, but is usually stated with S.I. units as: R = 8.314 J/mol·K
The values given in the question are
p= 5.30 atm , V=3.50 L
T (in Kelvin) = 125+273 K
= 398 K
R = 0.0821 L·atm /mol·K
The Ideal Gas equation can be re written as
pM=DRT
M is the molar mass , D is the density
M for N₂ is 28 gm/mol
so density can be determined as
[tex]\rm D= \dfrac{p M}{RT} \\\\\rm D= \dfrac{5.3\; \times 28}{0.082 \;\times398} \\\\\rm D =4.54 gm/litres[/tex]
Therefore the density of a sample of nitrogen gas (N₂) that exerts a pressure of 5.30 atm in a 3.50-L container at 125°C is 4.54 gm/litre
To know more about Ideal Gas Law
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