Assume that you have 0.480 mol of N2 in a volume of 0.700 L at 300 K .

1. Calculate the pressure in atmospheres using the ideal gas law.
2. Calculate the pressure in atmospheres using the van der Waals equation. For N2 , a=1.35 (L2⋅atm)/mol2 , and b=0.0387 L/mol

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Respuesta :

JhoanEusse JhoanEusse · Answer 1 · 2020-02-11T05:09:02+01:00

Answer:

1) 16.88 atm

2) 34.47 atm

Explanation:

Data:

Volume=0.700L

Temperature = 300K

Number of moles=0.480 mol

Ideal gas constant=0.082057 L*atm/K·mol

1) The ideal gas law is:

[tex]PV=nRT [/tex] (1)

with P the pressure, T the temperature, n the number of moles, V the volume and R the ideal gas constant , so solvig (1) for P:

[tex]P=\frac{nRT}{V} [/tex]

[tex]P=\frac{(0.480)(0.082057)(300)}{0.700}=16.88 atm [/tex]

2) The vander Walls equation is:

[tex] (P+\frac{a}{V^{2}})(V-b)=RT[/tex]

solving for P

[tex] P=\frac{RT}{V-b}-\frac{a}{V^2}=\frac{(0.082057)(300)}{0.700-0.0387}-\frac{1.35}{0.700^2}=34.47 atm[/tex]