Question

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

Answer 1

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:

$PV=nRT$ (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:

$P=\frac{nRT}{V}$

$P=\frac{(0.480)(0.082057)(300)}{0.700}=16.88 atm$

2) The vander Walls equation is:

$(P+\frac{a}{V^{2}})(V-b)=RT$

solving for P

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