Question

Calculate the pressure exerted by 11.1 moles of neon gas in a volume of 5.45 L at 25°C using (a) the ideal gas equation and (b) the van der Waals equation. (For neon, a = 0.211 atm · L2/mol2 and b = 0.0171 L/mol.)

Answer 1

49.82414 atm

50.74675 atm

Step-by-step explanation:

P = Pressure

V = Volume = 5.45 L

R = Gas constant = 0.08205 L atm/mol K

T = Temperature = 25°C

a = 0.211 atm L²/mol²

b = 0.0171 atm L²/mol²

From ideal gas law we have

`PV=nRT\\\Rightarrow P=(nRT)/(V)\\\Rightarrow P=(11.1* 0.08205(273.15+25))/(5.45)\\\Rightarrow P=49.82414\ atm`

The pressure is 49.82414 atm

From Van der Waals equation we have

`\left(P+(an^2)/(V^2)\right)\left(v-nb\right)=nRT\\\Rightarrow P=(nRT)/(V-nb)-(an^2)/(V^2)\\\Rightarrow P=(11.1* 0.08205* (273.15+25))/(5.45-(11.1* 0.0171))-(0.211* 11.1^2)/(5.45^2)\\\Rightarrow P=50.74675\ atm`

The pressure is 50.74675 atm