Question

The van der Waals equation of state for a real gas is (P+ ) (V - nb) = nRT 

At what pressure will 1.00 mole of CH₄ be in a 10.0 L container at 298 K assuming CH₄ is a real gas. 

(van der Waals constants for CH₄ are α = -2.253 L² atm mol^-2. b = 0.04278 L mol^-1) 

•  2.43 atm 

•  2.28 atm 

•  2.51 atm 

•  24.5 atm 

•  0.440 atm

Answer 1

we have van der waals equation and vules given
use R = 0.0821 l atm/mol/k
[P+an^2/V^2][v-nb] = nRT

[P+an^2/V^2] = nRT/[V-nb]

[P+an^2/V^2] = 1*0.0821 l atm/mol/k*298 K/[10 L - 1*0.04278 Lmol-1]
[P+an^2/V^2] = 24.4658/9.95722 = 2.45709

[P +2.253*1^2/(10)^2] = 2.45709

P+ 0.02253 = 2.45709
P = 2.45709-0.02253 = 2.43456 atm

Answer option A:: 2.43 atm
*********************************