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
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
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