Question

Use the van der Waals equation of state to calculate the pressure of 2.30 mol of CH, at 455 K in a 5.50 L vessel. Van der Waals constants can be found in the van der Waals constants table. Use the ideal gas equation to calculate the pressure under the same conditions. atm

Answer 1

classmate Date Page For CHI , a=0 2.300 bar 1²/mo12 Se 23 2360 X 1X0'. d =2.3008 1.01325 atmo L/mol a = 2.33 atm 2²/molt ba 0.04301 L/mol. Now, Vander waads equini (P+ am (V- nb) = nRT =(P+ 21338622303) (5.50- 2:30X0:04301) e - 2 20 30 082 x 256 → (P + 0.407) (5:4012) - 85.813 p= 85.813 - 0.407 = 15.48 5.4012 Thus, Pressure is 15.48 atm sou for Ideal gas, w ood PV = nRT reprox 6.50 a soron No= 5.50 Litrea 5.50x103 m3. IT Å 455k R=8.314 neep J.K mo 1 n=2. 30 4 PX 5.50 810 322.308 8.314 x 455 p= (2-30 X 8.314x455) / 5.50 X sors - 1581927 pa 2181927/ 101 325 atm = 15.61124 atm I 1 atm= 101325 pa

classmate Date Page Ideal behaviou is limited to gan molecules. - Boiling point CH4 i 1610 5 °C eau 76° 72°C Thus, cala is tum liquid at room temperature tus conile CH4 is gaseous at rz. Thus, CHL occupies a targer volume. Thus, Cty shows more ideal behavion. Am CH 4 because it occupies a larger volume and it heis smaller dispersion forces between molecules C: CH4 is gaseous molecule , thens, dispersion forces between niolecules is