Using the van der Waals Equation
If 10.00 mol of an ideal gas were confined to 22.41 L a: 0.0 aC. it would exert a pressure of
10.00 atm. Use the van der Waals equation and Table to estimate the pressure exerted by
1.000 mol of Ct2{g) in 22.41 L at 0.0 aC.
Table Van der Waals Constants for Gas Molecules
Substance a L2@atm/mol2 b L moll
He 0.0341 0.02370
Ne 0.211 0.0171
Ar 1.34 0.0322
Kr 2.32 0.0398
Xe 4.19 0.0510
H2 0.244 0.0266
N2 1.39 0.0391
02 1.36 0.0318
F2 1.06 0.0290
CI2 6.49 0.0562
H20 5.46 0.0305
NH3 4.17 0.0371
CH4 2.25 0.0428
C02 3.59 0.0427
CCI4 20.4 0.1383
Calculate the pressure of a 2.975-mol sample of N2 in a 0.7500-L flask at 300.0 aC using the van der Waals equation and then repeat the calculation using the ideal-gas equation. Within the limits of the significant figures justified by these parameters, wl the xleal-gas equation overestimate or underestimate the pressure, and if so by how much?
(a) Underestimate by 17.92 atm. (b) Overestimate by 21.87 atm. (c) Underestimate by 0.06 atm. (d) Overestimate by 0.06 atm.
Chapter 2: Atoms Keyterms Important Scientist ● Law of Conservation of Mass ○ Matter is neither created nor destroyed during a chemical change ○ Cannot create materials from nothing, only by changing the way atoms are combined ● Law of Definite Proportions ○ A compound always contains the same elements in certain definite proportions and in no others ○ All samples of water will have 2 atoms of hydrogen and 1 atom of oxygen ○ The ratio of atoms yields a constant 2:1 volume ration ● Law of Multiple Proportions ○ Stated that elements might combine in mor
