Answer: Using the van der Waals EquationIf 10.00 mol of an

Chapter , Problem 1PE

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Problem 1PE

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.