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# Solved: Using the van der Waals EquationIf 10.00 mol of an ISBN: 9780321910417 77

## Solution for problem 2PE Chapter 10.15SE

Chemistry: The Central Science | 13th Edition

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Problem 2PE

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                                0.0303

Xe                    4.10                                0.0510

H2                    0.244                                0.0200

N2                    1.30                                0.0301

02                    1.38                                0.0318

F2                    1.06                                0.0200

CI2                    0.40                                0.0502

H20                    5.46                                0.0305

NH3                    4.17                                0.0371

CH4                    2.25                                0.0428

C02                    3.50                                0.0427

CCI4                    20.4                                0.1383

A sample of 1.000 mol of C02{g} is confined to a 3.000-L container at 0.000 aC. Calculate the pressure of the gas using (a) the ideal-gas equation and (b) the van der Waals equation.

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##### ISBN: 9780321910417

Since the solution to 2PE from 10.15SE chapter was answered, more than 230 students have viewed the full step-by-step answer. This full solution covers the following key subjects: . This expansive textbook survival guide covers 305 chapters, and 6351 solutions. The answer to “Using the van der Waals EquationIf 10.00 mol of an ideal gas were confined to 22.41 L a: 0.0 aC. it would exert a pressure of10.00 atm. Use the van der Waals equation and Table to estimate the pressure exerted by1.000 mol of Ct2{g) in 22.41 L at 0.0 aC.Table Van der Waals Constants for Gas MoleculesSubstance a L2@atm/mol2 b L mollHe 0.0341 0.02370Ne 0.211 0.0171Ar 1.34 0.0322Kr 2.32 0.0303Xe 4.10 0.0510H2 0.244 0.0200N2 1.30 0.030102 1.38 0.0318F2 1.06 0.0200CI2 0.40 0.0502H20 5.46 0.0305NH3 4.17 0.0371CH4 2.25 0.0428C02 3.50 0.0427CCI4 20.4 0.1383A sample of 1.000 mol of C02{g} is confined to a 3.000-L container at 0.000 aC. Calculate the pressure of the gas using (a) the ideal-gas equation and (b) the van der Waals equation.” is broken down into a number of easy to follow steps, and 125 words. The full step-by-step solution to problem: 2PE from chapter: 10.15SE was answered by , our top Chemistry solution expert on 09/04/17, 09:30PM. This textbook survival guide was created for the textbook: Chemistry: The Central Science, edition: 13. Chemistry: The Central Science was written by and is associated to the ISBN: 9780321910417.

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

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