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Using the van der Waals EquationIf 10.00 mol of an ideal

Chemistry: The Central Science | 12th Edition | ISBN: 9780321696724 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward ISBN: 9780321696724 27

Solution for problem 16PE Chapter 10

Chemistry: The Central Science | 12th Edition

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Chemistry: The Central Science | 12th Edition | ISBN: 9780321696724 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward

Chemistry: The Central Science | 12th Edition

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Problem 16PE

Using the van der Waals Equation

If 10.00 mol of an ideal gas were confined to 22.41 L at 0.0 °C, 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 Cl2(g) in 22.41 L at 0.0 °C.

Table Van der Waals Constants for Gas Molecules

Substance

a(L2@atm/mol2)

b(L/mol)

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

O2

1.36

0.0318

F2

1.06

0.0290

Cl2

6.49

0.0562

H2O

5.46

0.0305

NH3

4.17

0.0371

CH4

2.25

0.0428

CO2

3.59

0.0427

CCl4

20.4

0.1383

A sample of 1.000 mol of CO2(g) is confined to a 3.000-L container at 0.000 °C. Calculate the pressure of the gas using (a) the ideal-gas equation and (b) the van der Waals equation.

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Textbook: Chemistry: The Central Science
Edition: 12
Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward
ISBN: 9780321696724

The answer to “Using the van der Waals EquationIf 10.00 mol of an ideal gas were confined to 22.41 L at 0.0 °C, 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 Cl2(g) in 22.41 L at 0.0 °C.Table Van der Waals Constants for Gas MoleculesSubstancea(L2@atm/mol2)b(L/mol)He0.03410.02370Ne0.2110.0171Ar1.340.0322Kr2.320.0398Xe4.190.0510H20.2440.0266N21.390.0391O21.360.0318F21.060.0290Cl26.490.0562H2O5.460.0305NH34.170.0371CH42.250.0428CO23.590.0427CCl420.40.1383A sample of 1.000 mol of CO2(g) is confined to a 3.000-L container at 0.000 °C. 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 92 words. This textbook survival guide was created for the textbook: Chemistry: The Central Science, edition: 12. The full step-by-step solution to problem: 16PE from chapter: 10 was answered by , our top Chemistry solution expert on 04/03/17, 07:58AM. Chemistry: The Central Science was written by and is associated to the ISBN: 9780321696724. This full solution covers the following key subjects: mol, gas, van, Waals, equation. This expansive textbook survival guide covers 49 chapters, and 5471 solutions. Since the solution to 16PE from 10 chapter was answered, more than 357 students have viewed the full step-by-step answer.

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