(5) Using the data in Table 1C.3 (from the textbook), calculate the pressure that 2.500 moles of carbon dioxide confined in a volume of 1.000 L at 450 K exerts. Compare the pressure with that calculated assuming ideal-gas behavior.

(5) Using the data in Table 1C.3 (from the textbook), calculate the pressure that 2.500 moles of carbon dioxide confined in a volume of 1.000 L at 450 K exerts. Compare the pressure with that calculated assuming ideal-gas behavior.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter10: Solids, Liquids, And Phase Transitions

Section: Chapter Questions

Problem 6P

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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

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Table 1C.3 van der Waals coefficients*
a/(atm dmºmol²)
b/(10²dm²mol')
Ar
1.337
3.20
CO,
3.610
4.29
Не
0.0341
2.38
Хе
4.137
5.16
* More values are given in the Resource section.

(5) Using the data in Table 1C.3 (from the textbook), calculate the pressure that 2.500 moles of
carbon dioxide confined in a volume of 1.000 L at 450 K exerts. Compare the pressure with
that calculated assuming ideal-gas behavior.

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