Calculate the pressure that CCl4 will exert at 80 °C if1.00 mol occupies 33.3 L, assuming that (a) CCl4 obeys theideal-gas equation; (b) CCl4 obeys the van der Waals equation.(Values for the van der Waals constants are given inTable 10.3.) (c) Which would you expect to deviate morefrom ideal behavior under these conditions, Cl2 or CCl4?Explain.
Calculate the pressure that CCl4 will exert at 80 °C if1.00 mol occupies 33.3 L, assuming that (a) CCl4 obeys theideal-gas equation; (b) CCl4 obeys the van der Waals equation.(Values for the van der Waals constants are given inTable 10.3.) (c) Which would you expect to deviate morefrom ideal behavior under these conditions, Cl2 or CCl4?Explain.
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
Chapter9: The Gaseous State
Section: Chapter Questions
Problem 88AP
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Question
Calculate the pressure that CCl4 will exert at 80 °C if
1.00 mol occupies 33.3 L, assuming that (a) CCl4 obeys the
ideal-gas equation; (b) CCl4 obeys the van der Waals equation.
(Values for the van der Waals constants are given in
Table 10.3.) (c) Which would you expect to deviate more
from ideal behavior under these conditions, Cl2 or CCl4?
Explain.
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