Gases behave non-ideally at high pressures and low temperatures. Larger molecules also tend to increase the volume of the gas beyond what is predicted by the ideal gas equation.
You may want to reference (Pages 196 - 236) Chapter 5 while completing this problem.
Which of the following best explains why the two values of pressure in Parts A (using van der Waals equation) and B (using ideal gas equation) are different?
The perceived forces between chlorine gas molecules that contribute to nonideal behavior are most strongly influenced by
a) the high system pressure and high system temperature.
b) the high system temperature and relatively large chlorine molecule size.
c) the polar chlorine molecules and the low system temperature.
d) the high system pressure and relatively large chlorine molecule size.
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