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13 Dec 2019
If 1.00 mol of argon is placed in a 0.500-L container at 28.0 ?C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.363L2 bar mol?2 and b=0.03219L mol?1.
If 1.00 mol of argon is placed in a 0.500-L container at 28.0 ?C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.363L2 bar mol?2 and b=0.03219L mol?1.
Hubert KochLv2
17 Dec 2019
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