Problem: It turns out that the van der Waals constant b equals four times the total volume actually occupied by the molecules of a mole of gas. Using this figure, calculate the fraction of the volume in a container actually occupied by Ar atoms:Assume b= 0.0322 L/mol.at 200 atm pressure and 0 oC. (Assume for simplicity that the ideal-gas equation still holds.) 

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Concept: van der Waals equation.

Using the b constant for Ar gas, find the initial volume of Ar gas. 

Next use the ideal gas law to solve for the volume at T= 0°C and P = 200 atm.

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It turns out that the van der Waals constant b equals four times the total volume actually occupied by the molecules of a mole of gas. Using this figure, calculate the fraction of the volume in a container actually occupied by Ar atoms:
Assume b= 0.0322 L/mol.

at 200 atm pressure and 0 oC. (Assume for simplicity that the ideal-gas equation still holds.) 

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