**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.

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 ^{o}C. (Assume for simplicity that the ideal-gas equation still holds.)

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