A 0.500 mol sample of O2 gas is in a large cylinder with a movable piston on one

Question

A 0.500 mol sample of O2 gas is in a large cylinder with a movable piston on one end so it can be compressed. The initial volume is large enough that there is not a significant difference between the pressure given by the ideal gas law and that given by the van der Waals equation.

As the gas is slowly compressed at constant temperature (use 300 K), at what volume does the van der Waals equation give a pressure that is 5% higher than the ideal gas law pressure? Let a= .14 N*m^4/mol^2 and b=3.2 *10^-5 m^3/mol.

At what volume does the van der Waals equation give a pressure that is 5% lower than the ideal gas law pressure?

Explanation / Answer

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