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If 1.00 mol of argon is placed in a 0.500-l container at 22.0 ?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=1.345(l2?atm/mol2 and b=0.03219l/mol.

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calet2112989
Calculate the pressure using the Van der Waals equation and the pressure using the ideal gas equation PV=nRT. Subtract the two pressures to get the difference. then:Calculate how many moles of ammonia you have using the ideal gas equation PV=nRT. Multiply the number of moles by the molar mass of ammonia to get the mass in grams.

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