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.

Question

Jordan Sanders

Chemistry

10 June, 03:42

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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Jaylyn Heath · Answer 1

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.