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When comparing two gases to determine which one is closest to an ideal gas, which strategy is best? A. Look up the van der Waals' contstants. The gas with the smaller "b" value must be more ideal

BCalculate R. The more ideal gas is the one with an R value closest 0.08206 L • atm • mol–1 • K–1

CLook up the van der Waals' contstants. The gas with the higher "a" value must be more ideal.

DCalculate the molar mass of each gas. A large molar mass indicates an ideal gas.

Verified Answer :

P + a n² / V²) x (V - nb) = nRT 

certainly if a = 0 and b = 0, the equation reduces to 
P x V = nRT 
(the ideal gas law right?) 

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