Which equation accounts for deviations from ideal gas behavior?

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Multiple Choice

Which equation accounts for deviations from ideal gas behavior?

Explanation:
Deviations from ideal gas behavior come from real gas characteristics: molecules occupy finite space and they attract each other. The van der Waals equation adds two corrections to the ideal gas law to capture these effects. It includes a term that increases the pressure to account for attractive forces (often written as P + a(n/V)^2) and a term that reduces the effective volume available to the molecules (V − nb) to account for the finite size of the molecules. The full form for n moles is (P + a(n/V)^2)(V − nb) = nRT, or for one mole, (P + a/Vm^2)(Vm − b) = RT. This framework explains why real gases don’t follow PV = nRT exactly at high pressures or low temperatures: the simple ideal gas law neglects both molecular size and intermolecular attractions, which the van der Waals equation explicitly incorporates.

Deviations from ideal gas behavior come from real gas characteristics: molecules occupy finite space and they attract each other. The van der Waals equation adds two corrections to the ideal gas law to capture these effects. It includes a term that increases the pressure to account for attractive forces (often written as P + a(n/V)^2) and a term that reduces the effective volume available to the molecules (V − nb) to account for the finite size of the molecules. The full form for n moles is (P + a(n/V)^2)(V − nb) = nRT, or for one mole, (P + a/Vm^2)(Vm − b) = RT. This framework explains why real gases don’t follow PV = nRT exactly at high pressures or low temperatures: the simple ideal gas law neglects both molecular size and intermolecular attractions, which the van der Waals equation explicitly incorporates.

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