Under what limiting conditions does a real gas governed by Van der Waals' equation closely approximate an ideal gas_______________________?
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Answer: A. Both a and b are small
Explanation
Real gases approach ideal gas behavior under conditions where correction constants are negligible. Low pressure and high temperature make both molecular volume and intermolecular attraction terms small. Under these limiting conditions, the Van der Waals equation simplifies directly into the ideal gas law. The Van der Waals equation modifies the ideal gas law by adding correction terms for real fluids. Constant a accounts for intermolecular attractive forces pulling molecules inward toward each other. Constant b accounts for the finite physical volume occupied by the gas molecules themselves.
Chemical engineers use ideal gas assumptions to simplify routine calculations at ambient conditions. Recognizing when real gas corrections are necessary prevents significant errors in reactor design. High-pressure industrial processes demand complex equations of state rather than ideal gas models. Large correction values indicate extreme non-ideal behavior occurring at high pressures and low temperatures. Mixed magnitude conditions still result in significant departures from ideal gas law predictions. Assuming only one constant is small ignores the combined effects required for ideal approximation.
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