Question #c2abd

1 Answer
Dr. Hayek
Sep 17, 2015

A real gas behaves closely to ideal behavior at low pressures and high temperatures.

Explanation:

No gas exactly follows the ideal gas law. An ideal gas is a hypothetical concept.

For a gas to behave ideally, we have assumed that there were no interparticle interactions and zero volume for the gas particles. For an ideal gas, #(PV)/(nRT) = 1 # under all conditions.
The following figure is a plot of #(PV)/(nRT)# versus P for several gases at 200 K.

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For real gases, #(PV)/(nRT)# approaches 1 only at very low pressures.

To illustrate the effect of temperature, #(PV)/(nRT)# is plotted versus P for nitrogen gas at several temperatures.

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As the temperature is increased, the behavior of the gas appears to become more ideal. From the above figures, it can be deduced that a real gas behaves closely to ideal behavior at low pressures and high temperatures.

Pictures were taking from: Chemistry - The Central Science #12^(th)# Ed.

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