Ideal vs. Real Gases No gas is ideal. As the temperature of a gas increases and the pressure on the gas decreases the gas acts more ideally.

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Presentation transcript:

Ideal vs. Real Gases No gas is ideal. As the temperature of a gas increases and the pressure on the gas decreases the gas acts more ideally.

Real Gases Do Not Behave Ideally CH 4 H2H2 N2N2 CO 2 Ideal gas P (atm) PV nRT

Equation of State of an Ideal Gas Robert Boyle ( 1662 ) found that at fixed temperature –Pressure and volume of a gas is inversely proportional PV = constantBoyle’s Law J. Charles and Gay-Lussac ( circa 1800 ) found that at fixed pressure –Volume of gas is proportional to change in temperature Volume Temp o C All gases extrapolate to zero volume at a temperature corresponding to – o C (absolute zero). He CH 4 H2OH2O H2H2

Copyright © 2007 Pearson Benjamin Cummings. All rights reserved. T 1 T 2 V 1 V 2 = (Pressure is held constant) T 1 T 2 P 1 P 2 = (Volume is held constant)

Copyright © 2007 Pearson Benjamin Cummings. All rights reserved. T 1 T 2 V 1 V 2 = (Pressure is held constant) T 1 T 2 P 1 P 2 = (Volume is held constant) Charles Gay-Lussac

Kelvin Temperature Scale Kelvin temperature (K) is given by K = o C where K is the temperature in Kelvin, o C is temperature in Celcius Using the ABSOLUTE scale, it is now possible to write Charles’ Law as V / T = constant Charles’ Law Gay-Lussac also showed that at fixed volume P / T = constant Combining Boyle’s law, Charles’ law, and Gay-Lussac’s law, we have P V / T = constant Gay-Lussac Charles