Unit 10 real gases vdw fl14 final
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The document discusses real gases and their behaviors in relation to the van der Waals equation, highlighting that real gases deviate from ideal behavior due to interactions at low temperatures and high pressures. It introduces the compressibility factor (z) as a measure of these deviations and explains how the van der Waals equation corrects the ideal gas law to account for intermolecular attractions and the volume occupied by gas molecules. Additionally, the document compares the van der Waals constants for various gases based on their molecular properties.
Unit 10 real gases vdw fl14 final
- 1. *Real Gases and the van der Waals Equation By Shawn P. Shields, Ph. D. This work is licensed by Shawn P. Shields-Maxwell under a Creative Commons Attribution- NonCommercial-ShareAlike 4.0 International License.
- 2. *Real Gases…What are they? *Most gases behave ideally when they are held at low pressures and “high” temperatures. (Room temperature is considered high T.) *Remember that “ideal behavior” means that the gas molecules do not interact with each other. Only kinetic energy is present.
- 3. *Real Gases…What are they? *However, sometimes gas molecules DO interact with each other. *Interactions between gas molecules is more likely at *low temperatures *high gas pressures (i.e., high gas densities). This introduces potential energy into the picture!
- 4. *Real Gases…What are they? * Molecules that have significant intermolecular attractions (aka “polar” molecules) may also interact with each other. + “partial charges” on the molecules are attracted to each other Water is a polar molecule.
- 5. *The Compressibility Factor, Z *We can use the “compressibility factor” (Z) to detect deviations of a gas from ideal behavior in experiments. 𝐙 = 𝐏𝐕 𝐧𝐑𝐓 *When Z < 1, intermolecular attractions exist, and gas molecules can “feel” each other’s presence.
- 6. *Real Gas Behavior Compare 3 scenarios for gases in a piston… The first piston shows a gas at low pressure. Vactual = Videal Ideal Gas Law and KTG are obeyed. Low P
- 7. *Real Gas Behavior The second piston shows a gas at med-high pressure. As the volume decreases, some molecules stick together, effectively reducing the moles of gas. Now, Vactual < Videal The gas is more compressible, and attractions dominate! Med to high P
- 8. *Real Gas Behavior Compare 3 scenarios for gases in a piston… The third piston shows a gas at REALLY high pressure. The gas cannot move and we see that it actually DOES take up space…as our common sense might tell us. Now, Vactual > Videal Repulsions dominate! Ridiculously high P
- 9. *The Compressibility Factor, Z *More about the compressibility factor Z Z = 1 𝒁 = 𝑷𝑽 𝒏𝑹𝑻 P (atm) Perfectly ideal gas behavior Real gases Behaves as an ideal gas under reasonable conditions Attractions dominate Repulsions dominate
- 10. *The van der Waals Equation *Corrects the Ideal Gas Law for real gas behavior. 𝑃 = 𝑛𝑅𝑇 𝑉 − 𝑛𝑏 − 𝑎𝑛2 𝑉2 *The van der Waals constants a and b are experimentally-determined for each individual gas. *The vdw constant a describes the strength of attractions with units L2 atm mole–2 *The vdw constant b increases with increasing molecular size with units L mol–1
- 11. *The van der Waals Equation *Corrects the Ideal Gas Law for real gas behavior. 𝑃 = 𝑛𝑅𝑇 𝑉 − 𝑛𝑏 − 𝑎𝑛2 𝑉2 Correction for the volume taken up by the gas molecules Correction for the attractions between gas molecules. The actual pressure P is reduced by this amount compared to the Ideal Gas law.
- 12. *The van der Waals Equation *Predict the relative size of the van der Waals constants for the following gases: H2 gas (very small and not polar) SO2 gas (larger atoms and polar) 𝑃 = 𝑛𝑅𝑇 𝑉 − 𝑛𝑏 − 𝑎𝑛2 𝑉2
- 13. *The van der Waals Equation *Predict the relative size of the van der waals constants for the following gases: H2 gas (very small and not polar) SO2 gas (larger atoms and polar) The vdw constant a and b would both be larger for SO2 gas.
- 14. *The van der Waals Equation *Which gas would produce the lowest pressure, with moles, T and V constant? CH4 (methane) gas (small molecule and not polar) H2O gas (small molecules and polar) 𝑃 = 𝑛𝑅𝑇 𝑉 − 𝑛𝑏 − 𝑎𝑛2 𝑉2
- 15. *The van der Waals Equation *Which gas would produce the lowest pressure, with moles, T and V constant? 𝑃 = 𝑛𝑅𝑇 𝑉 − 𝑛𝑏 − 𝑎𝑛2 𝑉2 If CH4 is a small molecule, and not polar, this means that a and b are both relatively small. (a = 2.25, b = 0.0428) The gas should behave close to ideally. If H2O gas is also a small molecule, then the vdw constant b will be of a similar size. However, since water is polar, the vdw constant a will be quite a bit larger. (a = 5.46, b = 0.0305) The pressure exerted by water will be lower than the ideal pressure.
- 16. *Summary *Real gases interact with each other and take up volume in the container. *The van der Waals equation corrects the Ideal Gas Law for real gas behavior. 𝑃 = 𝑛𝑅𝑇 𝑉 − 𝑛𝑏 − 𝑎𝑛2 𝑉2 If the gas is under ideal gas conditions, the van der Waals equation reduces to the Ideal Gas Law PV=nRT (Try this by making a and b = 0)