CHEM 001 Lecture Notes - Lecture 17: Ideal Gas, Collision Theory, Activation Energy
13 Aug 2020
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High pressures (+10 atm) push gas molecules together, causing them to exert weaker outward forces on the container. Low temperatures (~boiling points) cause gas molecules to settle close together and thus exert weaker outward force on the container. C. * my theory, not sure if true*: volume: vreal > videal. Higher pressures (+100 atm) push gas molecules so close that the actual volumes begin to touch, causing it to resist compression relative to what was predicted. Higher temperatures (>>>>boiling points) cause gas molecules to move around so violently they push the container outward farther than what was calculated. Rms velocity of real and ideal gas molecules is directly proportional to the temperature. In a pv/rt = n graph, the numerator is the product of volume and pressure. Thus, the deviations will be less or greater than ideal at some points to either vreal > videal or preal < pideal. Positive deviation = molecular volume, very high temperature and pressure,
