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Chem 6AH lecture 4

# Chem 6AH lecture 4 - Response of gas to temperature All...

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Q: As molar mass of a gas increases, its pressure should decrease (assume everything else is constant) - decrease, because the frequency that hit the wall is slower as the molecules get heavy Ideal Gas Law: E(QV) of State - related differ...(Pressure Boyle: the father of experiemental chemistry and biology: no preconception between the experiment ABC: Avocadro, Broyle's , Charles Bolyle's Law - Gases can be compressed or expanded and will return to their original volume - PV = constant (at fixed T and n) - P= c(1/V); is a function of T and n For 1 mol of gas at 273 K, c= 22.414L - atm - Standard tem: 0C, and 1 atm - Small deviations at high P and small V due to gases beng real - As gases start have contact with one another, they behavior differently - Low pressures: satified exactly: 1 atm: small correcttons - High pressure: substantial corrections needed Charles Law:

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Unformatted text preview: - Response of gas to temperature: All gases at low P expand by same relative amount (for a given Tf and Ti) Avogadro's Law : " Equal volumes of different gases at the same temp and pressure contain equal numbers of particles" but he didn't specify what these "particles" were Bolye: PV = constant Charles: V/T = constant Avogadro: V/n = constant PV/nT= constant = R microscopic principle: Clausius, Maxwell, Boltzmann, invented kinetic molecular theory, a model based on physis 4 principles: 1. Pure gas = large # of molecules where distance between is much greater than size. 2. movement is in random direction, linear, distrib of speeds. 3. No attractive or repulsive forces exerted (const velocity on passing), point charge has no mass, massless panmpom 4. collisions are elastic (no net energy) if gas molecules attract each other, pressure goes down...
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