Kinetic-MolecularTheoryofGases.pdf

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Department
Chemistry
Course
CHE 2A
Professor
A N D R E A S T O U P A D A K I S
Semester
Winter

Description
February  10,  2014 V=k(1/p) V=k(t) V=k(n) but  not  explanations  why? led  to  empirical  law P(v)=n(R)(t) (ideal  gas  law) kinetic  model 1)assumptions 2)physic  laws 3)math  reasoning Qualitative  Model A-­great  number  of  molecules/atoms B-­Molecules  are  considered  point  masses C-­  are  in  ceaseless  random  motion D-­  do  not  interact  (no  attractive/repulsive  forces) E-­  Kinetic  energy  collides  and  transfers  from  particle  to  particle  BUT  its  not  transformed  to  other forms  of  energy  (elastic  collisions) Quantitative each  collision  gives  rise  to  brief  force  on  the  wall experience  an  almost  constant  force steady  pressure P=  ⅓(N/V)  mu^2  (mean  square  speed) N=number  of  molecules V=  volume  of  the  container  gas  occupies m=mass  of  one  molecule P=pressure Types  of  Average  Speed average  speed  -­  average  kinetic  energy -­Mean  Speed -­Mean  Square  Speed -­Root  mean  Square  Speed Most  Probable Speed  of  the  largest  number  of  particles appears  most  frequent urms=  sqrt  (3RT/M) U=sqrt  (8RT/nM) all  speeds  are  proporti
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