CHEM 131 Lecture Notes - Lecture 22: Ideal Gas Law, Ideal Gas, Intermolecular Force
17 Nov 2016
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Properties of gas: neither definite shape of volume, uniformly fills any container, exerts pressure on all surroundings-collisions, changes volume with temperature, pressure, number of moles, miscible- mix together. One can visualize it as a collection of perfectly hard spheres which collide but which otherwise do not interact with each other. The relationship between them may be deduced from kinetic theory and is called the. Pressure: force per unit area p=f/a, si units- newton/meter2=1pascal (pa, 1atm=29. 92 hg=1bar=760torr=14. 7psi=101,325pa, atmospheric pressure (patm)- the force exerted on the surface of the earth due to weight of atmosphere, atmospheric pressure decreases with increasing altitude. Dalto(cid:374)"s la(cid:449) of partial pressures: total pressure- sum of the individual pressures, pi-partial pressure of a gas i, for a (cid:448)olu(cid:373)e of a gas of at(cid:373)ospheric co(cid:373)positio(cid:374) at stp ptotal=pat(cid:373)+p(cid:1005)+p(cid:1006) . A(cid:448)agadro"s la(cid:449)- equal volumes of ideal gases at same temperature and pressure contain the same number of moles.
