5 Outline - Chapter 5 Chemistry Outline Lecture Ch. 5 Gases...

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Chapter 5 Chemistry Outline Lecture Ch. 5 Gases Chem behavior is based upon comp but all gases have many phys similarities Pressure = Force/Area Barometer- measures atmospheric pressure Gas Laws- Physical behavior of gases is defined by four variables, P V T n Boyle’s Law- (T and n constant) P1V1 = P2V2 Charles’s Law = (P and n are fixed) V1/T1 = V2/T2 (T in Kelvin) Avogadro’s Law = (P and T fixed) V1/n1 = V2/n2 Standard Molar Volume At STP (0 C and 1 atm) 1 mol of any gas occupies 22.4141 L Combined Gas Laws PV = nRT R = the universal gas constant Molar Mass and density m/v = P MM / RT = d Dalton’s Law of partial pressure Each gas in a mixture exerts a partial pressure Total Pressure = the sum of the partial pressures Mole Fraction, X Find portion chem entity makes up in eq’n and multiply by total pressure to find partial pressure Kinetic Molecular Theory Postulates – Volume of a gas is neglible, Gas particles are in constant, random, straight-line motion; gas particles collisions are elastic, total kinetic energy is constant
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Average Kinetic energy and speed AKE = .5 m u^2 Figures 5.13-5.16 KE is prop to T KE = .5mu^2 u is for speed KE (nrg/mol) depends on T Total KE also depends on the number of moles. NRG is an extensive property.
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This note was uploaded on 04/28/2008 for the course CHEM 1111 taught by Professor Robertparson during the Fall '08 term at Colorado.

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5 Outline - Chapter 5 Chemistry Outline Lecture Ch. 5 Gases...

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