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CH10[1]

# CH10[1] - Chapter 10 Gases A B C D E Definitions Gas Laws...

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Chapter 10 Gases A. Definitions B. Gas Laws C. Ideal Gas Equation D. Kinetic Theory of Gases E. Deviations from Ideal Behavior HW #P5 Covered on Quiz #2 and Exam #2

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Chapter 10 Gases A. Definitions 1. Gas B molecules of a gas are not held together, expand to fill the space available and can be compressed. 2. Volume is the space occupied. 1 liter = 1 cubic decimeter 1 cc = 1 ml 1 Ρ = 1000 ml = 1000 cc 3. Temperature Scales Ε C = 5/9 ( Ε F B 32 Ε ) K = Ε C + 273.15 absolute zero in temperature is 0 K or B 273.15 Ε C
4. Pressure pressure is measured as a force acting on an area tires are pounds/in 2 We primarily use relative measures of pressure, since we are always surrounded by gases. A barometer at sea level will measure 760 mm of Hg. This is defined as 1 atm. 1 atm = 760 mm Hg also 1 mm Hg = 1 Torr STP (standard temperature and pressure) 1 atm (760 mm Hg) and 0 Ε C (273 K) P = F A kg - meter/s 2 m 2 scientific is which is a Pascal (Pa)

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Example: Convert 0.605 atm into pressure in Torr. B. Gas Laws 1. Pressure and Volume Relations B Boyle = s Law, Fig 10.7 Observation B for a given amount of air at constant temperature increasing pressure decreases the volume. 1 Ρ at 1 atm 0.5 Ρ at 2 atm Two Expressions PV = constant 2. Volume and Temperature Relations B Charles = Law Observation B demonstration for constant pressure V α T T is in Kelvin Charles = Law B At constant pressure the volume of a given quantity of gas is proportional to absolute temperature . 3. Quantity and Volume Relations B Avogadro = s Law Gay-Lussac = s combining volumes V α P 1
H 2 + Cl 2 !6 2 HCl 1 volume + 1 volume !6 2 volumes

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CH10[1] - Chapter 10 Gases A B C D E Definitions Gas Laws...

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