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Chemistry - The Central Science Chapter 10

# Chemistry - The Central Science Chapter 10 - Chapter 10...

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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 #P7 - 10.26, 10.31, 10.44, 10.45, 10.47, 10.51, 10.54, 10.57, 10.80, 10.111 Covered On Quiz #4 and Exam 2

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Chapter 10 Gases A. Definitions 1. Gas 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 R = 1000 ml = 1000 cc 3. Temperature Scales E C = 5/9 ( E F – 32 E ) K = E C + 273.15 absolute zero in temperature is 0 K or –273.15 E C
P = F A kg - meter/s 2 m 2 scientific is which is a Pascal (Pa) 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 E C (273 K)

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V α P 1 Example: Convert 0.605 atm into pressure in Torr. B. Gas Laws 1. Pressure and Volume Relations – Boyle’s Law Observation – for a given amount of air at constant temperature increasing pressure decreases the volume. 1 R at 1 atm 0.5 R at 2 atm Two Expressions PV = constant
2. Volume and Temperature Relations – Charles’ Law Observation – demonstration for constant pressure V α T T is in Kelvin Charles’ Law – At constant pressure the volume

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Chemistry - The Central Science Chapter 10 - Chapter 10...

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