Media Portfolio

Chapter 12
Gases

12-02a-c

Title	Gases diffusing
Caption	Gases diffuse; they tend to flow spontaneously from a region of high concentration to a region of low concentration. (a) With the stopcock closed, no flow is possible. (b) With the stopcock open, there is a net flow of gases from the region of higher concentration on the left to the region of lower concentration on the right. (c) With the stopcock open, there is no net flow of gas once there is a uniform mixture and concentrations are equal.
Keywords	diffusion, spontaneous, concentration

12-03

Title	Pool table analogy
Caption	Gas molecules can be compared to billiard balls in random motion, bouncing off each other and off the sides of the pool table.
Keywords	pool table, analogy, random motion, billiard balls, kinetic theory

12-04

Title	Kinetic molecular theory
Caption	Orange particles of gas in 3D cube illusrate the kinetic molecular theory. According to the kinetic molecular theory, particles of a gas are in constant motion, occasionally bouncing off one another and off the walls of their container.
Keywords	random motion, kinetic theory, elastic, collision, assumptions

12-05

Title	Barometers
Caption	(a) A scientific laboratory barometer. (b) Schematic representation of a mercury barometer.
Keywords	barometer, pressure measurement, atmospheric, mercury

12-07

Title	Boyle's law demonstration
Caption	Boyle's law can be demonstrated by adding liquid mercury to the open end of a J-tube. As the pressure is increased by addition of mercury, the volume of the sample of trapped gas decreases. Gas pressure and volume are inversely related; one increases when the other decreases.
Keywords	Boyle, Boyle's law, J-tube, gas pressure, volume, inverse

12-08

Title	Effect of pressure on the volume of a gas
Caption	A diagram illustrating the effect of different pressures on the volume of a gas. The diagram demonstrates the behavior of a gas as described by Boyle's law. When the pressure on the gas is doubled, the volume is reduced by half.
Keywords	Boyle's law, gas pressure, volume, inverse

12-09

Title	Graph of gas volume versus pressure
Caption	The figure shows a graph of experimental data involving pressure and volume changes for a fixed sample of gas at constant temperature. The shape of the curve follows an inverse relationship. As pressure increases from 1 to 2 atmospheres, volume decreases from 60 to 30 mL. Compare the volumes at 3 atm and 6 atm of pressure.
Keywords	Boyle's law, graph, gas pressure, volume, inverse

12-10

Title	Bicycle tire and pump
Caption	A simple bicycle tire pump demonstrates Boyle's law. A pressure increase from P1 to P2 causes a volume decrease from V1 to V2. Pressure and gas volume are inversely related.
Keywords	Boyle's law, graph, gas pressure, volume, constant temperature, inverse, bicycle, tire pump, gas law

12-11

Title	Volume - temperature relationship for gases
Caption	The volume-temperature relationship for gases at constant pressure. Gas volume and temperature are directly proportional.
Keywords	Charles, constant pressure, volume, temperature, directly proportional, Kelvin, gas law

12-13a-c

Title	Obeying Gay-Lussac's law
Caption	(a) A pressurized can of hair spray or deodorant has a constant volume. Pressure increases as temperature increases. Heating the can could cause it to explode or rupture. (b) A can of food must be punctured or opened before (c) heating directly over a campfire. These examples illustrate Gay-Lussac's law; pressure and temperature are directly proportional.
Keywords	Gay-Lussac, pressure, temperature, constant volume, directly proportional, Kelvin, gas law

12-15

Title	Molar volume
Caption	The diagram shows a molar volume at STP in the form of a 1) cube and as 2) 5 gal. paint bucket plus 1 gal. The molar volume of any gas at STP is 22.4 L.
Keywords	molar volume, STP, 22.4 L

12-16

Title	Dalton's Law of partial pressures
Caption	The figure shows that the pressure of the pressure of the mixture of O2 and N2 (rightmost tank) is the sum of the pressures in the O2 and N2 tanks. Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressures exerted by each gas.
Keywords	Dalton's law, partial pressure, gas law

12-17ab

Title	Collecting gas by displacement of water
Caption	To collect a gas by displacement of water, the bottle is filled completely with water and inverted in a large vessel of water (a). As the gas to be collected is released into the bottle, gas bubbles rise to fill the bottle as water in the bottle is displaced. When the water levels inside and outside the bottle are equal, pressures inside and outside the bottle are also equal (b). At this point Patm=Pgas colected+Pwater vapor.
Keywords	displacenment of water, gas, collection, gas pressure

12-18

Title	Reaction of hydrogen gas with oxygen gas
Caption	The reaction of hydrogen gas with oxygen gas is shown. Two volumes of H2 react with one volume of O2 to give two volumes of water vapor. The total volume for reactants is 3, and the total volume for products is 2. Each volume contains the same number of molecules. The same numbers of hydrogen and oxygen atoms have been represented as reactants and as products. Atoms are neither created nor destroyed in chemical reactions.
Keywords	mole ratio, volume ratio, gas, hydrogen gas, oxygen gas, Gay-Lussac

12-19

Title	Reaction of carbon monoxide gas with oxygen gas
Caption	The reaction of carbon monoxide gas with oxygen gas. Two volumes of CO react with one volume of O2 to give two volumes of CO2. The total volume for reactants is 3, and the total volume for products is 2. Each volume contains the same number of melecules. Volume ratios and mole ratios are the same for the gases. Also, the same numbers of carbon and oxygen atoms have been represented as reactants and as products. Atoms are neither created nor destroyed in chemical reactions.
Keywords	mole ratio, volume ratio, gas, carbon monoxide, carbon dioxide, oxygen gas, Gay-Lussac

12-20

Title	Reaction of nitrogen gas with hydrogen gas
Caption	The reaction of nitrogen gas with hydrogen gas. One volume of N2 reacts with three volumes of H2 to give two volumes of NH3. The total volume for reactants is 4, and the total volume for products is 2. Each volume contains the same number of molecules. Volume ratios and mole ratios are the same for gases. Also, the same numbers of nitrogen and hydrogen atoms have been represented as reactants and as products. Atoms are neither created nor destroyed in chemical reactions.
Keywords	mole ratio, volume ratio, gas, nitrogen, hydrogen gas, ammonia

12-21

Title	Stoichiometric conversions for gases, liquids and solids
Caption	Stoichiometric conversions for gases, liquids, and solids. Conversion factors are shown alongside arrows.
Keywords	stoichiometric conversions, gas, liquid, solid, solution, ideal gas, molar volume

Title	Kinetic Energy in a Gas
Caption
Keywords

Title	P-V Relationships
Caption
Keywords

Title	Work of Gas Expansion
Caption
Keywords

Title	Diffusion of Bromine Vapor
Caption
Keywords

© 1995-2002 by Prentice-Hall, Inc.
A Pearson Company
Distance Learning at Prentice Hall
Legal Notice