Untitled - Kelly Walsh High School

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Gases 85 Don’t Forget! Quick Tip Don’t Forget! Now you can use the reaction stoichiometry to convert from moles O 2 to moles KClO 3 and then to grams KClO 3: (0.021486 mol O 2 )a 2 mol KClO 3 3 mol O 2 ba 122.55 g KClO3 b 1.7554 1.76g KClO3 1 mol KClO3 Check to make sure that your answer is reasonable. In this case, for example, the mass of the KClO 3 must be less than the mass of the impure mixture. Another useful relationship is one derived from Avogadro’s law: 1 mol of any gas occupies 22.4 L at STP (standard temperature and pressure of 0 o C (273 K) and 1 atm). If you can find the volume at STP, you can then convert it to moles using this relationship and then to grams, if needed. Be sure when using any of the gas laws that you are dealing with gases, not liquids or solids. If the value 22.4 L/mol is used, make sure that it is applied to a gas at STP.
86 CHEMISTRY FOR THE UTTERLY CONFUSED 5-3 The Kinetic-Molecular Theory of Gases The kinetic-molecular theory (KMT) represents the properties of gases by modeling the gas particles themselves at the microscopic level. The KMT assumes that: • Gases are composed of very small particles, either small molecules or individual atoms. • The gas particles are so tiny in comparison to the distances between them, that the KMT assumes the volume of the gas particles themselves is negligible. • The gas particles are in constant motion, moving in straight lines in a random fashion and colliding with each other and the inside walls of the container. These collisions with the inside container walls comprise the pressure of the gas. • KMT assumes that the gas particles neither attract nor repel each other. They may collide with each other, but if they do, it assumes the collisions are elastic—no kinetic energy is lost, only transferred from one gas molecule to another. • Finally, the KMT assumes that the average kinetic energy of the gas is proportional to the Kelvin temperature. A gas that obeys all of these conditions is an ideal gas. Using the KMT, we can derive several quantities related to the properties of the gas particles. First, KMT qualitatively describes the motion of the gas particles. The average velocity of the gas particles is the root mean square velocity and has the symbol u rms. This is a special type of average speed. It is the average speed of a gas particle having the average kinetic energy. We can represent it as: where u rms 23RT/M R is a molar (ideal) gas constant of 8.314 J/mol·K (8.314 kg·m 2 /s 2 ·mol·K) T is the Kelvin temperature M is the molar mass of the gas. These root mean speeds are very high. Hydrogen gas, H 2, at 20. o C has a value of approximately 2000 m/s.
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Chemistry for the Utterly Confused
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We would like to dedicate this book
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Contents ix Chapter 5 Gases 79 Do I
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Contents xi Get Started 146 10-1 Mo
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Contents xiii 15-4 pH 222 15-5 Acid
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Contents xv Chapter 20 Nuclear Chem
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CHAPTER 1 ◆◆◆◆◆◆◆◆
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Chemistry: First Steps 3 compound b
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Chemistry: First Steps 5 exact norm
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Chemistry: First Steps 7 We now nee
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Chemistry: First Steps 9 mathematic
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Chemistry: First Steps 11 we do not
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Chemistry: First Steps 13 19. How m
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CHAPTER 2 ◆◆◆◆◆◆◆◆
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Atoms, Ions, and Molecules 17 Caref
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Atoms, Ions, and Molecules 19 table
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Atoms, Ions, and Molecules 21 If a
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Atoms, Ions, and Molecules 23 Once
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Atoms, Ions, and Molecules 25 and n
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Atoms, Ions, and Molecules 27 1. Th
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Atoms, Ions, and Molecules 29 20. N
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CHAPTER 3 ◆◆◆◆◆◆◆◆
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Mass, Moles, and Equations 33 Caref
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Page 74 and 75: Aqueous Solutions 51 4-2 Solubility
Page 76 and 77: Aqueous Solutions 53 Don’t Forget
Page 78 and 79: Aqueous Solutions 55 Quick Tip Cert
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Page 86 and 87: Aqueous Solutions 63 Quick Tip Mg(N
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Page 104 and 105: Gases 81 Quick Tip Don’t Forget!
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Page 118 and 119: Gases 95 ANSWER KEY 1. PTotal PA
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Page 122 and 123: Thermochemistry 99 Quick Tip Don’
Page 124 and 125: Thermochemistry 101 Don’t Forget!
Page 126 and 127: Thermochemistry 103 C2H2(g) (5/2) O
Page 128 and 129: Thermochemistry 105 Quick Tip Some
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Page 132 and 133: Quantum Theory and Electrons 109 Al
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Page 144 and 145: Periodic Trends 121 8-2 Ionization
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Page 152 and 153: Chemical Bonding 129 Quick Tip In S
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Chemical Bonding 135 Don’t Forget
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Chemical Bonding 137 9-6 Bond Energ
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Chemical Bonding 139 Quick Tip invo
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Chemical Bonding 141 Quick Tip Elem
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Chemical Bonding 143 11. a 12. b 13
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CHAPTER 10 ◆◆◆◆◆◆◆◆
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Molecular Geometry and Hybridizatio
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CHAPTER 11 ◆◆◆◆◆◆◆◆
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Intermolecular Forces, Solids and L
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CHAPTER 12 ◆◆◆◆◆◆◆◆
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Solutions 173 ways of expressing th
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Solutions 175 Don’t Forget! Don
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Solutions 177 12-3 Colligative Prop
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Solutions 179 Just as the freezing
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Solutions 181 Don’t Forget! Using
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Solutions 183 Quick Tip A molar mas
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Solutions 185 3. All methods of num
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CHAPTER 13 ◆◆◆◆◆◆◆◆
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Kinetics 189 4. Physical state of r
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Kinetics 191 Don’t Forget! consta
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Kinetics 193 Don’t Forget! the co
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Kinetics 195 Quick Tip Careful! Rem
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Kinetics 197 The decomposition of h
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Kinetics 199 reaction is first orde
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Kinetics 201 energy of a reaction.
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CHAPTER 14 ◆◆◆◆◆◆◆◆
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Chemical Equilibria 205 Quick Tip D
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Chemical Equilibria 207 14-3 Le Ch
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Chemical Equilibria 209 Given the f
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Chemical Equilibria 211 Careful! Do
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Chemical Equilibria 213 Quick Tip F
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Chemical Equilibria 215 Quick Tip I
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Chemical Equilibria 217 10. Write K
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CHAPTER 15 ◆◆◆◆◆◆◆◆
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Acids and Bases 221 Don’t Forget!
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Acids and Bases 223 The pH of pure
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Acids and Bases 225 Quick Tip Quick
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Acids and Bases 227 15-7 Lewis Acid
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Acids and Bases 229 We do not have
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Acids and Bases 231 Quick Tip We ne
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Acids and Bases 233 2. Alkali metal
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CHAPTER 16 ◆◆◆◆◆◆◆◆
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Buffers and Other Equilibria 237 we
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Buffers and Other Equilibria 239 Do
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Buffers and Other Equilibria 241 16
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Buffers and Other Equilibria 243 Qu
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Buffers and Other Equilibria 245 Qu
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Buffers and Other Equilibria 247 pK
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Buffers and Other Equilibria 249 Th
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CHAPTER 17 ◆◆◆◆◆◆◆◆
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Entropy and Free Energy 253 17-2 En
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Entropy and Free Energy 255 17-5 Ut
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Entropy and Free Energy 257 Quick T
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Entropy and Free Energy 259 Be Care
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Entropy and Free Energy 261 Before
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Entropy and Free Energy 263 ANSWER
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CHAPTER 18 ◆◆◆◆◆◆◆◆
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Electrochemistry 267 Quick Tip Some
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Electrochemistry 269 Don’t Forget
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Electrochemistry 271 We can use thi
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Electrochemistry 273 do is reverse
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Electrochemistry 275 Don’t Forget
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Electrochemistry 277 Be Careful! Th
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Electrochemistry 279 ANSWER KEY 1.
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CHAPTER 19 ◆◆◆◆◆◆◆◆
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Chemistry of the Elements 283 19-2
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Chemistry of the Elements 285 Be Ca
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Chemistry of the Elements 287 Don
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Chemistry of the Elements 289 6. Wh
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CHAPTER 20 ◆◆◆◆◆◆◆◆
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Nuclear Chemistry 293 The sum of th
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Nuclear Chemistry 295 Don’t Forge
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Nuclear Chemistry 297 that is not a
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Nuclear Chemistry 299 Don’t Forge
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Nuclear Chemistry 301 t 1/2 (ln 2)
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Nuclear Chemistry 303 1. A typical
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CHAPTER 21 ◆◆◆◆◆◆◆◆
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Organic, Biochemistry, and Polymers
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Index 327 chemical formulas, 19-21
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Index 329 Gibbs free energy (G), 25
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Index 331 octet rule, 128, 135, 140
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Index 333 viscosity, 161 voltaic ce
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