Untitled - Kelly Walsh High School

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CHAPTER 3 ◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆ Mass, Moles, and Equations ◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆◆ You should read this chapter if you need to review or learn about: ➜ Balancing chemical equations ➜ The mole concept ➜ Avogadro’s number Molar mass ➜ ➜ ➜ Reaction stoichiometry Limiting reactants ➜ Percent yield ➜ Empirical and molecular formulas ➜ Percent composition ➜ Working mole problems 31 Copyright © 2007 by John Moore and Richard Langley. Click here for terms of use.
32 CHEMISTRY FOR THE UTTERLY CONFUSED Get Started This is a critical chapter in your study of chemistry. Our goal is to help you master the mole concept. You will learn about balancing equations and the mole/mass relationships (stoichiometry) inherent in these balanced equations. You will learn, given amounts of reactants, how to determine which one limits the amount of product formed. You will also learn how to determine the empirical and molecular formulas of compounds. All of these will depend on the mole concept. Make sure that you can use your calculator correctly. If you are unsure about setting up problems, refer back to Chapter 1 of this book and go through Section 1-4, on using the Unit Conversion Method. Review how to find atomic masses on the periodic table. Practice, Practice, Practice. 3-1 Balancing Chemical Equations A chemical equation represents a chemical change that is taking place. On the left side of the reaction arrow are the reactants, the chemical substances that are changed. On the right of the reaction arrow are the reaction products, the new substances formed. Sometimes additional information appears above or below the reaction arrow. The Law of Conservation of Mass states that the total mass remains unchanged. This means that the total mass of the atoms of each element represented in the reactants must appear as products. In order to indicate this, we must balance the reaction. When balancing chemical equations, it is important to realize that you cannot change the formulas of the reactants and products; the only things you may change are the coefficients in front of the reactants and products. The coefficients indicate how many of each chemical species react or form. A balanced equation has the same number of each type of atom present on both sides of the equation and the coefficients are present in the lowest whole number ratio. For example, iron metal reacts with oxygen gas to form rust, iron(III) oxide. We may represent this reaction by the following balanced equation: 4 Fe(s) 3 O 2(g) l 2 Fe 2O 3(s) This equation tells us that 4 iron atoms react with 3 oxygen molecules to form 2 rust compounds. Note that the number of iron atoms and oxygen atoms are the same on both sides of the equation (2 Fe 2O 3 4 Fe and 6 O). Let’s see how we went about arriving at the balanced equation for the rusting of iron.
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Chemistry for the Utterly Confused
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Page 10 and 11: Contents ix Chapter 5 Gases 79 Do I
Page 12 and 13: Contents xi Get Started 146 10-1 Mo
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Page 16 and 17: Contents xv Chapter 20 Nuclear Chem
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Page 24 and 25: CHAPTER 1 ◆◆◆◆◆◆◆◆
Page 26 and 27: Chemistry: First Steps 3 compound b
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Page 36 and 37: Chemistry: First Steps 13 19. How m
Page 40 and 41: Atoms, Ions, and Molecules 17 Caref
Page 42 and 43: Atoms, Ions, and Molecules 19 table
Page 44 and 45: Atoms, Ions, and Molecules 21 If a
Page 46 and 47: Atoms, Ions, and Molecules 23 Once
Page 48 and 49: Atoms, Ions, and Molecules 25 and n
Page 50 and 51: Atoms, Ions, and Molecules 27 1. Th
Page 52 and 53: Atoms, Ions, and Molecules 29 20. N
Page 56 and 57: Mass, Moles, and Equations 33 Caref
Page 58 and 59: Mass, Moles, and Equations 35 Quick
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Page 66 and 67: Mass, Moles, and Equations 43 the b
Page 68 and 69: Mass, Moles, and Equations 45 7. Th
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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
Page 80 and 81: Aqueous Solutions 57 Quick Tip Quic
Page 86 and 87: Aqueous Solutions 63 Quick Tip Mg(N
Page 88 and 89: Aqueous Solutions 65 All the separa
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Gases 81 Quick Tip Don’t Forget!
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Gases 83 Quick Tip Let’s see how
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Gases 85 Don’t Forget! Quick Tip
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Gases 87 Second, the KMT relates th
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Gases 89 The larger the gas particl
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Gases 91 Note that the mandatory co
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Gases 93 If it was not clear before
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Gases 95 ANSWER KEY 1. PTotal PA
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CHAPTER 6 ◆◆◆◆◆◆◆◆
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Thermochemistry 99 Quick Tip Don’
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Thermochemistry 101 Don’t Forget!
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Thermochemistry 103 C2H2(g) (5/2) O
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Thermochemistry 105 Quick Tip Some
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CHAPTER 7 ◆◆◆◆◆◆◆◆
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Quantum Theory and Electrons 109 Al
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Quantum Theory and Electrons 111 Th
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Quantum Theory and Electrons 113 Do
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Quantum Theory and Electrons 115 Do
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Quantum Theory and Electrons 117 AN
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CHAPTER 8 ◆◆◆◆◆◆◆◆
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Periodic Trends 121 8-2 Ionization
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Periodic Trends 123 The general tre
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Periodic Trends 125 in its ground s
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CHAPTER 9 ◆◆◆◆◆◆◆◆
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Chemical Bonding 129 Quick Tip In S
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Chemical Bonding 131 9-3 Ionic Bond
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Chemical Bonding 133 Quick Tip Neve
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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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Untitled - Kelly Walsh High School

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