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Determine the Type of Reaction for each equation. Then predict the products of each of the following chemical reactions. If a reaction will not occur, explain why not. Then Balance the equation. 1) __Ag2SO4 + __NaNO3 → Double Displacement No reaction because there is sulfate but it's paired with silver 2) __NaI + __CaSO4 → Double Displacement No reaction because there is sulfate and its paired with calcium 3) __HNO3 + __Ca(OH)2 → Acid base 4) __CaCO3 → Decomposition 5) __AlCl3 + __(NH4)PO4 → Double Displacement 6) __Pb + __Fe(NO3)3 → Single Displacement No because Lead is not as reactive as Iron. 7) __C3H6 + __O2 → Combustion 8) __Na + __CaSO4 → Double Displacement 105
The Learning Goal for this assignment is: Stoichiometry and Balancing Reactions Stoichiometry is a section of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data. In Greek, stoikhein means element and metron means measure, so stoichiometry literally translated means the measure of elements. In order to use stoichiometry to run calculations about chemical reactions, it is important to first understand the relationships that exist between products and reactants and why they exist, which require understanding how to balanced reactions. Balancing In chemistry, chemical reactions are frequently written as an equation, using chemical symbols. The reactants are displayed on the left side of the equation and the products are shown on the right, with the separation of either a single or double arrow that signifies the direction of the reaction. The significance of single and double arrow is important when discussing solubility constants, but we will not go into detail about it in this module. To balance an equation, it is necessary that there are the same number of atoms on the left side of the equation as the right. One can do this by raising the coefficients. Reactants to Products The students will learn how balanced chemical equations are used in stoichiometric calculations and how to calculate amounts of reactants and products in a chemical equation. A chemical equation is like a recipe for a reaction so it displays all the ingredients or terms of a chemical reaction. It includes the elements, molecules, or ions in the reactants and in the products as well as their states, and the proportion for how much of each particle is create relative to one another, through the stoichiometric coefficient. The following equation demonstrates the typical format of a chemical equation: 2Na(s) + 2HCl(aq) → 2NaCl(aq) + H2(g) In the above equation, the elements present in the reaction are represented by their chemical symbols. Based on the Law of Conservation of Mass, which states that matter is neither created nor destroyed in a chemical reaction, every chemical reaction has the same elements in its reactants and products, though the elements they are paired up with often change in a reaction. In this reaction, sodium (Na), hydrogen (H), and chloride (Cl) are the elements present in both reactants, so based on the law of conservation of mass, they are also present on the product side of the equations. Displaying each element is important when using the chemical equation to convert between elements. Stoichiometric Coefficients In a balanced reaction, both sides of the equation have the same number of elements. The stoichiometric coefficient is the number written in front of atoms, ion and molecules in a chemical reaction to balance the number of each element on both the reactant and product sides of the equation. These stoichiometric coefficients are useful since they establish the mole ratio between reactants and products. In the balanced equation: 2Na(s)+2HCl(aq)→2NaCl(aq)+H2(g) 106
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Chemistry Notebook Nedjie Jean-Fran
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Table E Selected Polyatomic Ions Fo
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Table H Vapor Pressure of Four Liqu
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Table K Common Acids Table N Select
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Table R Organic Functional Groups C
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Table S Properties of Selected Elem
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Table T Important Formulas and Equa
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CHEMISTRY EXAM FORMULA AND RESOURCE
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Activity Series of Metals Name Symb
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Unit 1 Measurement Lab Separation o
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Unit 5 (28 days) Chapter 10 Chemica
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30. Always lubricate glassware (tub
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7
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Print vs. print Online vs. online P
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To use the Stair-Step method, find
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Using SI Units Match the terms in C
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Standards of Measurement Fill in th
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SCIENTIFIC NOTATION RULES How to Wr
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Convert each number from Scientific
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Significant Figures Rules There are
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How Many Significant Digits for Eac
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The following rule applies for mult
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1qt=32 oz 1gal = 4qts 1.00 qt = 946
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Chapter 6 The Periodic Table The st
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Atoms Are Building Blocks Atoms are
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Electrovalence Don't get worried ab
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Summary 35
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Research the Scientist and summariz
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Electron Configuration Color the su
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Electron Configuration In order to
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10. Name __________________________
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Using Wikipedia, define the 8 categ
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Ionization Energy Define Ionization
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Ion Size Define Ion Size: Explanati
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The Nucleus A typical model of the
Page 75 and 76: Gamma Radiation After a decay react
Page 77 and 78: Nuclear Fission The word fusion mea
Page 79 and 80: Students will be able to predict sh
Page 81 and 82: This analysis shows that sodium has
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Page 85 and 86: 1 2 3 4 5 6 Name of Cation Calcium
Page 87 and 88: POLAR BONDING results when two diff
Page 89 and 90: Step 6 Put the atoms in the structu
Page 91: Orbitals Equation Lone Pairs Angle
Page 94 and 95: carbon dioxide Chemical Name CO 2 C
Page 96 and 97: hydronium Chemical Name H 3 O + Che
Page 98 and 99: Sulfur hexafluoride Chemical Name S
Page 100 and 101: Bent: They look, well, bent. Bond a
Page 102 and 103: 4. the chlorine atom in hydrochlori
Page 104 and 105: Chapter 23 Functional Groups The st
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Page 108 and 109: anched chains: Hexane - a 6-carbon
Page 110 and 111: Isomers Because carbon can bond in
Page 112 and 113: Chapter 12 Stoichiometry The studen
Page 114 and 115: Other atomic weights are listed on
Page 116 and 117: Find Molecular Mass 1- 10 1. NaBr 4
Page 118 and 119: Step 3 Always leave hydrogen and ox
Page 120 and 121: 1) ___ 2 NaNO3 + ___ PbO ___ Pb(NO
Page 122 and 123: 1) 2 NaNO3 + PbO Pb(NO3)2 + Na2O 2
Page 124 and 125: 4) Double displacement: This is whe
Page 128 and 129: we can determine that 2 moles of HC
Page 130 and 131: When there is no limiting reagent b
Page 132 and 133: Example 7 How much 5M stock solutio
Page 134 and 135: Theoretical and Actual Yields Key T
Page 136 and 137: Review Purposes To get an over
Page 138 and 139: Liters to Liters Define- Going from
Page 140 and 141: Chapter 14 The Behavior of Gases Th
Page 142 and 143: 13.1 The Nature of Gases Kinetic En
Page 144 and 145: Freezing Point- The temperature at
Page 146 and 147: It is important that you realize th
Page 148 and 149: 3. The pressure of nitrogen gas in
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Page 152 and 153: conduct an electric current in eith
Page 154 and 155: Create and interpret potential ener
Page 156 and 157: Structure effects: determines what
Page 158 and 159: Specific Heat Here is the definitio
Page 160 and 161: Step One: solid ice rises in temper
Page 162 and 163: Step Three: liquid water rises in t
Page 164 and 165: Step Five: steam rises in temperatu
Page 166 and 167: then it is exothermic, meaning the
Page 168 and 169: Define the types of reactions. Give
Page 170 and 171: 1. If this compound was at room tem
Page 172 and 173: 1. In what part of the curve would
Page 174 and 175: Reduction Oxidation reduction react
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So far, the properties have an obvi
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The acid base theory of Brønsted a
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IV. Problems with the Theory This t
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Let's discuss significant figures a
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On your calculator you would input
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Ag+ + Cu ---> Ag + Cu2+ I have deli
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7. Half Reactions A half-reaction i
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Notice that each separate substance
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