Chapter 11 Homework name:_____________________________________ 11.1: Describing Chemical Reactions Vocabulary: Define the following terms. Chemical Equation‐ Skeleton Equation‐ Catalyst‐ Coefficient‐ Balanced Equation‐ Law of Conservation of Mass‐ Practice Problems: 1. How do you write a word equation? 2. How do you write a skeleton equation? 3. Describe the steps in writing a complete balanced equation? 4. Write skeleton equations for these reactions. a. Heating copper(II) sulfide in the presence of diatomic oxygen produces pure copper and sulfur dioxide gas. b. When heated, baking soda (sodium hydrogen carbonate) decomposes to form the products sodium carbonate, carbon dioxide and water. 5. Write and balance equations for the following reactions. a. Iron metal and chlorine gas react to form solid iron(III) chloride. b. Solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas. c. Solid magnesium reacts with aqueous silver nitrate to form solid silver and aqueous magnesium nitrate. 6. Balance the following equations. a. SO2 + O2 Æ SO3
b. Fe2O3 + H2 Æ Fe + H2O c. P + O2 Æ P4O10
d. Al + N2 Æ AlN Chapter 11 Homework name:_____________________________________ 11.2: Types of Chemical Reactions Vocabulary: Define the following terms. Combination (synthesis) reaction‐ Decomposition reaction‐ Single‐replacement reaction‐ Double replacement reaction‐ Combustion‐ Activity series‐ Practice Problems: 1. What are the five types of chemical reactions? 2. What are the keys to predicting the products of the five general types of reactions? 3. Classify each reaction and balance the equations. a. C3H6 + O2 Æ CO2 + H2O b. Al(OH)3 Æ Al2O3 + H2O c. Li + O2 Æ LiO2
d. Zn + AgNO3 Æ Ag + Zn(NO3)2 4. Which of the five general types of reaction would most likely occur given each set of reactants? What are the probable products? a. an aqueous solution of two ionic compounds. b. a single compound c. two elements d. oxygen and a compound of carbon and hydrogen 5. Complete and balance an equation for each reaction. a. CaI2 + Hg(NO3)2 Æ b. Al + Cl2 Æ c. Ag + HCl Æ d. C2H2 + O2 Æ e. MgCl2 Æ f. H2O2 Æ 6. What are the three types of products that result from double replacement reactions? Chapter 11 Homework name:_____________________________________ 11.3: Reactions in Aqueous Solution Vocabulary: Define the following terms. Complete Ionic Equation‐ Spectator Ion‐ Net Ionic Equation‐ Precipitate‐ Practice Problems: 1. What is a net ionic equation? 2. How can you predict the formation of a precipitate in a double‐replacement reaction? 3. Write a balanced net ionic equation for each reaction. a. Pb(NO3)2(aq) + H2SO4(aq) Æ PbSO4(s) + HNO3(aq) b. Pb(C2H3O2)(aq) + HCl(aq) Æ PbCl2(S) + NH4NO3(aq) c. Na3PO4(aq) + FeCl3(aq) Æ NaCl(aq) + FePO4(s) d. (NH4)2S(aq) + Co(NO3)2(aq) Æ NH4No3(aq) 4. Write a balanced net ionic equation for each reaction. Identify the spectator ions in each reaction. a. HCl(aq) + AgNO3(aq) Æ b. Pb(C2H3O2)2(aq) + LiCl(aq) Æ c. Na3PO4(aq) + CrCl3(aq) Æ 5. Identify the precipitate formed when solution of these ionic compounds are mixed. a. H2SO4 + BaCl2 Æ b. Al2(SO4)3 + NH4OHÆ c. AgNO3 + H2S Æ d. CaCl2 + Pb(NO3)2 Æ e. Ca(NO3)2 + Na2CO3 Æ 6. Will a precipitate from when the following aqueous solutions of ionic compounds are mixed? a. AgNO3 and Na2SO4
b. NH4Cl and Ba(NO3)2
c. CaCl2 and K2SO4
d. Hg(NO3)2 and HCl