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Chemistry Honors Ch.11 Test Review: Chemical Reactions I. Name: ______ANSWER KEY ________ Balancing Equations: a. Please balance the following equations: ___Fe2O3(s) + _3__CO(g) --->__2__Fe(s) + _3__CO2(g) ___3__ NO2 + ___H2O ---> __2_HNO3 + ___NO __4_S2H5 + _13__O2 ---> __8__SO2 + _10__H2O __2_VO + __3__Fe2O3 ---> ___6_FeO + ___V2O5 b. Please write out the balanced chemical formulas for the following equations: Sulfuric acid and aluminum react to form aluminum sulfate and hydrogen gas: 3 H2SO4 + 2 Al Al2(SO4)3 + 3 H2 Calcium iodide and silver nitrate react to form calcium nitrate and silver iodide: CaI2 + 2Ag(NO3) Ca(NO3)2 + 2AgI Phosphoric acid and ammonium hydroxide react… (predict products and balance equation) H3PO4 + 3 NH4OH (NH4)3(PO4) + 3 H2O c. Challenge Problems: ___Ag2O + __2_NH4OH + __2_NH4NO3 ----> _2__[Ag(NH3)2]NO3 + ___3_H2O (balanced equation of pentanol) 2C5H12O + 15O2 ===> 10CO2 + 12H2O II. Classifying Reactions: a. Please write the following equations and classify the reactions: Chlorine gas and potassium bromide potassium chloride and bromine liquid Cl2 + 2KBr 2KCl + Br2 Single replacement Ammonium nitrate water and nitrogen oxide NH4NO3 2H2O + N2O Decomposition Lead (II) nitrate + potassium iodide lead (II) iodide + potassium nitrate Pb(NO3)2 + KI PbI2 + KNO3 Double replacement Iron + oxygen Iron (II) Oxide Fe + O2 FeO Synethsis b. Which major type of reaction is NOT a redox reaction? ___double replacement III. Single Replacement Reactions: a. Predict if the reaction will proceed. If so, write the balanced equation. 1. Lead + zinc acetate __________NR___________________________________________________________________________________ 2. Iron + aluminum oxide _____________NR________________________________________________________________________________ 3. Silver nitrate + nickel _________2AgNO3 + Ni Ni(NO3)2 + 2 Ag ___________________ 4. Aluminum bromide + chlorine ____________2AlBr3 + 3Cl2 2AlCl3 + 3Br2 _________________________ 5. Magnesium + nitric acid _____________Mg + 2HNO3 Mg(NO3)2 + H2 ________________________________________ 6. Silver + sulfuric acid ____________________NR_________________________________________________________________________ 7. Zinc + water ______________Zn + HOH NR __________ b. Please write the total ionic equations for the single replacement reaction that do occur. 1. Lead + zinc acetate _____________________________________________________________________________________________ 2. Iron + aluminum oxide _____________________________________________________________________________________________ 3. Silver nitrate + nickel ________2Ag+ (aq) + 2NO3- (aq) + Ni (s) Ni2+ (aq) + 2(NO3)- (aq) + 2 Ag (s) 4. Aluminum bromide + chlorine __________2Al3+ (aq) + 6Br- (aq) + 3Cl2 (g) 2Al3+ (aq) + 6Cl- (aq) + 3Br2 (g) 5. Magnesium + nitric acid ____________Mg (s) + 2H+ (aq) + 2NO3- (aq) Mg2+ (aq) + 2NO3- (aq) + H2 (g) 6. Silver + sulfuric acid _____________________________________________________________________________________________ 7. Zinc + water _____________________________________________________________________________________________ c. Please indicate which species is getting reduced and the number of electrons it gains for the reactions that do occur. 1. Lead + zinc acetate _____________________________________________________________________________________________ 2. Iron + aluminum oxide _____________________________________________________________________________________________ 3. Silver nitrate + nickel _ 2Ag+ + 2e- 2Ag 4. Aluminum bromide + chlorine 3Cl2 + 6e- 6Cl- ____________ 5. Magnesium + nitric acid 2H+ + 2e- H2 __________________________________ 6. Silver + sulfuric acid _____________________________________________________________________________________________ 7. Zinc + water _____________________________________________________________________________________________ IV. Double Replacement Reactions: a. Please write the balanced chemical equations for the following reactions with its state of matter. Indicate if the reaction occurs. 1. potassium bromide + silver nitrate silver bromide + potassium nitrate __________KBr (aq) + Ag(NO3) (aq) __> AgBr (s) + KNO3 (aq) 2. silver nitrate + potassium chromate silver chromate + potassium nitrate 2AgNO3 (aq) + K2CrO4 (aq) Ag2CrO4 (s) + 2KNO3 (aq) 3. ammonium chloride + cobalt (II) sulfate ____NO RXN___2NH4Cl (aq) + CoSO4 (aq) (NH4)2SO4 (aq) + CoCl2 (aq) 4. zinc acetate + cesium hydroxide _____ Zn(C2H3O2)2 (aq) + 2CsOH (aq) Zn(OH)2 (s) + 2Cs(C2H3O2) (aq) 5. lithium hydroxide + sodium chromate _____NO RXN_______2LiOH (aq) + Na2CrO4 (aq) Li2CrO4 (aq) + 2NaOH (aq) b. Write the total and net ionic equations for the following reactions. 1. potassium bromide + silver nitrate silver bromide + potassium nitrate ________Ag+(aq) + Br-(aq) AgBr (s) 2. silver nitrate + potassium chromate silver chromate + potassium nitrate ________2Ag+ (aq) + CrO42- (aq) Ag2CrO4 (s) _________ 3. ammonium chloride + cobalt (II) sulfate __________________________NR___________________________________________________________________ 4. zinc acetate + cesium hydroxide ____ Zn2+ (aq) + 2OH- (aq) Zn(OH)2 (s) ________________________________________________________________________________ 5. lithium hydroxide + sodium chromate _______________________________NR______________________________________________________________ c. Challenge problem: 1. Ammonium sulfate and potassium hydroxide react in a double replacement reaction. Write the balanced equation and its states of matter: ________(NH4)2SO4 (aq) + 2 KOH (aq) 2 NH4OH (aq) + K2(SO4) (aq) 2. Upon doing this reaction, you notice that this reaction DOES occur because one of your aqueous products can further decompose into a common liquid and gas. Please write the molecular formula, total ionic, and net ionic equations: MF: (NH4)2SO4 (aq) + 2 KOH (aq) 2 NH3 (g) + 2 H20 (l) + K2(SO4) (aq) Total Ionic: 2(NH4)+ (aq) + (SO4)2- (aq) + 2 K+ (aq) + 2(OH)- (aq) 2 NH3 (g) + 2 H20 (l) + 2K+ (aq) + (SO4)2- (aq) Net Ionic: 2(NH4)+ (aq) + 2(OH)- (aq) 2 NH3 (g) + 2 H20 (l) V. Culminating Problem: Add the following numbers: The number of total oxygen gas molecules from Part I: ___28_____________ + The number of synthesis reactions from Part II: ________1____________ + The total number of electrons gained in all successful reactions from Part III: _____10________ + The number of reactions that do NOT occur from Part IV: ______2_________________ = _________40______________