Download + _3__CO(g) --->__2__Fe(s) + _3__CO2(g)

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______________