Equations Test Review 2011
Name: ____________________________
Part 1: Balance and label type of reaction. (S = Synthesis, D = Decomposition, SR = Single
Replacement, DR = Double Replacement, C = Combustion).
1) ____Mg (s) + ____HCl (aq)  ____H2 (g) + ____MgCl2 (s)
Type of Reaction: ______
2) ____Fe (s) + ____O2 (g) ____Fe2O3 (s)
Type of Reaction: ______
3) ____C4H10 (g) + ____O2 (g) ____ CO2 (g) + ____H2O (l)
Type of Reaction: ______
4) ____Fe2O3 (s) + ____H2 (g) ____Fe (s) + ____H2O (l)
Type of Reaction: ______
5) ____Pb(NO3)2 (aq) + ____KI (aq)  ____PbI2 (s) + ____2KNO3 (aq)
Type of Reaction: ______
6) ____P4O10 (s) + ____H2O (l)  ____H3PO4 (s)
Type of Reaction: ______
Part 2: Complete and balance the following equations. Add states to both reactants and products.
1) ____Na
2) ____C3H6
+ ____H2O
_____________________________________________
+ ____O2
_____________________________________________
3) ____Co(HCO3)2
4) ____Ni
__________________________________________________
+ ____Al2(SO4)3
 _________________________________________
5) ____________________________________  ____HI
6) ____Mg
+ ____N2
7) ____Cu(OH)2
 ______________________________________________
 ____________________________________________________
8) __________________________________  ____Li2O + ____CO2
9) ____LiOH (aq) + ____NaNO3 (aq)  _______________________________________
10) ____H2SO4 (aq) + ____KOH (aq)  _______________________________________
11) ____Cl2
+ ____KI
_______________________________________________
12) ____AgNO3 (aq) + ____MgCl2 (aq)  ______________________________________
Part 3: Matching - Use options in box on right.
1)
2)
3)
4)
5)
6)
7)
8)
____ only one reactant
____ burning
____ use the activity series
____ can be by means of electrolysis
____ precipitate
____neutralization
____ only one product
____ usually forms CO2 + H2O
Use the following options (you may
use a choice more than once).
a) synthesis
b) decomposition
c) single replacement
d) double replacement
e) combustion
Part 4: Short Answer
1) What are 4 signs that a chemical reaction has occurred?
2) How would you determine if a solid metal will replace a metal ion in single replacement reactions?
3) When would you write “No Reaction” after combining two aqueous salt solutions?
4) How does law of conservation of mass apply to reactions?
5) From the following choices, circle the element that would be a diatomic:
Cl
N
F
Ca
Br
Na
H
Part 5: Net Ionic Reactions
Write the balanced equation, complete ionic equation, and net ionic equation for the reaction between
ammonium sulfide (aq) and iron (II) nitrate (aq).
Balanced Eqn: _________________________________________________________________________
Complete Ionic Equation: ________________________________________________________________
Net Ionic Equation: _____________________________________________________________________
Part 6: Lab Reactions/Demos
1) Write the balanced chemical equation for the decomposition of Nickel (II) Carbonate.
What gas is produced?
What test could be used to verify the type of gas produced?
2) Write the balanced chemical equation for the reaction of water and sulfur dioxide.
What indicator could be used to determine if an acid or base is formed?
What color should you see after adding the indicator to your product?
3) Write the balanced chemical equation for the reaction of copper (II) oxide with another compound to
produce a base.
What indicator could be used to determine if a base is actually formed?
What color should you see after adding the indicator to your product?
4) Write the balance chemical equation for the reaction of solid zinc with sulfuric acid.
What gas is produced?
What test could be used to verify the type of gas produced?