Honors Chem I
Chemical Equation Review
Name _________________________________
#_______
1. Why must equations be balanced?
Matter can neither be created nor destroyed so the numbers of atoms for each element must be the
same on both sides of the equation. Balancing with coefficients makes the numbers equal.
2. What can give evidence that a chemical reaction has occurred?
Production of light, heat, a gas, a precipitate, or a color change
3. What are hydrocarbons?
Compounds mostly consisting of hydrogen anf carbon
Place the correct coefficients in the blanks provided to balance the following equations.
4.
__2__ Li
+
__2___ H2O
5.
_____ Mg(OH)2
6.
_____ Fe2O3
+
__3___ CO
7.
______ AlCl3
+
__4___ NaOH
8.
______ Fe2(SO4)3
9.
__8____ O2
10.
______ C2H6O
+
11
__4___ Fe
+
12.
__2___ Ho
+
13.
_____ C6H12O6
+
+

__2___ LiOH

_____ H2SO4

__3___ BaCl2
+
_____ NaAlO2

_____ Sb2O4
___3__ O2

__2___ CO2
__3___ O2

__2___ Fe2O3
__6___ H2O

___2__ Ho(OH)3
__6___ O2

__3___ NaCl
+
+
+
___2__ H2O
__3___ CO2
__2___ FeCl3

+
+
+
__2___ SbS3
+
_____ H2
_____ MgSO4
___2___ Fe

+
__3___ BaSO4
___6__ SO2
__3___ H2O
__6___ CO2
+
+
__3___ H2
+
__6___ H2O
__2___ H2O
14.
__2___ Re
+
__3___ Br2

__2___ ReBr3
15.
_____ PCl5
+
___4__ H2O

_____ H3PO4
16.
_____ Cl2O7
+
_____ H2O

__2___ HClO4
17.
_____ Al4C3
+
__12___ H2O

__4___ Al(OH)3
18.
_____ Ca3P2
19.
__2___ C2H6O
+

__6___ H2O
+
_____ O2

+
___5__ HCl
+
___3__ CH4
___3___ Ca(OH)2
__2___ C2H4O
+
+
__2___ PH3
___2__ H2O
Write the equations from each of the following word equations. Make sure to include state symbols, such as
(g), where indicated. Balance the equations.
20.
Aluminum metal reacts with hydrochloric acid (HCl) to yield aluminum chloride and hydrogen gas.
2 Al + 6 HCl  2 AlCl3 + 3 H2 (g)
21.
Calcium hydroxide reacts with phosphoric acid (H3PO4) to yield calcium phosphate and water
3 Ca(OH)2 + 2 H3PO4  Ca3(PO4)2 + 6 H2O
22.
Copper metal react with sulfuric acid (H2SO4) to yield copper (II) sulfate and water and sulfur
dioxide
Cu + 2 H2SO4  CuSO4 + 2 H2O + SO2
23.
Hydrogen gas reacts with nitrogen monoxide to yield water and nitrogen gas
2 H2 (g) + 2 NO  2 H2O + N2 (g)
24.
Cesium hydroxide reacts with sodium iodide to yield sodium hydroxide and cesium iodide
CsOH + NaI  NaOH + CsI
25.
Manganese (IV) chloride reacts with calcium metal to yield calcium chloride and manganese metal
MnCl4 + 2 Ca  2 CaCl2 + Mn
26.
Copper (II) phosphate reacts with chromium (III) oxide to yield copper (II) oxide and chromium (III)
phosphate
Cu3(PO4)2 + Cr2O3  3 CuO + 2 CrPO4
27.
Sodium iodate reacts with gallium (III) hydroxide to yield sodium hydroxide and gallium (III) iodate
3 NaIO3 + Ga(OH)3  3 NaOH + Ga(IO3)3
28.
Heptane(C7H16) reacts with oxygen gas to yield carbon dioxide and water
C7H16 + 11 O2  7 CO2 + 8 H2O
In the blank to the left indicate the type of reaction then predict the products for each. If no reaction occurs then
write N.R. after the arrow. For the reactions that occur be sure to balance the final equation. Write in the
reactants for the word reactions.
29. _double replacement_____
FeCl2
+
30. _decomposition_________
2 AlCl3
31. _single replacement____
Zinc
+
Zn
+
32. _synthesis___________
3 Sr
+
33. _combustion_________
2 C4H10
+
34. _single replacement_____
Br2
CaF2

+

Na2S
FeS (s) + 2 NaCl (aq)
2 Al + 3 Cl2
Lead (II) Chromate

PbCrO4

ZnCrO4 + Pb
 Sr3N2
N2
13 O2

 N.R.
8 CO2 + 10 H2O
35. _decomposition_______

2 NaH
36. _combustion__________
2 C7H15OH
37. _double replacement ____
Fe(NO3)3
+
38. _synthesis______________
4 Ag
O2
39. _double replacement_____
Cu(NO3)2
40. _decomposition_________
2 NaBr
41. _single replacement_____
Nickel
+
Ni
42. _synthesis_____________

Sodium hydride
Zr
+

3 NaOH

Fe(OH)3 (s) + 3 NaNO3 (aq)
 2 Ag2O
Na2S
 CuS + 2 NaNO3
2 Na + Br2
Chromium (II) Hydroxide
+
+
 14 CO2 + 16 H2O
21 O2
+
+
2 Na + H2

Cr(OH)2

O2

N.R.
(use Ni+3 if rxn occurs)
ZrO2
(use Zr+4)
43. _combustion__________
C12H22O11
+
12 O2
 12 CO2 + 11 H2O
In the following redox reactions determine the elements oxidized/reduced and place your response in the
spaces provided.
44.
45.
C2H6 +
O2

CO2 +
C = -3
O=0
C = +4
H = +1
O = -2
Element oxidized:
_C (-3 to +4)____
H2O
H = +1
O = -2
Element reduced:
Fe(NO3)2

Ca(NO3)2
Fe = +2
Ca = +2
N = +5
N = +5
O = -2
O = -2
Element oxidized:
_Ca (0 to +2)____
Ca
+
Ca = 0
+
_O (0 to -2)____
Fe
Fe = 0
Element reduced:
_Fe (+2 to 0)____
In the spaces provided correctly write the molecular equation, ionic equation, and net ionic equation from the
given reactants.
46.
Molecular Eqn.:(be sure to balance your final result and include state symbols for all products)
__2__ Cr(NO3)3 (aq)
+
__3__ (NH4)2CO3 (aq)  Cr2(CO3)3 (s) + 6 NH4NO3 (aq)
Ionic Eqn.:
-
-
2 Cr+3 (aq) + 6 NO3 (aq) + 6 NH4+ (aq) + 3 CO3-2 (aq)  Cr2(CO3)3 (s) + 6 NH4+ (aq) + 6 NO3 (aq)
Net Ionic Eqn.:
2 Cr+3 (aq) + 3 CO3-2 (aq)  Cr2(CO3)3 (s)
47.
Molecular Eqn.:
____ Na3PO4 (aq)
+
_3___ CsF (aq)

3 Na F (aq) + Cs3PO4 (aq)
Ionic Eqn.:
-3
-3
3 Na+ (aq) + PO4 (aq) + 3 Cs+ (aq) + 3 F- (aq)  3 Na+ (aq) + 3 F- (aq) + 3 Cs+ (aq) + PO4 (aq)
Net Ionic Eqn.: No Reaction
48.
Molecular Eqn.:
_2___ NH4Cl (aq) + _____ Pb(C2H3O2)2 (aq)
 2 NH4C2H3O2 (aq) + PbCl2 (s)
Ionic Eqn.:
-
2 NH4+ (aq) + 2 Cl (aq) + Pb+2 (aq) + 2 C2H3O2- (aq)  2 NH4+ (aq) + 2 C2H3O2- (aq) + PbCl2 (s)
Net Ionic Eqn.:
-
2 Cl (aq) + Pb+2 (aq)  PbCl2 (s)