SCH 3U1
Types of Reactions
1.
2.
Identify each of the following reactions as a synthesis, decomposition, single
replacement, or double replacement reaction and balance each reaction.
a)
Mg(OH)2
+
HNO3 →
b)
H2O
SO3
→
c)
FeCl3
+
NaOH
d)
Cl2
+
ZnI2
e)
H2SO4
f)
+
→
Mg(NO3)2
+
H2SO4
Fe(OH)3
+
NaCl
→
ZnCl2
+
I2
+
Mg
→
MgSO4
K2O
+
H2O
→
KOH
g)
NaClO3
→
NaCl +
h)
AsCl3
H2S
→
As2S3
i)
Pb(NO3)2
→
PbO
+
j)
NaOH
H3PO4 →
+
+
H2 O
+
H2
O2
NO2
Na3PO4
+
HC1
+
O2
+
H2O
Predict the formula of the product in each of the following synthesis reactions,
then balance the chemical equation. General forms:
metal (s) + non-metal (s,l,g)
binary compound (s)
non-metal (s,l,g) + oxygen (g)
non-metal oxide (g)
metal (s) + water (l)
base (aq) + hydrogen (g)
metal oxide (s) + water (l)
base (aq)
non-metal oxide (g) + water (l)
oxyacid (aq)
a)
Li
+
O2
b)
P4
+
O2
Hint: product name is diphosphorus trioxide)
3.
c)
Mg
+
N2
d)
K2O
+
H2O
e)
SO2
+
H2O
Predict the products of and write balanced equations for, the following
decomposition reactions. The symbol “Δ” indicates heat must be added.
Δ
a)
Ag2O (s)
Δ
Hint: two elements
b)
CuCO3 (s)
Hint: a metal oxide + a common greenhouse gas
4.
5.
6.
7.
Write the balanced equation for the following single displacement reactions:
General forms:
metal (s) + water (l)
base (aq) + hydrogen (g)
metal (s) + acid (aq)
salt (aq) + hydrogen (g)
metal (s) + salt (aq)
metal (s) + salt (aq)
non-metal (s,l,g) + salt (aq)
salt (aq) + non-metal (s,l,g)
a)
Zn
+
Pb(NO3)2
b)
Mg
+
H2SO4
c)
Cl2
+
KI
d)
Rb
+
H2O
Compounds containing carbonates, sulfides and hydroxides are generally
insoluble in aqueous solutions (i.e. they form a precipitate), except those of with
alkali metal ions or ammonium ions. All compounds of the alkali metals and of
ammonium are soluble. Use this information to write balanced equations for the
following double displacement reactions. Indicate which product is the precipitate
and which is a solution using state symbols (s and aq).
a)
Na2CO3 (aq)
+
CuSO4 (aq)
b)
(NH4)2 SO4 (aq) +
CaCl2 (aq)
c)
KOH (aq)
+
Co(NO3)2 (aq)
d)
Na2S (aq)
+
Pb(NO3)2 (aq)
CuCO3 (s) + Na2SO4 (aq)
Write balanced equations for the following neutralization reactions. General
form: base + acid
salt + water
a)
Cu(OH)2 (aq)
+
HNO3 (aq)
b)
LiOH (aq)
+
H3PO4 (aq)
c)
Fe(OH)2 (aq)
+
H2SO3 (aq)
d)
Ca(OH)2 (aq)
+
HBr (aq)
Classify each reaction as endothermic or exothermic.
a)
b)
c)
d)
sodium chloride (s) +
energy
sodium (s) + chlorine (g)
hydrogen peroxide (aq)
hydrogen (g) + oxygen (g) + energy
C3H8 (g) + 5 O2 (g)
3 CO2 (g) + 4 H2O (g)
MgSO4•5H2O (s) + energy
MgSO4 (s) + 5H2O (g)