Equations Problem
Set /50 Brandon Jansen
Block: D
CLASSIFYING EQUATIONS: (/7)
1. Classify each reaction as a synthesis (S), decomposition
(D), single replacement (SR), double replacement (DR), or combustion (C)
reaction.
|
Reaction
|
 
Classification
  |
|
|
a.
|
Li + AlCl3 → Al + LiCl
|
SR
|
|
b.
|
NH3 → N2 + H2
|
  D |
|
c.
|
K + Br2 → KBr
|
S
|
|
d.
|
C10H22 + O2 → CO2 + H2O
|
  C |
|
e.
|
NH4OH + H2CO3 → H2O + (NH4)2CO3
|
C
|
|
f.
|
Zn + SnF4 → Sn + ZnF2
|
    SR |
|
g.
|
Ni + HCl → NiCl2 + H2
|
SR
|
|
h.
|
Au(CN)3 + Zn → Au + Zn(CN)2
|
    SR |
|
i.
|
O2 + Be → BeO
|
S
|
|
j.
|
FeCl3 + Na2SO3 → NaCl + Fe2(SO3)3
|
  DR |
|
k.
|
C8H18 + O2 → CO2 + H2O
|
  C |
|
l.
|
(NH4)2S + Mn(NO3)2 → NH4NO3 + MnS
|
DR
|
|
m.
|
Al2(SO4)3 + Na3PO4 → Na2SO4 + AlPO4
|
    DR |
|
n.
|
H3(PO4) + Cu(OH)2 → H2O + Cu3(PO4)2
|
  C |
SYNTHESIS: (/8)
1. Complete and balance each equation for a synthesis
reaction.
(a) 2 K + O2 → 2 KO
(b) 2 Ca + Cl2 → 2 CaCl
(c) 16 Cu+2 + S8 → 4 Cu2S8
(d) 4 Fe+3 + 3 O2 →
2 Fe2O3
2. Write a balanced chemical equation to represent each
reaction described below.
(a) Aluminum metal reacts with oxygen to form aluminum oxide.
2 Al + O3=Al2O3
(b) Metallic zinc combines with sulphur to form zinc sulphide.
Zn + S2= ZnS
DECOMPOSITION: (/8)
1.
Complete and balance each equation for a decomposition
reaction.
(a) NaCl → Na + Cl
(b) CaBr2 → Ca + 2 Br
(c) CCl4 → C + 4 Cl
(d) NCl3 → N + 3 Cl
(e) P4O10 → 4 P + 5 O2
2.
Write a balanced chemical equation to represent each reaction
described below.
(a)
Rubidium oxide decomposes into its elements.
2 RaO= 2 Ra + O2
(b)
Calcium chloride decomposes into its elements.
CaCl2=
Ca + 2 Cl
SINGLE REPLACEMENT: (/9)
1. Complete and balance each equation for a single replacement
reaction.
(a) K + H3PO4 → KPO4
+ H3
(b) Cl2 + MgBr2 → MgCl2 + Br2
(c) Br2 + KI →
KBr2
+ I
(d) 3 Mg+ Zn3(PO4)2 → Mg3(PO4)2
+ 3
Zn
(e) K + Al(NO3)3 → KNO3
+ Al
2. Write a balanced chemical equation to represent each
reaction described below.
(a) Silver reacts with Gold (III) nitrate.
Ag + Au(NO3)3
→
Ag(NO3)3 + Au
(b) Copper (II) reacts with lead (II) sulphate.
Cu + Pb(SO4)2
→
Cu(SO4)2
+ Pb
DOUBLE REPLACEMENT: (/9)
1. Complete and balance each equation for a double replacement
reaction.
(a) 2 Na2SO4 +
2 BaCl2 →
Ba2(SO4)2 + 4 NaCl
(b) 2 HNO3 + Ba(OH)2 → Ba(NO3)2 + 2 H2O
(c) 3 Na2CO3 +
2 Fe(NO3)3 → Fe2(CO3)3
+ 6 NaNO3
(d) 2 Al2(SO4)3 + 6 Ba(OH)2 → 3 Ba2(SO4)2
+ 4 Al(OH)3
(e) 2 NaOH + H2SO4 →
2 H2O
+ Na2SO4
2. Write a balanced chemical equation to represent each
reaction described below.
(a) Solutions of sodium hydroxide and hydrochloric acid
react.
NaOH + HCl → H2O + NaCl
(b) A silver nitrate solution reacts with a sodium chloride
solution.
AgNO3 + NaCl → NaNO3 + AgCl
COMBUSTION: (/9)
1. Complete and balance each equation for a combustion
reaction.
(a)
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
(b)
2 C2H6 + 7 O2 →
4 CO2 + 6 H2O
(c)
C6H12O6 +
8 O2 → 6 CO2 + 6 H2O
(d)
CH4+ 2 O2→ CO2 + 2 H2O
(a) Candle wax, C25H52, is burned to produce
carbon dioxide and water.
C25H52 + 38 O2 → 25 CO2
+ 26 H2O
(b) Sucrose, C12H22O11, is burned to produce
carbon dioxide and water.
C12H22O11 + 12 O2 → 12 CO2
+ 11 H2O
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