H CH 9 Homework
1. iron + sulfur  iron (II) sulfide
1-1-1; synthesis
2. silver nitrate + sodium bromide  sodium nitrate + silver bromide
1-1-1-1; double replacement
3. potassium chlorate  potassium chloride + oxygen
2-2-3; decomposition
4. butane (C4H10) + oxygen  carbon dioxide + water
2-13-8-10; combustion
5. potassium iodide + lead (II) nitrate  lead (II) iodide + potassium nitrate
2-1-1-2; double replacement
6. aluminum + oxygen  aluminum oxide
4-3-2; synthesis
7. magnesium chloride + ammonium nitrate  magnesium nitrate + ammonium
1-2-1-2; double replacement
chloride
8. sodium peroxide + water  sodium hydroxide + oxygen
2-2-4-1; none
9. ferric chloride + potassium hydroxide  potassium chloride + ferric hydroxide
1-3-3-1; double replacement
10. aluminum + sulfuric acid  aluminum sulfate + hydrogen
2-3-1-3; single replacement
11. sodium carbonate + calcium hydroxide  sodium hydroxide + calcium carbonate
1-1-2-1; double replacement
12. carbon dioxide + water  carbonic acid
1-1-1; synthesis
13. sodium + water  sodium hydroxide + hydrogen
2-2-2-1; single replacemnt
14. zinc + sulfuric acid  zinc sulfate + hydrogen
1-1-1-1; single replacement
15. aluminum sulfate + calcium hydroxide  calcium sulfate + aluminum hydroxide
1-3-3-2; double replacement
16. calcium oxide + water  calcium hydroxide
1-1-1; synthesis
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17. iron + cuprous nitrate  ferrous nitrate + copper
1-2-1-2 SR
18. iron (II) sulfide + hydrochloric acid  hydrogen sulfide + iron (II) chloride
1-2-1-1 dr
19. potassium oxide + water  potassium hydroxide
1-1-2 Syn
20. octane (C8H18) + oxygen  carbon dioxide + water
2-25-16-18 Comb
21. potassium hydroxide + phosphoric acid  potassium phosphate + water
3-1-1-3; neutralization
22. calcium chloride + nitric acid  calcium nitrate + hydrochloric acid
1-2-1-2
23. magnesium hydroxide + sulfuric acid  magnesium sulfate + water
1-1-1-2; neutralization
24. phosphorous + oxygen  phosphorous pentoxide
2-5-2
25. sodium carbonate + hydrochloric acid  sodium chloride + water + carbon
1-2-2-1-1
dioxide
26. magnesium + nitric acid  magnesium nitrate + hydrogen
1-2-1-1
27. calcium carbonate  calcium oxide + carbon dioxide
1-1-1
28. ammonia (NH3) + sulfuric acid  ammonium sulfate
2-1-1
29. magnesium chloride + fluorine  magnesium fluoride + chlorine
1-1-1-1
30. fluorine + sodium hydroxide  sodium fluoride + oxygen + water
2-4-4-1-2
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Now, try these!!!
1. ZnSO4 + KI + KIO3 + H2O  Zn5(OH)8SO4 + K2SO4 + I2
15-20-4-12-3-12-12
2. K2SeO3 + KI + HCl  KCl + Se + I2 + H2O
1-4-6-6-1-2-3
3. KIO3 + KI + HCl  KCl + I2 + H2O
1-5-6-6-3-3
4. FeCl2 + K2Cr2O7 + HCl  FeCl3 + KCl + CrCl3 + H2O
6-1-14-6-2-2-7
5. Cr2(SO4)3 + KMnO4 + H2O  H2CrO4 + MnSO4 + K2SO4 + H2SO4
5-6-16-10-6-3-6
6. HBO2 + KIO3 + KI  KBO2 + H2O + I2
6-1-5-6-3-3
5) from SO4  G =3a-3 sub into H
from H  c = d + (3a-3)
from O  8 + c = 4d sub into H giving 4d – 8 = d + 3a -3
from Cr  since 2a=d you get 8a – 8 = 2a + 3a – 3 therefore a =5/3
Oxidation/Reduction:
Identify the species in each reaction that have been oxidized and reduced and write the
half reaction.
1. FeCl3 + SnCl2  FeCl2 + SnCl4
Fe+3 + e-  Fe+2 (reduced); Sn+2  Sn+4 + 2 e- (oxidized)
2. SbCl5 + KI  SbCl3 + KCl + I2
Sb+5 + 2 e-  Sb+3 (reduced); I-1  I20 + e- (oxidized)
3. CdS + I2 + HCl  CdCl2 + HI + S
I20 + e-  I-1 (reduced); S-2  S0 + 2 e- (oxidized)
4. H2SO3 + I2 + H2O  H2SO4 + HI
I20 + e-  I-1 (reduced); S+4  S+6 + 2 e- (oxidized)
5. NaClO + H2S  NaCl + H2SO4
Cl+1 + 2 e-  Cl-1 (reduced); S-2  S+6 + 8 e- (oxidized)
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Reaction Prediction:
Identify the type of reaction, predict the products, balance the equation, and tell if the
reaction will take place or not.
1. aluminum + hydrochloric acid 
2 Al + 6 HCl  2 AlCl3 + 3 H2 ; single replacement; yes
2. calcium hydroxide + nitric acid 
Ca(OH)2 + 2 HNO3  Ca(NO3)2 + 2 HOH ; neutralization; yes
3. methane (CH4) + oxygen 
CH4 + 2O2  CO2 + 2 H2O ; combustion
4. aluminum + oxygen 
4Al + 3O2 2Al2O3
5. zinc chloride + hydrogen sulfide 
ZnCl2 + H2S  ZnS + 2 HCl ; double replacement; yes
6. dinitrogen pentoxide + water 
N2O5 + H2O  2 HNO3 ; synthesis
7. silver chloride + bromine 
2 AgCl + Br2  2 AgBr + Cl2 ; single replacement; NR
8. sodium chlorate 
2 NaClO3  2 NaCl + 3 O2 ; decomposition
9. barium nitrate + sodium chromate 
Ba(NO3)2 + Na2CrO4  BaCrO4 + 2 NaNO3 ; double replacement; yes
10. zinc carbonate 
ZnCO3  ZnO + CO2; decomposition
11. calcium phosphate + aluminum sulfate 
Ca3(PO4)2 + Al2(SO4)3  3 CaSO4 + 2 AlPO4; double replacement; yes
12. potassium + fluorine 
2 K + F2  2 KF; synthesis
13. copper + sulfuric acid 
Cu + H2SO4  CuSO4 + H2; single replacement; no
14. lithium oxide + water 
Li2O + H2O  2 LiOH; synthesis
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15. strontium chloride (electrolyzed) 
SrCl2  Sr + Cl2; decompositon
16. magnesium carbonate + phosphoric acid 
3 MgCO3 + 2 H3PO4  Mg3(PO4)2 + 3 H2CO3; double replacement ; yes
17. propane (C3H8) + oxygen 
C3H8 + 5 O2  3 CO2 + 4 H2O; combustion
18. lead + potassium chlorate 
Pb + 2 KClO3  Pb(ClO3)2 + 2 K; single replacement; NR
19. calcium carbonate + lithium chloride 
CaCO3 + 2 LiCl  Li2CO3 + CaCl2; double replacement; ?
20. potassium nitrate 
4 KNO3  2 K2O + 2 N2 + 5 O2; decomposition
21. calcium + oxygen 
2 Ca + O2  2 CaO; synthesis
22. potassium hydroxide + sulfuric acid 
2 KOH + H2SO4  K2SO4 + 2 HOH; neutralization; yes
23. calcium + aluminum chloride 
3 Ca + 2 AlCl3  3 CaCl2 + 2 Al; single replacement; yes
24. potassium sulfide + iron (II) nitrate 
K2S + Fe(NO3)2  FeS + 2KNO3; double replacement; yes
25. sulfur dioxide + water 
SO2 + HOH  H2SO3; synthesis
26. lithium sulfide (dissociated) 
Li2S  2Li+1 +S-2; decomposition (physical change)
27. calcium + water 
Ca + 2 HOH  Ca(OH)2 + H2; single replacement; yes
28. sodium + nitric acid 
2 Na + 2 HNO3  2 NaNO3 + H2; single replacement; yes
29. barium oxide 
2 BaO  2 Ba + O2; decomposition
30. stannous sulfate + copper 
SnSO4 + Cu  CuSO4 + Sn; single replacement; NR
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Alpha/Beta Decay:
U92238
Undergoes  decay and becomes 
Th90234
Undergoes  decay and becomes 
Pa91234
Undergoes  decay and becomes 
U92234
Undergoes  decay and becomes 
Th90230
Undergoes  decay and becomes 
Ra88226
Undergoes  decay and becomes 
Rn86222
Undergoes  decay and becomes 
Po84218
Undergoes  decay and becomes 
Pb82214
Undergoes  decay and becomes 
Bi83214
Undergoes  decay and becomes 
Po84214
Undergoes  decay and becomes 
Pb82210
Undergoes  decay and becomes 
Bi83210
Undergoes  decay and becomes 
Po84210
Undergoes  decay and becomes 
Pb82206
Which is stable.
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Half-Life Calculations:
1. 64 g of a substance decays for 4 half-lives. How much of the original substance is
left? 4 g
2. Plutonium-236 has a half-life of roughly 2 years. 32 g of it decay over a period of
8 years. How much of the original sample is left? 2 g
3. How long will it take 60 g of a substance to decay to 3.8 g if the half-life is 4.3 x
106 years? 1.7 x 107 yrs
4. Molybdenum-91 has a half-life of 15.49 minutes. After 40 minutes 1 g of it
remains. What was the mass of the original sample? 6 g
5. 64 g of a substance decays to 1 g in 18 minutes. What is the half-life of the
substance. 3 min
CH 8 Review:
1. What things can you do to initiate or increase the rate of a reaction?
Add energy, stir, add a catalyst, increase concentration, increase surface area
2. What is a catalyst?
Initiates or speeds up a reaction and is not involved in the reaction.
3. Draw Lewis structures to illustrate the reaction on page 1 #12.





O=C=O + O – H  H – O –C – O –H
|
 || 
H
O
4. Why does alpha decay result in the loss in mass of 4 units and change in the
identity of the element? You lose 2 p+ and 2 no
5. How are electrons produced during beta decay?
no is converted to a p+ and an e-; the electron is ejected from the nucleus.
6. Why do you write water as HOH on the reactant side?
In order to predict the correct products for a single replacement reaction.
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