Chapter 9 Balancing Equations
Chemical Equations – Balance equations and indicate the type of reaction
1. 2Ca + O2 -----> 2CaO
2. ZnSO4 + (NH4)2 S-----> (NH4)2SO4 + ZnS
3. 2KI + Cl2 -----> 2KCl + I2
4. 2C2H6 + 5O2 -----> 4CO2 + 6H2O
5. C + H2O -----> CO + H2
6. CaO + H2O -----> Ca(OH)2
7. HCl + NaOH ------> NaCl + H2O
8. BaCl2 + H2SO4 -----> BaSO4 + 2HCl
9. 2Al2O3 -----> 4Al + 4O2
10. 2Al + 6HCl -----> 2AlCl3 + 3 H2
11. 2NaHCO3 -----> Na2CO3 + H2O + CO2
12. Mg + 2HCl -----> H2 + MgCl2
13. C2H8 + 4O2 -----> 2CO2 + 4 H2O
14. 2Al + 3H2SO4 -----> Al2(SO4)3 + 3H2
15. CuO + H2 -----> H2O + Cu
16. N2 + 3H2 -----> 2NH3
17. Cl2 + 6KOH -----> 5KCl + KClO3 + 3H2O
18. 2C2H6 + 7 O2 -----> 4CO2 + 6H2O
19. C6H8O6 + 5 O2 -----> 6CO2 + 4H2O
20. 2Bi(NO3)3 + 3 H2S -----> Bi2S3 + 6HNO3
H. Cannon, C. Clapper and T. Guillot
Klein High School
Balancing Equations
Composition/Synthesis Reactions
Balance the following:
1. 2Al + 3Cl2 ---> 2AlCl3
2. 4Na + O2 ----> 2Na2O
3. MgO + H2O  Mg(OH)2
4. 2 H2O + O2 ----> 2H2O2
5. 2S + 3O2 ---> 2SO3
6. 2H2 + O2 ---> 2H2O
7. Li2O + H2O ---> 2LiOH
8. H2 + S ---> H2S
9. H2 + Cl2 ---> 2HCl
10. 2Mg + O2 ---> 2MgO
11. 4Fe +3 O2 ---> 2Fe2O3
12. 4P + 5O2 ---> 2P2O5
13. S + O2 ---> SO2
14. N2 + O2 ---> 2NO
15. 2SO2 + O2 ---> 2SO3
16. magnesium metal when heated with nitrogen gas reacts to produce solid magnesium
nitride 3Mg + N2 Mg3N2
17. solid lithium reacts with oxygen to form lithium oxide
4Li + O2 2Li2O
18. solid sodium reacts with oxygen to form sodium peroxide
2Na + O2  Na2)2
9-2
HC/CC/TG KHS
Balancing Equations
Balance the following and identify reaction type:
1. H2O2 ---> H2O + O2
2. C12H22O11 + O2 ---> C O2 + H2O
3. H2O ----> H2 + O2
4. Al + Cl2 ---> AlCl3
5. HgO ---> Hg + O2
6. Mg(ClO3)2 ---> MgCl2 + O2
7. CuO ---> Cu + O2
8. RbCl + O2 ---> RbClO4
9. CaCO3 ---> CaO + CO2
10. KClO3 ---> KCl + O2
11 Al2O3 ---> Al + O2
12. Li2O + H2O ---> LiOH
13. KNO3 ---> KNO2 + O2
14. NaHCO3 ---> Na2CO3 + H2O + CO2
15. Al(NO3)3 ----> Al + N2 + O2
16. P2O5 + H2O  H3PO4
17. NH4NO2 ---> N2 + H2O
18. SO2 + O2 ---> SO3
19. H2SO4 ---> H2O + SO3
20. NH4NO3 ---> H2O + N2O
21. Calcium sulfite decomposes to produce calcium oxide and sulfur dioxide
9-3
HC/CC/TG KHS
Balancing Equations
Predicting Reactions
Write balanced equations to indicate the products of the following reactions between the
given reactants?
1. Al + Cu(NO3)2 --->
2. Fe (III) + CuCl2 --->
3. Zn + HCl --->
4. Br2 + NaI --->
5. Al + SnCl2 --->
6. Li + H2O --->
7. Na + H2O --->
8. Cu(II) + NaCl --->
9. Ag + NaCl ---->
10. Br2 + NaCl ---->
11. Zn + NiCl2 --->
12. CuO + H2 --->
13. Al + Cu(NO3)2 --->
14. Ca + H2O ---> 4. Fe + CuSO4 ---> Fe2(SO4)3 + Cu
15. Fe+3 + CuSO4
16. Cl2 + KI --->
17. Mg + H2SO4 --->
18. Cr+3 + HCl --->
19. Cu (II) + AgNO3 --->
20. Mg + HCl --->
9-4
HC/CC/TG KHS
Balancing Equations
Balance the following:
1. BaCl2 + H3PO4 ---> Ba3(PO4)2 + HCl
2. H2SO4 + KOH ---> K2SO4 + H2O
3. AgNO3 + H2S ---> Ag2S + HNO3
4. Na + O2 ----> Na2O
5. KOH + CO2 ---> K2CO3 + H2O
6. Ca(OH)2 + HC2H3O2 ----> Ca(C2H3O2)2 + H2O
7. Pb(C2H3O2)2 + K2CrO4 ----> PbCrO4 + KC2H3O2
8. Pb(NO3)2 + Na2CrO4 ---> PbCrO4 + NaCO3
9. H2 + Cl2 ---> HCl
10. PbCl2 + HNO3 ---> Pb(NO3)2 + HCl
11. AlCl3 + LiOH ---> Al(OH)3 + LiCl
12. H2O2 ---> H2O + O2
13. C6H12O6 + O2 ---> C O2 + H2O
14. Ba(OH)2 + CO2 ---> BaCO3 + H2O
15. CaC2 + H2O ---> Ca(OH)2 + C2H2
16. Fe + O2 ---> Fe2O3
17. HCl + AgNO3 ---> HNO3 + AgCl
18. NaHCO3 ---> Na2CO3 + H2O + CO2
19. Ca(OH)2 + H2SO4 ----> CaSO4 + H2O
20. PdCl2 + HNO3 ---> Pd(NO3)2 + HCl
21. PCl5 + H2O -----> H3PO4 + HCl
22. Na2O + P4O10 -----> Na3PO4
9-5
HC/CC/TG KHS
Balancing Equations
23. P4O10 + 6H2O -----> 4H3PO4
24. 3CaCO3 + 2H3PO4 -----> Ca3(PO4)2 + 3CO2 + 3H2O
25. 3MnO2 + 4Al -----> 2Al2O3 _ 3Mn
26. C2H6O + 3O2 ------> 2CO2 + 3H2O
27. 2Al(ClO3)3 -----> 2AlCl3 + 9O2
28. 2 KClO3 -----> 2KCl + 3O2
29. Al2O3 + 3H2O -----> 2 Al(OH)3
30. 2Na + H2O -----> Na2O + H2
31. Br2 + 2NaI -----> 2NaBr + I2
32. 2 Cu+1 + FeCl2 -----> 2CuCl + Fe
33. Ba + H2O -----> BaO + H2
34. 2Al + 6HC2H3O2 -----> 2Al(C2H3O2)3 + 3H2
35. Br2 + 2NaCl -----> 2NaBr + Cl2
36. Cu + NaCl -----> CuCl + Na
37. 2Au+1 + NiSO4 -----> Ni + Au2SO4
38. Cl2 + 2NaI -----> 2NaCl + I2
39. Mg + H2O -----> MgO + H2
40. Zn + NiCl2 -----> ZnCl2 + Ni
9-6
HC/CC/TG KHS
Balancing Equations
Predict the balanced outcome of the following
1. Chlorine gas and potassium iodide Cl2 + 2KI  2KCl + I2
2. Combustion of sucrose (C12H22O11) C12H22O11 + 12O2  12CO2 + 11H2O
3. Decompostion of potassium chlorate 2KCLO3  2KCl + 3O2
4. Combustion of ethane (C2H6) 2C2H6 + 9O2  4CO2 + 6H2O
5. Aluminum chloride reacts with lithium hydroxide
AlCl3 + 3LiOH  Al(OH)3 + 3LiCl
6. Displacement of iron from ferric oxide by magnesium
Fe2O3 +3 Mg 3 MgO + 2Fe
7. Decomposition of aluminum oxide
2Al2O3  4Al + 3O2
8. Combustion of butene (C4H8)
C4H8 + 6O2 4CO2 + 4H2O
9. Decomposition of hydrogen peroxide
H2O2  H2 + O2
10. Combination of sulfur and oxygen
S + O2  SO2
11. Combustion of C8H18
2C8H18+ 25O2  16CO2 + 18H2O
12. Displacement reaction between iron (III) oxide and aluminum
Fe2O3 + 2Al  Al2O3 + 2Fe
13. Combustion of C2H5OH
C2H5OH + 3O2  2CO2 + 3H2O
14. Reaction of lead (II) nitrate with phosphoric acid
3Pb(NO3)2 + 2H3PO4  Pb3(PO4)2 + 6HNO3
15. Combustion of pentene (C5H10)
2C5H10 + 15O2  10CO2 + 10H2O
16. Decompostion of sodium bicarbonate
2NaHCO2  Na2O + CO2 + H2O
17. Combustion of C6H6
2C2H6 + 7O2  4CO2 + 6H2O
18. Reaction between calcium hydroxide and sulfuric acid
Ca(OH)2 + H2SO4  CaSO4 + 2H2O
19. Reaction between silicon tetrafluoride and water
SiF4 + 2H2O 4 HF + SiO2
20. Combustion of C4H10
2C4H10 + 13O2  8CO2 + 10H2O
9-7
HC/CC/TG KHS
Balancing Equations
Exercise 7 Balance the following:
1. C2H6 + O2 ---> CO2 + H2O
2. C4H8 + O2 ---> CO2 + H2O
3. C8H18 + O2 ----> CO2 + H2O
4. C2H5OH + O2 ---> CO2 + H2O
5. C5H10 + O2 ---> CO2 + H2O
6. C6H6 + O2 ---> CO2 + H2O
7. C4H10 + O2 ---> CO2 + H2O
8. C3H8 + O2 ----> CO2 + H2O
9. C6H8O6 + O2 ---> CO2 + H2O
10. C4H8 + O2 ---> CO2 + H2O
Write the equation for the following reactions:
1. zinc plus chlorine
2. sodium hydroxide and potassium
3. silver plus sulfur
4. magnesium and calcium chloride
5. bromine plus sodium
6. mercury (II) oxide and zinc
7. phosphorus plus oxygen
8. gold (III) sulfide and platinum (IV)
9. aluminum and iodine
10. mercury I oxide decomposes
11. hydrogen and oxygen
12. sodium hydroxide and potassium nitrate
9-8
HC/CC/TG KHS
Balancing Equations
13. carbon and chlorine
14. iron (III) acetate and calcium sulfate
15. copper(II) and nitrogen
16. cupric oxide and stannic chloride
17. iron (III) and sulfur
18. platinum (II) phosphite and strontium bromide
19. carbon plus excess oxygen
20. tin (II) chloride and sodium fluoride
21. iron (III) and copper (II) sulfate
22. plumbic chlorate and potassium sulfide
23. aluminum and silver nitrate
24. nickel(II) oxalate and ferric dichromate
25. mercury (I) and silver nitrate
26. beryllium sulfide and sodium bromide
27. strontium iodide and fluorine
28. aluminum oxide and potassium iodide
29. chlorine and silver iodide
30. calcium nitrate and sodium acetate
31. nitric acid and sodium citrate
32. aluminum oxide and manganese (IV) sulfite
9-9
HC/CC/TG KHS
Balancing Equations
Types of Reactions Lab
In this experiment you will cause several reactions to occur. From your tests,
observations and powers of deduction, you will be able to (1) describe the products; (2)
name the products: (3) identify the “type” of reaction: and (4) balance the chemical
equation for the reaction.
Reaction 1: Place one heaping spoonful of potassium chlorate in a dry test tube. Clamp
at a 45-degree angle to a ring stand. Heat with a Bunsen burner, slowly at first, until it
melts and then starts to give off a colorless gas (looks like smoke). Light a wood splint,
let it burn a few second, and then blow it out. Then quickly hold the glowing splint jus
inside the mouth of the test tube. The splint busting into flame again verifies the
presence of oxygen. There is a pinkish-white solid that remains in the test tube.
Reaction 2: Put 2 squirts of copper (II) sulfate solution in a test tube. Place a shine strip
of zinc metal in the test tube and observe for several minutes. (Go on to another section
and return.) Pour off the liquid into the sink, but dump the solids on a paper towel.
Remove the leftover zinc (save for Reaction 6) and inspect the precipitate, which is a
finely divided powder. Another product remains dissolved in the solution.
Reaction 3: Obtain a 2-cm length of magnesium ribbon. Holding one end with the
crucible tongs, ignite the other end in a Bunsen burner flame. WEAR GOGGLESAND
DO NOT LOOK DIRECTLY A THE FLAME! Hold the magnesium over the base of
the ring stand as it burns. With what in the air is the magnesium reacting? Describe the
product.
Reaction 4: To a test tube, add one squirt of a solution of potassium chromate and one
squirt of a solution of barium chloride. Swirl to mix. Describe the precipitate that forms.
Reaction 5: place one large spoonful of sodium bicarbonate in a dry metal crucible.
Place in a triangle on a ring on a ring stand; partly cover with a watch glass, leaving
enough space open at one edge to insert a wood splint. Heat with a Bunsen burner,
slowly at first, until it starts to give off a colorless gas. Light a wood splint, let it burn a
few second, DO NOT BLOW OUT. Insert the lit end into the crucible. The flame
being extinguished verifies the presence of carbon dioxide. Observe any deposit on the
watch glass. There is a white solid that remains in the crucible.
Reaction 6: Put the zinc strip from Reaction 2 back in a test tube and add 2 squirts of
dilute hydrochloric acid (HCl). Cover the test tube with your thumb for one or two
minutes until you feel some pressure. Light a match and hold it (still lit) over the mouth
of the test tube to test for flammability, which indicates hydrogen gas. This test may be
repeated as long as gas is being produced. Pour the unused acid down the sink. Save and
leftover zinc and throw away in the wastebasket.
9-10
HC/CC/TG KHS
Balancing Equations
Chapter 9 Activity Series of Metals
Lithium
Potasiium
Barium
Calcium
Sodium
Magnesium
Aluminum
Zinc
Iron
Nickel
Tine
Lead
(Hydrogen)
Copper
Mercury
Silver
Gold
Li
K
Ba
Ca
Na
Mg
Al
Zn
Fe
Decreasing activity
Ni
Sn
Pb
(H)*
Cu
Hg
Ag
Au
*Metals from Li to Na will replace H from acids and water. From Mg to Fe they will
replace hydrogen from acids only.
ACTIVITY SERIES OF NONMETALS
F2
Cl2
Br2
Decreasing Activity
I2
9-11
HC/CC/TG KHS