Chemical Equations and Reactions Name:

Date: Period:

1. A chemical equation is balanced if there is an __________________ number of each kind of

_____________________ on both sides of the equation.

2. Determine the number of atoms of each kind in each of the following:

a. CaCO3 _____ Ca, _____ C, _____ O

b. (NH4)2SO4 _____ N, _____ H, _____ S, _____ O

c. 3 H2O _____ H, _____ O

d. 4 Mg(OH)2 _____ Mg, _____ O, _____ H

e. 5 Ba(NO3)2 _____ Ba, _____ N, _____ O

3. Now look at the following chemical equations. Count the number of atoms of each element on the reactant and product side. Determine if the statement is a balanced equation.

a. 2 Na + 2 H2O 2 NaOH + H2

Reactants Products

_______ Na _______

_______ H _______

_______ O _______ Balanced? Yes _____ No _____

b. 4 NH3 + 6 NO 5 N2 + 6 H2O

Reactants Products

_______ N _______

_______ H _______

_______ O _______ Balanced? Yes _____ No _____

c. NaCl + F2 NaF + Cl2

Reactants Products

_______ Na _______

_______ Cl _______

_______ F _______ Balanced? Yes _____ No _____

d. 3 NaBr + H3PO4 2 HBr + Na3PO4 Balanced? Yes _____ No _____

_______ Na _______

_______ Br _______

_______ H _______

_______ P _______

_______ O _______

e. N2H4 + N2O4 3 N2 + 4 H2O Balanced? Yes _____ No _____

f. 2 Bi + 3 F2 2 BiF3 Balanced? Yes _____ No _____

g. Al + Ni(NO3)2 Al(NO3)3 + Ni Balanced? Yes _____ No _____

h. 3 NaBH4 + 4 BF3 2 B2H6 + 3 NaBF4 Balanced? Yes _____ No _____

i. 4 C3H5(NO3)3 6 N2 + O2 + 12 CO2 + 10 H2O

Balanced? Yes _____ No _____

j. Ca10F2(PO4)6 + 7 H2SO4 2 HF + 3 Ca(H2PO4)2 + 7 CaSO4

Balanced? Yes _____ No _____

Directions: Balance the following reactions. Place a “B” at the end of any that are balanced as written.

4. _____ Zn + _____O2 → _____ZnO

5. _____HI → _____H2 + _____I2

6. _____B + _____F2 → _____BF3

7. _____N2 + _____H2 → _____NH3

8. _____Fe + _____H2O → _____Fe3O4 + _____H2

9. BaCl2 + H2SO4 → BaSO4 + HCl

10. P + O2 → P4O10

11. KClO3 → KCl + O2

12. C3H8 + O2 → CO2 + H2O

13. Cu + AgNO3 → Cu(NO3)2 + Ag

14. Te + H2O → TeO + H2

15. La(NO3)3 + NaOH → La(OH)3 + NaNO3

16. RhO3 → RhO + O2

17. Hf + N2 → Hf3N4

18. Ga + H2SO4 → Ga2(SO4)3 + H2

19. PdCl2 + HNO3 → Pd(NO3)2 + HCl

20. RbBr + AgCl → AgBr + RbCl

21. PaI5 → Pa + I2

22. Fe2O3 → Fe + O2

23. Cu + Cl2 → CuCl2

24. Na + O2 → Na2O

25. H2 + O2 → H2O

26. Na2SO4 + CaCl2 → CaSO4 + NaCl

27. Al2O3 → Al + O2

28. C2H6 + O2 → CO2 + H2O

29. SO3 + H2O → H2SO4

30. SiCl4 → Si + Cl2

31. C + H2 → CH4

32. Br2 + NaI → NaBr + I2

33. Zn + HCl → ZnCl2 + H2

34. H2S + O2 → H2O + SO2

35. Ba(NO3)2 + Na2SO4 → BaSO4 + NaNO3

36. C5H12 + O2 → CO2 + H2O

37. HgO → Hg + O2

38. H2SO4 + Pb + PbO2 → PbSO4 + H2O

39. C6H12O6 + O2 → CO2 + H2O

40. Ca + H2O → Ca(OH)2 + H2

41. C6H12O6 → C2H5OH + CO2

42. HC2H3O2 + NaHCO3 → CO2 + NaC2H3O2 + H2O

Challenging:

43. NaCl + SO2 + H2O O2 → Na2SO4 + HCl

44. Fe2O3 + CO → CO2 + Fe

45. Ca3(PO4)2 + C + SiO2 → CaSiO3 + CO + P4

More:

46. C + O2 → CO

47. Mg + O2 → MgO

48. CuO + C → Cu + CO2

49. NH3 + O2 → NO2 + H2O

50. O3 → O2

51. Cu + AgNO3 → Cu(NO3)2 + Ag

52. C8H18 + O2 → CO2 + H2O

53. Sn + HF → SnF2 + H2

54. Al(OH)3 + HCl → AlCl3 + H2O

55. Ca3(PO4)2 + H2SO4 → H3PO4 + CaSO4

56. Fe + O2 → Fe3O4

57. NH4NO3 → N2O + H2O

58. C + Al2O3 → Al + CO2

59. N2 + H2 → NH3

60. BaCl2 + Na2SO4 → BaSO4 + NaCl

61. C6H12O6 + O2 → CO2 + H2O

62. Al + Fe2O3 → Fe + Al2O3

63. CO2 + LiOH → Li2CO3 + H2O

64. NO + H2 → NH3 + H2O

65. Al + H2SO4 → Al2(SO4)3 + H2

66. HgO → Hg + O2

67. KClO3 → KCl + O2

68. CaBr2 + Na3P → Ca3P2 + NaBr

69. H2O + Fe → Fe2O3 + H2

70. C6H12O6 → C + H2O

71. C2H6 + O2 → CO2 + H2O

72. Li3PO4 → Li + P + O2

73. Ca(OH)2 + HNO3 → Ca(NO3)2 + H2O

74. Al2(SO4)3 + Ca(OH)2 → Al(OH)3 + CaSO4

75. P + O2 → P2O5

76. N2 + H2 → NH3

77. CH4 + O2 → CO2 + H2O

78. Fe2O3 + H2 → Fe + H2O

79. AsCl3 + H2S → As2S3 + HCl

80. C3H8 + O2 → CO2 + H2O

81. K2S + CuBr2 → CuS + KBr

82. Al + O2 → Al2O3

83. H2S + KOH → H2O + K2S

84. Fe + S8 → FeS

85. Ca(NO3)2 + Na3PO4 → Ca3(PO4)2 + NaNO3

DIRECTIONS: Refer to the unbalanced chemical equation below to answer the following questions. Write your answers in the space provided.

Al(NO3)3 + FeCl2 → Fe(NO3)2 + AlCl3

86. Write the names of the reactants in this equation:

_______________________________________ _____________________________________

87. Write the names of the products in this equation:

_______________________________________ _____________________________________

88. Balance the equation above. What is the coefficient for Al(NO3)3? ___________

What is the coefficient for FeCl2? ___________

What is the coefficient for Fe(NO3)2? ___________

What is the coefficient for AlCl3? ___________

89. How many oxygen atoms are there on each side of the balanced equation? __________

90. What should you do if an equation you have written cannot be balanced? ________________________

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91. How is balancing an equation related to the Law of Conservation of Matter? _____________________

___________________________________________________________________________________

92. Describe the correct way to balance an equation: ___________________________________________

___________________________________________________________________________________

93. How are the physical states of the reactants and products indicated in a chemical equation? __________

___________________________________________________________________________________

Write complete equations for the following using the state symbols!

Remember the seven diatomic elements !!!

93a.Two molecules of solid sodium chloride decompose when exposed to an electric current into two atoms of sodium metal and 1 molecule of chlorine gas.

93b.One molecule in a barium chloride solution reacts with one molecule in a sodium sulfate solution to produce 1 molecule of solid barium sulfate and 2 molecules of sodium chloride in solution.

93c.Two molecule of solid potassium chlorate, when heated, decompose into two molecules of solid potassium chloride and 3 molecules of oxygen gas.

93d. One molecule of solid calcium carbonate decomposes when heated into one molecule of solid calcium oxide and 1 molecule of carbon dioxide gas.

93e. Two molecules of solid aluminum hydroxide decomposes when heated into one molecule of solid aluminum oxide and three molecules of water vapor .

93f. One atom of zinc metal when mixed with two molecules of a hydrochloric acid solution react and produce one molecule of zinc chloride in solution and one molecule of hydrogen gas.

DIRECTIONS: Write balanced chemical equations for each of the following reactions. Indicate the physical state of the reactants and products (ex – s,g,l,aq).

94. Hydrogen gas reacts with nitrogen gas to produce ammonia gas (NH3).

95. Hydrogen bromide gas reacts with oxygen gas to produce liquid water and bromine gas.

96. When a solid piece of magnesium is placed in hydrochloric acid, hydrogen gas bubbles off and magnesium chloride is left in solution.

97. Hydrochloric acid can be added to calcium carbonate to produce calcium chloride in solution, carbon dioxide gas and water.

98. Solid carbon disulfide can be used to form carbon dioxide gas and sulfur dioxide gas when it reacts with oxygen gas.

99. Solid manganese dioxide reacts with hydrochloric acid to produce manganese (II) chloride, liquid water and chlorine gas.

100. Write the equation for the following reaction: ammonia, NH3, reacts with hydrochloric acid to form ammonium chloride.

101. When heated, calcium carbonate decomposes to form calcium oxide and carbon dioxide. Write the equation for this reaction:

102. Write the equation for the following reaction: barium oxide reacts with water to form barium hydroxide.

103. Acetaldehyde, CH3CHO, decomposes to form methane, CH4, and carbon monoxide. Write the equation for this reaction.

104. Write the equation for the following reaction: zinc reacts with copper (II) nitrate to form zinc nitrate and copper.

105. When heated, calcium sulfite decomposes to form calcium oxide and sulfur dioxide. Write an equation for this reaction.

106. Write the equation for the following reaction: iron metal reacts with sulfuric acid to form iron (II) sulfate and hydrogen gas.

107. Azomethane, C2H6N2, decomposes to form ethane, C2H6, and nitrogen gas at 297 °C. Write an equation for this reaction.

108. Write out the equation for the following reaction: carbon monoxide reacts with chlorine gas to form phosgene, COCl2.

109. Manganese (II) iodide decomposes when exposed to light to form manganese and iodine. Write an equation for this reaction.

110. Write a balanced chemical equation for the reaction in which dinitrogen pentoxide reacts with water to form nitric acid.

111. Magnesium reacts with titanium (IV) chloride to produce magnesium chloride and titanium. Write the balanced equation for this reaction.

112. Write a balanced chemical equation for the reaction in which carbon reacts with zinc oxide to produce zinc and carbon dioxide.

113. Bromine reacts with sodium iodide to form sodium bromide and iodine. Write the balanced equation for this reaction.

114. Write a balanced chemical equation for the reaction in which phosphorus trichloride reacts with chlorine gas to produce phosphorus pentachloride.

115. Phosphorus reacts with bromine to produce phosphorus tribromide. Write the balanced equation for this reaction.

116. Calcium hydride reacts with water to produce calcium hydroxide and hydrogen gas. Write the balanced equation for this reaction.

117. Write the balanced chemical equation for the reaction in which sulfuric acid reacts with potassium hydroxide to produce potassium sulfate and water.

118. Write a balanced chemical equation for the reaction in which propane, C3H8, reacts with oxygen gas to produce carbon dioxide and water.

119. Benzene, C6H6, reacts with oxygen gas to produce carbon dioxide and water. Write the balanced equation for this reaction.

Synthesis Reactions

Equations

Chemical reactions are happening around you all the time. A match burns. A car rusts. Food spoils. Leaves decay. These are just a few chemical reactions.

Probably the most important chemical reactions take place in your body. They are happening this very moment. Digestion is a chemical process. So is respiration. In every one of your trillions of cells, chemical reactions are taking place all the time. Life depends upon chemical reactions.

There are several kinds of chemical reactions. One kind is a synthesis reaction. “Synthesis” means putting together. A synthesis reaction combines substances, usually elements (but sometimes smaller compounds), to form a new, larger compound. When the compound forms, we say it has been synthesized. Below is a “model” of a synthesis reaction.

A + B → AB Element + Element → Compound

1. RUSTING When iron rusts, it combines with oxygen.4Fe + 3O2 → 2Fe2O3

iron + oxygen → iron oxide (rust)

Element + Element

Compound

2. THE BURNING OF CARBON Charcoal is made of the element carbon, C. When carbon burns, it combines with oxygen. This produces the gas carbon dioxide, CO2.

C + O2 → CO2

carbon + oxygen → carbon dioxide Element +

Element Compound

A synthesis reaction is like any other kind of chemical reaction. No matter is created or destroyed. The atoms just change their arrangement.

Equation I: CO2 + C → 2CO2 Equation II: CO2 + H2O → H2CO3

120. How is Equation I different from the other synthesis equations seen in this packet? ________________

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121. 1. How is Equation II different from the other synthesis equations seen in this packet? _____________

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122. Look at the equations below. Identify the synthesis reactions by placing a check (√) next to it.

Equation A Synthesis Reaction

Not a Synthesis Reaction

a. 2K + Br2 → 2KBr

b. 2H2O → 2H2 + O2

c. NaCl → Na + Cl

d. 4Au + 3O2 → 2Au2O3

e. 2Na + 2HCl → 2NaCl + H2

f. Cu + Br2 → CuBr2

g. ZnSO4 + FeCl2 → ZnCl2 + FeSO4

h. 2Na + Br2 → 2NaBr

i. 2HgO → 2Hg + O2

j. CH4 + 2O2 → CO2 + 2H2O

Decomposition Reaction

Synthesis reactions build compounds. Anything that can be built can also ne taken apart. The breakdown of a compound into simpler substances is called decomposition. Decomposition is a chemical process.

Let’s look at two examples:

1. Common table salt (sodium chloride) is a compound composed of the elements sodium and chlorine. It can be melted, and if electricity is passed through melted sodium chloride, it decomposes. It changes back into atoms of sodium and chlorine. Here is the reaction:

The decomposition of a compound by means of electricity is called electrolysis. Only certain compounds can be decomposed by electrolysis. Usually these compounds are liquids.

2. Potassium chlorate (KClO3) is a compound composed of potassium, chlorine and oxygen. Heat decomposes potassium chlorate into oxygen and potassium chloride (a simpler compound.) Here is the reaction:

Notice that the decomposition is not complete, the oxygen has been separated, but the potassium and chlorine are still joined in the compound, potassium chloride. Another kind of decomposition reaction can separate potassium chloride into its elements. Only certain compounds can be decomposed with heat

2NaCl 2Na + Cl sodium chloride sodium chlorine (compound) (element) (element)

2KClO3 2KCl + 3O2 potassium chlorate potassium chloride oxygen (compound) (a simpler compound) (element)

Look at the diagram above and previous page. Electrolysis decomposes water. This is the equation for the reaction:

170. Identifying Synthesis and Decomposition Reactions:

Equation A Synthesis Reaction

A Decomposition Reaction Neither

a. CuCl2 → Cu + Cl2

b. 3Hf + 2N2 → Hf3N4

c. Zn + 2HCl → ZnCl2 + H2

d. C3H8 + 5O2 → 4H2O + 3CO2

e. 2NaOH → 2Na + O2 + H2

f. Fe + S → FeS

g. CaCl2 + FeSO4 → Ca SO4 + FeCl2

h. 4P + 5O2 → 2P2O5

i. 3CuCl2 + 2Al → 2AlCl3 + 3Cu

j. Ca(OH)2 → CaO + H2O

Matching:

______ 123. synthesis reaction A) breaks down compounds

______ 124. decomposition reaction B) uses electricity

______ 125. electrolysis and heat C) methods of decomposition

______ 126. electrolysis D) simpler than a compound

______ 127. an element E) builds compounds

Short Answer:

128. Does boiling decompose water? ________________

129. What does boiling do to water? _________________________________________________________

___________________________________________________________________________________

2H2O → 2H2 + O2

water → hydrogen + oxygen

Activity Series of Metals

* Hydrogen is included in the activity series of metals because it has a positive oxidation number.

Ease

of o

xida

tion

incr

ease

s

ElementLithiumPotassiumBariumCalciumSodiumMagnesiumAluminumManganeseZincChromiumIronCobaltNickelTinLeadHydrogen*CopperMercurySilverPlatinumGold

Single & Double Replacement & Combustion Packet

In a Single Replacement Reaction a free element takes the place of or replaces another element that is part of a compound. The element that was replaced is now “free.”

A + BC → AC + Bfree element compound new compound new free element

Let’s study an actual replacement reaction – one between zinc (Zn) and hydrochloric acid (HCl). The zinc is the “free” element and the hydrochloric acid is the compound.

Zn + HCl → ZnCl2 + H2

The zinc replaces the hydrogen. The hydrogen gas is set free.

The reaction produces a new compound, zinc chloride (ZnCl2), and free hydrogen (H2). Notice that the elements we started with are the elements we ended with, they are just arranged in a different way. This kind of reaction is called a single replacement reaction where a free element replaces an element that is part of a compound.

For example, if you do a simple experiment of placing an iron nail (Fe) in a solution of copper (II) sulfate (CuSO4), you will see that after a few minutes the nail is coated with copper metal. Here is the equation for the reaction:

Fe + CuSO4 → FeSO4 + Cu

Single Replacement Reactions

Decide whether each reaction is possible. Place a check next to the reactions that are possible.

130. _____ Zn + CuSO4 ZnSO4 + Cu

131. _____ Pb + Mg(NO3)2 Pb(NO3)2 + Mg

132. _____ AgCl2 + Zn ZnCl2 + Ag

133. _____ 2HCl + Ca CaCl2 + H2

134. _____ Pt + 2HCl PtCl2 + H2

Write balanced equations for the following single replacement reactions. Make sure to check that each reaction is possible on your Activity Series List.

135) Magnesium metal reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas.

136) Sodium Chloride reacts with potassium to produce potassium chloride and sodium.

137) Zinc Sulfate reacts with copper to produce zinc metal and copper (II) sulfate.

138) Cobalt (II) oxide reacts with aluminum to produce aluminum oxide and cobalt.

139) Nickel (III) sulfate reacts with zinc to produce zinc sulfate and nickel

140. Identify (√) the following reactions as Synthesis (Syn), Decomposition (Decomp),Single Replacement (SR) or None of These

Equation Synthesis Reaction

Decomposition Reaction

Single Replacement

Reaction

None of These

a. C + 2S → CS2

b. 2H2O2 → 2H2 + O2

c. 2Al + 6HCl → 2AlCl3 + 3H2

d. Li3PO4 + 3NaF → 3LiF + Na3PO4

e. Zn + PbO → ZnO + Pb

f. CuCl2 + 2KBr → CuBr2 + 2KCl

g. CuSO4 + Fe → Cu + FeSO4

h. 2Na + Br2 → 2NaBr

i. 2HgO → 2Hg + O2

j. C3H8 + 5O2 → 3CO2 + 4H2O

Double Replacement Reactions:

A double replacement reaction takes place between two compounds. A part of one compound changes place with a part of the other compound. This produces two new compounds.

AB + CD → AD + CBcompound compound new compound new compound

The positive ion of one compound switches place with the positive part of the other compound. Let’s look at an example of a double replacement reaction between sodium hydroxide and hydrochloric acid:

NaOH + HCl → NaCl + HOH

The sodium and hydrogen change places and two new compounds form, NaCl and HOH (water).

Example #1) BaCl2 + Na2SO4 → BaSO4 + 2NaCl

barium sodium barium sodiumchloride sulfate sulfate chloride

141. Identifying Double Replacement Reactions:

EquationA Double

Replacement Reaction

Not a Double Replacement

Reactiona. Mg(OH)2 + 2HCl → MgCl2 + 2H2O

b. C6H10O5 +H2O → C6H12O6

c. Na2SO4 + BaCl2 → 2NaCl + BaSO4

d. 3Mg + N2 → Mg3N2

e. H2SO4 + BaCl2 → 2HCl + BaSO4

f. CH4 + 2O2 → CO2 + 2H2O

g. ZnCO3 → ZnO + CO2

h. CuSO4 + H2S → H2SO4 + CuS

i. NH4NO3 → 2H2O + N2O

j. C6H12 + 9O2 → 6CO2 + 6H2O

142. Identify (√) the following reactions as Synthesis (Syn), Decomposition (Decomp), Single Replacement (SR) , Double Replacement (DR) , Other

Equation Reaction Type

Syn. Decomp. S.R. D.R. Other

a. N2 + 3H2 → 2NH3

b. 2Br2 + 2H2O → 4HBr + O2

c. Mg + 2HCl → MgCl2 + H2

d. 2KBr + H2SO4 → K2SO4 + 2HBr

e. H2SO3 → H2O + SO2

f. C6H12O6 + 6O2 → 6CO2 + 6H2O

g. NaCl + AgNO3 → NaNO3 + AgCl

h. H2 + Cl2 → 2HCl

i. H2CO3 → H2O + CO2

j. C3H8 + 5O2 → 3CO2 + 4H2O

Combustion Reactions:

A combustion reaction takes place between a hydrocarbon (a compound made of hydrogen and carbon) and the element oxygen. Oxygen is a diatomic element which means it is so reactive it will bond with itself. Therefore the oxygen in the air required for combustion is O2. Carbon dioxide and water are always the products for these types of reactions.

CH + O2 → CO2 + H2O hydrocarbon oxygen carbon dioxide water

For example, when natural gas (methane, CH4) is burned with oxygen (O2) carbon dioxide (CO2) and water (H2O) are produced.

CH4 + 2O2 → CO2 + 2H2Omethane oxygen carbon dioxide water

In another example, cellular respiration, our body metabolizes glucose (C6H12O6) with oxygen (O2) and we produce carbon dioxide (CO2) and water (H2O). In this case the “hydrocarbon” also contains oxygen.

C6H12O6 + 6O2 → 6CO2 + 6H2Oglucose oxygen carbon dioxide water

143.Equation A Combustion Not a

Reaction Combustion Reaction

a. Mg(OH)2 + 2HCl → MgCl2 + 2H2O

b. 2Br2 + 2H2O → 4HBr + O2

c. C3H8 + 5O2 → 3CO2 + 4H2O

d. 3Mg + N2 → Mg3N2

e. H2SO4 + BaCl2 → 2HCl + BaSO4

f. CH4 + 2O2 → CO2 + 2H2O

g. ZnCO3 → ZnO + CO2

h. C6H10O5 +H2O → C6H12O6

i. NH4NO3 → 2H2O + N2O

j. C6H12 + 9O2 → 6CO2 + 6H2O

144. Identify (√) the following reactions as Synthesis (Syn), Decomposition (Decomp), Single Replacement (SR) , Double Replacement (DR) , Combustion (C)

EquationReaction Type

Syn. Decomp. S.R. D.R. C

a. CO2 → C + O2

b. NaCl + AgNO3 → NaNO3 + AgCl

c. S + Cl2 → SCl2

d. BaCl2 + 2NaOH → 2NaCl + Ba(OH)2

e. C3H8 + 5O2 → 3CO2 + 4H2O

f. CH4 → C + 2H2

g. Pb(NO3)2 + Mg → Pb + Mg(NO3)2

h. Mg + 2HCl → MgCl2 + H2

i. H2SO4 → H2 + S + 2O2

j. 2O2 + N2 → N2O4

k. 3CaBr2 + 2Na3P → Ca3P2 + 6NaBr

l. 2KI + Br2 → 2KBr + I2

m. C6H12O6 → 6C + 6H2O

n. C6H12 + 9O2 → 6CO2 + 6H2O

o. Si + O2 → SiO2

p. 2NaI + Pb(NO3)2 → 2NaNO3 + PbI2

q. 2C8H18 + 25O2 → 16CO2 + 18H2O

r. H2 + CO + O2 → H2CO3

s. C6H12O6 + 6O2 → 6CO2 + 6H2O

t. CS2 + 2F2 → CF4 + 2S

Types of Chemical Reactions

Directions: Label the following reactions as synthesis (S), decomposition (D), single replacement (SR), double replacement (DR) and combustion (C).

145. NaCl → Na + Cl2 ___________

146. Na + Cl2 → NaCl ___________

147. C2H4 + O2 → CO2 + H2O ___________

148. H2O → H2 + O2 ___________

149. H2 + O2 → H2O ___________

150. C8H18 + O2 → CO2 + H2O ___________

151. NaOH + HCl → HOH + NaCl ___________

152. Na + HCl → H2 + NaCl ___________

153. K + Cl2 → KCl ___________

154. K + AgCl → Ag + KCl ___________

155. C6H12 + O2 → CO2 + H2O ___________

156. Ca + S → CaS ___________

157. KOH + HNO3 → HOH + KNO3 ___________

158. Al + O2 → Al2O3 ___________

159. HgO → Hg + O2 ___________

160. NaOH + H2SO4 → Na2SO4 + H2O ___________161. Fe + O2 → Fe2O3 ___________

162. C6H8 + O2 → CO2 + H2O ___________

163. Pb(NO3)2 + K2CrO4 →PbCrO4 + KNO3 ___________

164. H2 + N2 → NH3 ___________

165. C3H5(NO3)3 → CO2 + N2 + H2O + O2 ___________

166. Fe + CuCl2 → FeCl2 + Cu ___________

167. KClO3 → KCl + O2 ___________

168. Mg + HCl → H2 + MgCl2 ___________

169. C5H10 + O2 → CO2 + H2O ___________

170. CO2 → C + O2 ___________

171. NaCl + AgNO3 → NaNO3 + AgCl ___________

172. S + Cl2 → SCl2 ___________

173. BaCl2 + NaOH → NaCl + Ba(OH)2 ___________

174. Zn + CuSO4 → ZnSO4 + Cu ___________

175. CH4 → C + H2 ___________

176. Pb(NO3)2 + Mg → Pb + Mg(NO3)2 ___________

177. H2SO4 → H2 + S + O2 ___________

178. C3H8 + O2 → CO2 + H2O ___________

179. O2 + N2 → N2O4 ___________

180. CaBr2 + Na3P → Ca3P2 + NaBr ___________

181. 2KI + Br2 → 2KBr + I2 ___________

182. C6H12O6 → C + H2O ___________

183. NaF → Na + F2 ___________

184. Si + O2 → SiO2 ___________

185. H2 + CO + O2 → H2CO3 ___________

186. C7H14 + O2 → CO2 + H2O ___________

187. Li3PO4 → Li + P + O2 ___________

Classifying Chemical Reactions

Part I: Matching

_______ 188. A + B → AB A. combustion reaction

_______ 189. A + BX → AX + B B. decomposition (analysis) reaction

_______ 190. AX + BY → AY + BX C. double replacement reaction

_______ 191 AB → A + B D. single replacement reaction

_______ 192. hydrocarbon + O2 → CO2 + H2O E. synthesis (direct combination) reaction

Part II: Classifying Classify the following reactions as synthesis (S), decomposition (D), single replacement (SR), double replacement (DR) or combustion (C).

_______ 193. CO2 → C + O2

_______ 194. NaCl + AgNO3 → NaNO3 + AgCl_______ 195. S + Cl2 → SCl2

_______ 196. BaCl2 + NaOH → NaCl + Ba(OH)2

_______ 197. C5H10 + O2 → CO2 + H2O_______ 198. Zn + CuSO4 → ZnSO4 + Cu_______ 199. CH4 → C + H2

_______ 200. C3H8 + O2 → CO2 + H2O_______ 201. Pb(NO3)2 + Mg → Pb + Mg(NO3)2

Part III: Short Answer

202. Explain why hydrogen is listed in the Activity Series even though hydrogen is not a metal.

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Part IV: Write the complete (with state symbols) balanced equation for the following reactions and then identify the type of reaction (S, D, SR, DR, C.)

203. Magnesium metal replaces mercury in a solution of mercury (II) nitrate.

204. Bromine gas combines with gaseous nitrogen to produce gaseous nitrogen tribromide.

205. A solution of potassium sulfate reacts with a solution of lead (II) nitrate.

206. Solid potassium chlorate is heated and decomposes into oxygen gas and solid potassium chloride.

207. The gas in our gas jets is methane, CH4. Write the reaction for the combustion of methane.

Equations

Directions: Write, balance and identify the type for each of the following reactions.

______ 208. silver nitrate + potassium sulfate → silver sulfate + potassium nitrate

______ 209. silver cyanide + potassium → potassium cyanide + silver

______ 210. nitrogen + hydrogen → ammonia

______ 211. zinc carbonate → zinc oxide + carbon dioxide

Directions: Write, balance and predict the products for each of the following reactions.

212. The double replacement rxn between sodium hydroxide and calcium nitrate:

213. The double replacement rxn between hydrogen sulfide and cadmium nitrate:

214. The decomposition of aluminum chloride:

215. The decomposition of sodium chloride:

216. The single replacement rxn between aluminum and lead (II) oxide:

217. The double replacement rxn between silver acetate and potassium chromate

218. The decomposition of water to produce gaseous products:

219. The direct combination (synthesis) of iron (III) oxide from a metal and a gas:

Directions: Write, balance, identify the type, and predict the products for each of the following reactions.

220. magnesium + zinc nitrate →

221. aluminum + phosphoric acid →

222. potassium + chlorine gas →

223. chromium (III) chloride + sulfuric acid →

Predicting Products

Directions: Predict the product and balance each of these reactions. List the reaction type

abbreviation to the left of each reaction.

________ 224. CuCl2

________ 225. N2 + H2

________ 226. Ca + AlCl3

________ 227. Al(NO3)3 + FeCl2

________ 228. C3H6 + O2

229. Aluminum sulfate reacts with barium chloride

230. Zinc reacts with copper (I) sulfate

231. Sodium chloride decomposes.

232. Calcium metal reacts with oxygen

233. Butane, C4H10, burns in air

Balancing Practice Quiz

Identify the type, predict the products if it occurs, and balance the following reactions:

234. _____ Ba + O2→

235. _____ Zn + CuSO4 →

236. _____ Ag + FeSO4 →

237. _____ BaCl2 + Na3PO4 →

238. _____ C6H12O6 + O2→

239. _____ Zn + Pb(NO3)2 →

240. _____ Cu + MgSO4 →

241. _____ KClO3 →

242. _____ C4H8 + O2→