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Chemistry 5
Chapter 8 Chemical EquationsName________________________________
Due by Friday, March 24th 2017
Chemical Equations Introduction:
Write complete equations for the following:
1. Two moles of solid sodium chloride decompose when exposed to an electric current into two moles of sodium metal and 1 mole of chlorine gas.
2. One mole of barium chloride in solution reacts with one mole of sodium sulfate in solution to produce 1 mole of solid barium sulfate and 2 moles of sodium chloride in solution.
3. Two mole of solid potassium chlorate, when heated, decompose into two moles of solid potassium chloride and 3 moles of oxygen gas.
4. One mole of solid calcium carbonate decomposes when heated into one mole of solid calcium oxide and 1 mole of carbon dioxide gas.
5. Two moles of solid aluminum hydroxide decomposes when heated into one mole of solid aluminum oxide and three moles of water vapor.
6. One mole of zinc metal when mixed with two moles of a hydrochloric acid solution react and produce one mole of zinc chloride in solution and one mole of hydrogen gas.
7. Eight moles of fluorine gas are bubbled through a solution containing eight moles of potassium sulfide and react to produce sixteen moles of potassium fluoride in solution and one mole of solid sulfur.
Balancing Equations: Balance the following reactions. Place a B at the beginning of any that are balanced as written.
8. _____ Zn + _____O2 _____ZnO
9. _____HI _____H2 + _____I2
10. _____B + _____F2 _____BF3
11. _____N2 + _____H2 _____NH3
12. _____Fe + _____H2O _____Fe3O4 + _____H2
13. _____BaCl2 + _____H2SO4 _____BaSO4 + _____HCl
14. _____P4 + _____O2 _____P4O10
15. _____KClO3 _____KCl + _____O2
16. _____C3H8 + _____O2 _____CO2 + _____H2O
17. _____Cu + _____AgNO3 _____Cu(NO3)2 + _____Ag
18. _____Te + _____H2O _____TeO + _____H2
19. _____La(NO3)3 + _____NaOH _____La(OH)3 + _____NaNO3
20. _____RhO3 _____RhO + _____O2
21. _____Hf + _____N2 _____Hf3N4
22. _____Ga + _____H2SO4 _____Ga2(SO4)3 + _____H2
23. _____PdCl2 + _____HNO3 _____Pd(NO3)2 + _____HCl
24. _____RbBr + _____AgCl _____AgBr + _____RbCl
25. _____PaI5 _____Pa + _____I2
26. Na + O2 Na2O
27. H2 + O2 H2O
28. Na2SO4 + CaCl2 CaSO4 + NaCl
29. Al2O3 Al + O2
30. C2H6 + O2 CO2 + H2O
31. SO3 + H2O H2SO4
32. SiCl4 Si + Cl2
33. C + H2 CH4
34. Br2 + NaI NaBr + I2
35. Zn + HCl ZnCl2 + H2
36. H2S + O2 H2O + SO2
37. Ba(NO3)2 + Na2SO4 BaSO4 + NaNO3
38. C5H12 + O2 CO2 + H2O
39. HgO Hg + O2
40. H2SO4 + Pb + PbO2 PbSO4 + H2O
41. C6H12O6 + O2 CO2 + H2O
42. Ca + H2O Ca(OH)2 + H2
43. C6H12O6 C2H5OH + CO2
44. HC2H3O2 + NaHCO3 CO2 + NaC2H3O2 + H2O
45. NaCl + SO2 + H2O + O2 Na2SO4 + HCl
46. Fe2O3 + CO CO2 + Fe
47. Ca3(PO4)2 + C + SiO2 CaSiO3 + CO + P4
48. aluminum+hydrochloric acidaluminum chloride+hydrogen
49. chromium(III) hydroxide + nitric acid water+chromium(III) nitrate
50. chromium + hydrobromic acid chromium (III) bromide + hydrogen
51. krypton difluoride + water krypton + oxygen + hydrofluoric acid
52. chlorine + water hydrochloric acid + oxygen
53. CH3OH + O2 CO2+H2O
54. Si2H6+O2SiO2+H2O
55. CH3NH2+O2CO2+H2O+N2
56. Na2SiO3+HFH2SiF6+NaF+H2O
57. NH3+O2NO+H2O
58. Sb2S3+HClH3SbCl6+H2S
59. Al+NaOH+H2ONaAl(OH)4+H2
60. C2H5Cl+NaPb(C2H5)4Pb+NaCl +Pb
Types of Reactions: Balance the following equations and indicate the type of reaction on the line provided.
61. NaCl Na + Cl2_____________________
62. Na + Cl2 NaCl_____________________
63. C2H4 + O2 CO2 + H2O_____________________
64. H2O H2 + O2_____________________
65. H2 + O2 H2O_____________________
66. C8H18 + O2 CO2 + H2O_____________________
67. NaOH + HCl H2O + NaCl_____________________
68. Na + HCl H2 + NaCl_____________________
69. K + Cl2 KCl_____________________
70. K + AgCl Ag + KCl_____________________
71. C6H12 + O2 CO2 + H2O _____________________
72. Ca + S8 CaS_____________________
73. KOH + HNO3 H2O + KNO3 _____________________
74. Al + O2 Al2O3_____________________
75. HgO Hg + O2_____________________
76. NaOH + H2SO4 Na2SO4 + H2O_____________________
77. Fe + O2 Fe2O3_____________________
78. C6H8 + O2 CO2 + H2O_____________________
79. Pb(NO3)2 + K2CrO4 PbCrO4 + KNO3_____________________
80. H2 + N2 NH3_____________________
81. C3H5(NO3)3 CO2 + N2 + H2O + O2_____________________
Decomposition, Synthesis, and Combustion
82. Pt2O
83. Mg(ClO3)2
84. P2O5
85. SrO + H2O
86. BaCO3
87. HNO3(aq)
88. C4H10 + O2
89. Al + O2
90. Cl2O3 + H2O
91. Al(OH)3
92. iron(III) chlorate is heated
93. zinc oxide powder is added to water
94. pentane (C5H12) is ignited in air
95. phosphorous acid is heated
96. magnesium phosphide is exposed to an electric current
97. lithium hydroxide is heated
98. hydrogen gas is ignited in air
99. magnesium ribbon is heated in the presence of sulfur
100. scandium carbonate is heated
101. dinitrogen pentoxide gas is bubbled through water
Single Replacement
102. Zn + CuSO4
103. Pb + Mg(NO3)2
104. AgC2H3O2 + Li
105. Cl2 + KBr
106. HF(aq) + Ca
107. magnesium + nitric acid
108. sodium chloride + aluminum
109. barium + calcium sulfate
110. nickel(II) sulfate + lithium
111. potassium + water
112. silver + strontium chloride
113. sodium fluoride + iodine
114. rubidium + iron(III) sulfate
115. sodium + water
116. fluorine + aluminum bromide
117. phosphoric acid + calcium
118. copper + water
Double Replacement
119. AgCH3COO + CaSO4
120. Pb(NO3)2 + Na2S
121. AgNO3 + FeCl3
122. H2SO4 +Ba(OH)2
123. Al(OH)3 +NH4Cl
124. A solution of lead(II) chlorate is mixed with a solution of chromium(III) iodide.
125. A solution of nitric acid is added to a solution of magnesium hydroxide.
126. Solutions of copper(II) chloride and potassium carbonate are mixed.
127. Solid sodium carbonate is sprinkled on a hydrochloric acid spill.
128. Perchloric acid is neutralized by the addition of ammonium hydroxide.
Energy and Change of Enthalpy
129. Indicate the following as either exothermic or endothermic.
a) CH4 + 74.4 kJ C + 2H2 a) ___________________
b) 1/8 S8 + O2 SO2b) ___________________
c) 3 C + 4 H2 C3H8 + 104 kJc) ___________________
d) butane + oxygen carbon dioxide + water d) ___________________
e) CO2 CO + O2 H = +238kJe) ___________________
130. The energy term of an exothermic reaction is added to the (right / left) side of chemical equation because energy is (absorbed / released).
131. The H of an endothermic reaction is indicated as a (+ / ) value because the enthalpy (potential energy) of the reactants is ( > / < ) than the enthalpy of the products.
132. All chemical fuels produce an (endothermic / exothermic) reaction upon ordinary combustion.
133. Baking a potato is an example of an (exothermic / endothermic ) reaction.
134. Copper and oxygen react according to the following:Cu + O2 CuO H = 155kJ Rewrite this equation for 1 mole of O2 and include energy in the equation.
135. Carbon and sulfur react according to the following equation: 4C + S8 + 3511 kJ 4CS2 Rewrite the equation for one mole of C, using the H notation.
136. Draw an energy diagram for the equation given in the previous problem. Be sure to label all parts. (progress of the reaction, enthalpy or energy, H, reactants, and products.
137. Using the graph below, determine:
a. The activation energy needed for the forward reaction?___________________
b. The activation energy needed for the reverse reaction? ___________________
c. H for the forward reaction? Endothermic or exothermic? ___________________
d. H for the reverse reaction? Endothermic or exothermic? ___________________
e. Label the activated complex on the curve.
f. Sketch what the curve might look like if a catalyst was added.
138. Draw a potential energy diagram with the following criteria:
a. Hrev = 30 kJ
b. Ea (forward reaction) = 70 kJ
c. Activated Complex = 90 kJ
139. Based on your diagram, determine:
18
a. Hfor_____________________
b. Ea (reverse) _________________
c. Enthalpy of reactants__________________
d. Enthalpy of products_________________
Bond Energy
140. Given:
a. Identify the type and number of bonds broken in this reaction and determine the total amount of energy required to break them.
b. Identify the type and number of bonds formed in this reaction and determine the total amount of energy released when they are formed.
c. Calculate the enthalpy change for the entire reaction.
d. Is this reaction endothermic or exothermic?
e. Write a thermochemical equation for the reaction.
f. Draw and label a potential energy diagram for the reaction.
141. Using bond energies, calculate the enthalpy change for the following reactions:
a.
b.
c.
d.
Ionic Equations and Dissociation Reactions
1. Write appropriate ionization equations or dissociation equations to represent what happens when each of the following chemicals are mixed with water:
a. HNO3(aq)
b. H2SO4(aq)
c. LiOH
d. Ba(OH)2
e. Na2SO4
2. Write molecular, ionic and net ionic equations for each of the following:
a. Solutions of potassium hydroxide and nitric acid are mixed.
b. Solutions of barium chloride and sodium sulfate are mixed.
c. Solid calcium oxide is added to a hydrochloric acid solution
d. Solutions of lithium acetate and copper(II) nitrate are mixed.
e. Solutions of iron(III) bromide and ammonium carbonate are mixed
f. A piece of zinc metal is added to a solution of copper(II) sulfate.
g. Solid lead(II) nitrate crystals are sprinkled into a solution of rubidium iodide.
h. A piece of aluminum metal is added to a solution of silver nitrate.
Review (Identify reaction type before writing the equation)
142. calcium metal is added to a solution of nitric acid.
143. solutions of copper(II) nitrate and sodium hydroxide are mixed.
144. scandium carbonate is heated
145. nitrous acid is heated
146. zinc + magnesium carbonate
147. dichlorine monoxide + water
148. calcium carbonate + perchloric acid
149. strontium chlorate is heated
150. lead(IV) sulfide is exposed to an electric current
151. the combustion of octane (C8H18)
152. silver oxide + water
153. dichromic acid + ammonium hydroxide
154. barium metal is dropped in water
155. copper(II) hydroxide is heated
156. lithium + sulfur
157. bromine + iron(III) iodide
158. solutions of sodium phosphate and calcium bromide are mixed.
159. barium metal is added to a solution of chlorous acid.
160. chloric acid is heated
161. aluminum metal is added to a solution of sodium chlorate
162. dinitrogen pentoxide gas is bubbled through water
163. lithium carbonate is heated
164. ammonium carbonate powder is sprinkled on a hydrochloric acid spill
165. iron(III) phosphide is exposed to an electric current
166. hexane (C6H14) is ignited
167. tin(II) oxide is added to water
168. strontium hydroxide is combined with acetic acid
169. tin(IV) hydroxide is heated
170. a piece of silver metal is held in a Bunsen burner flame
171. lead(II) sulfide is heated in a fluorine environment
172. calcium hydroxide powder is added to an ammonium nitrate solution
173. A hydrocarbon compound is found to be 85.71% carbon and 14.29% hydrogen by mass. When vaporized at 35C, 0.136 g of the compound occupies a volume of 45.0 mL and exerts a pressure of 691 torr. Write a balanced equation for the combustion of this compound.
174. Given:
a. Write a balanced molecular equation in H notation.
b. Is the reaction endothermic or exothermic?
c. Which has a higher enthalpy, the reactants or the products?
d. Would the temperature of the surroundings increase or decrease?
175. For each of the following, write complete and balanced molecular, ionic and net ionic equations.
a. Solutions of lead(II) nitrate and potassium iodide are mixed.
b. Solutions of hydrochloric acid and silver nitrate are mixed.
c. Solutions of sodium hydroxide and iron (III) nitrate are mixed.
Cumulative Review Questions
176. For 2607000 give the following:
a) Number written in scientific notation_________________________
b) Significant figures_________________________
c) Rounded to 3 significant figures_________________________
177. Convert 23.6 hectograms to milligrams
178. A copper cube with a mass of 58.60 g is placed into a water-filled graduated cylinder. The water in the cylinder rises from 26.5 mL to 33.1 mL. Determine the density of the copper?
179. List 3 physical properties and 3 chemical properties of water.
180. Complete the following chart
Homogeneous or Heterogeneous
Element, Compound, Mixture, Solution
rubbing alcohol
calcium oxide
gasoline
181. Write nuclear equations for:
a) Alpha emission of radon-222
b) Electron capture by nitrogen-15
c) Neutron bombardment of oxygen-16
182. What is the mass and charge of 5.26 x 1024 electrons?
183. A 2.65 gram sample of cobalt-55, with a half-life of 17.5 hours undergoes decay for 6.56 days. What mass of cobalt-55 remains at this point?
184. An element consists of 1.40% of an isotope with mass 203.973 amu, 24.10% of an isotope with mass 205.9745 amu, 22.10% of an isotope with mass 206.9759 amu, and 52.40% of an isotope with mass 207.9766 amu. Calculate the average atomic mass and identify the element.
185. Where appropriate, write formulas or names for each of the following:
a. ammonium sulfate ___________f) H3AsO4(aq)_________________________
b. dinitrogen monoxide___________g) FeSO3_________________________
c. phosphorous acid___________h) CuSO45H2O ______________________
d. lead(IV) oxalate___________i) BF3_________________________
e. aluminum nitrite___________j) Cr(OH)3_________________________
186. Determine the mass, in grams, of 4.22 x 1024 formula units of copper(I) sulfide.
187. What is the total number of electrons in 0.915 moles of nitrogen atoms?
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