Download Balance the following chemical equations: (Some may already be

Balance the following chemical equations: (Some may already be balanced.)
1.
H 2 + O 2 H 2O
26. N2 + H2 NH3
2.
S8 + O2 SO3
27. N2 + O2 3.
HgO Hg + O2
28. CO2 + H2O C6H12O6 + O2
4.
Zn + HCl ZnCl2 + H2
29. SiCl4 + H2O H4SiO4 + HCl
5.
Na + H2O NaOH + H2
30. H3PO4 H4P2O7 + H2O
6.
C10H16 + Cl2 C + HCl
31. CO2 + NH3 OC(NH2)2 + H2O
N 2O
7.
Si2H3 + O2 SiO2 + H2O
32. Al(OH)3 + H2SO4 Al2(SO4)3 + H2O
8.
Fe + O2 Fe2O3
33. Fe2(SO4)3 + KOH 9.
C7H6O2 + O2 CO2 + H2O
34. H2SO4 + HI H2S + I2 + H2O
K2SO4 +
Fe(OH)3
10. FeS2 + O2 Fe2O3 + SO2
35. Al + FeO Al2O3 + Fe
11. Fe2O3 + H2 Fe + H2O
36. Na2CO3 + HCl NaCl + H2O + CO2
12. K + Br2 KBr
37. P4 + O2 P2O5
13. C2H2 + O2 CO2 + H2O
38. K2O + H2O KOH
14. H2O2 H2O + O2
39. Al + O2 Al2O3
15. C7H16 +
O2 CO2
16. SiO2 + HF SiF4
17. KClO3 KCl
+ H 2O
+
H 2O
40. Na2O2 + H2O NaOH + O2
41. C + H2O CO + H2
42. H3AsO4 As2O5 + H2O
+ O2
18. KClO3 KClO4 + KCl
43. Al2(SO4)3 + Ca(OH)2 Al(OH)3 + CaSO4
+ H2O H3PO4
44. FeCl3 + NH4OH Fe(OH)3 + NH4Cl
19. P4O10
20. Sb + O2 Sb4O6
21. C3H8 + O2 22. Fe2O3 +
23. PCl5
CO + H 2O CO2
45. Ca3(PO4)2 + SiO2 P4O10 + CaSiO3
+ H 2O
Fe + CO2
HCl + H3PO4
46. N2O5 + H2O HNO3
47. Al + HCl AlCl3 + H2
48. H3BO3 H4B6O11
+
H 2O
24. H2S + Cl2 S8 + HCl
49. Mg + N2 Mg3N2
25. Fe + H2O Fe3O4
50. NaOH + Cl2 NaCl + NaClO + H2O
+ H2
The boxes shown below are pictorial representations of chemical reactions. The boxes on the left represent
the reactants and the boxes on the right represent the products. Convert each diagram into a balanced
chemical equation. Assume the reactions occur in the gas phase.
1.
When writing formulas for the compounds in this problem, write hydrogen first. For
compounds containing only oxygen and sulfur, write sulfur first in the formula.
Hydrogen
Oxygen
Sulfur
2.
When writing formulas for the compounds in this problem, write hydrogen first for
compounds that contain only hydrogen and oxygen. For compounds containing carbon,
write carbon first in the formula.
Hydrogen
Oxygen
Carbon
For each of the ionic and molecular compounds listed below, show how the compound dissociates or
ionizes when placed in water. In the middle column, show the dissociation or ionization reaction and in
the last column show the best representation of that compound in water. If the compound is insoluble,
write insoluble in the middle column. When you are finished, circle all of the compounds that are acids
and bases.
Compound
hypochlorous acid
sodium chloride
hydroiodic acid
silver chloride
sodium carbonate
zinc nitrate
ammonia (NH3)
potassium hydroxide
strontium acetate
HC2H2ClO2
iron(III) sulfate
perchloric acid
mercury(I) sulfide
HCN
ammonium
perchlorate
sodium hydroxide
potassium oxalate
H2SO4
aluminum perchlorate
potassium dihydrogen
phosphite
HC2H3O2
CH3COOH
Dissociation or Ionization Reaction
How Substance Exists in
Water
HClO(aq) + H2O(l)  H3O+(aq) + ClO-(aq)
HClO(aq)
CHEM 130
Fall 2012
Convert each statement below into a balanced chemical equation. If the
products are not given, you must predict what the products will be. Most of the
reactions in which you have to predict the products are double displacement
reactions, the others are combustion reactions. In your balanced chemical
equation, make sure you include the physical states of the reactants and
products.
1)
Potassium metal reacts with fluorine gas to produce potassium fluoride.
2)
Nitrogen gas reacts with hydrogen gas under high temperature to form ammonia
gas.
3)
Sulfur trioxide gas dissolves in water to form sulfuric acid.
4)
Solid calcium carbonate is heated to form solid calcium oxide & carbon dioxide gas.
5)
Water undergoes electrolysis to form oxygen gas & hydrogen gas.
CHEM 130
Fall 2012
6)
Aluminum metal is placed in aqueous hydrocloric acid and forms aqueous aluminum
chloride and hydrogen gas.
7)
Copper metal is immersed in a silver chlorite solution, aqueous copper(II) chlorite
and solid silver are formed.
8)
Aqueous barium bromate is mixed with aqueous lithium phosphate.
9)
Hydrochloric acid reacts with solid magnesium hydroxide.
10) Aqueous manganese(V) perchlorate is mixed with aqueous sodium sulfide.
11) Propane gas, C3H8, is burned(combusted).
12) Liquid MTBE, C5H12O, is burned(combusted).
CHEM 130
Fall 2012
Convert each of the statements below into a balanced chemical equation. After
balancing each reaction, write the total ionic equation and the net-ionic
equation. Place a box around the net-ionic equation and list the spectator ions
below this equation. You can predict the products of these reactions by noting
that they are double displacement reactions.
1)
An aqueous solution of lead(II) nitrate is mixed with an aqueous solution of
potassium iodide.
2)
Aqueous calcium chloride is mixed with aqueous ammonium phosphate.
3)
Aqueous platinum(III) bromide reacts with aqueous sodium sulfide.
CHEM 130
4)
Fall 2012
Aqueous hypochlorous acid is mixed with aqueous calcium hydroxide. Assume the
product, calcium hypochlorite, is soluble in water.
5)
Aqueous hydrobromic acid is mixed with aqueous sodium hydroxide.
6)
Aqueous potassium chloride is combined with aqueous magnesium acetate.
7)
Sulfuric acid reacts with potassium hydroxide in deionized water.
CHEM 130
Fall 2012
The two reactions below were problems on my exam during the Fall 2007
semester.
8) Aqueous sulfurous acid is mixed with aqueous potassium hydroxide.
9)
Aqueous copper(II) sulfate is mixed with a solution of cesium phosphate.
The following reactions are oxidation-reduction reactions. Balance each
equation and label the oxidation state of each element. Identify which element
is reduced and which element is oxidized and how many electrons are
transferred between the two elements. Once you have determined the
elements that are oxidized and reduced, identify the reducing and oxidizing
agents.
10)
A solid magnesium ribbon is burned in air to give the solid metal oxide.
CHEM 130
Fall 2012
11) The high temperature of engines cause the nitrogen & oxygen in air to react to form
nitrogen monoxide (a reaction that plays a role in the formation of smog).
12) Solid copper(II) chloride reacts with hydrogen gas to produce gaseous hydrochloric
acid and copper metal.
13) Solid carbon is heated with fluorine gas to give gaseous carbon tetrafluoride.