Chemical Equations Homework
(ALL work for this unit must be done on a separate sheet of paper.)
I. Writing Complete Balanced Equations
Write a balanced complete chemical equation to represent each of the following chemical reactions.
1. Silver nitrate when added to sodium bromide produces sodium nitrate and silver bromide.
2. Potassium iodide and lead (II) nitrate react to form lead (II) iodide and potassium nitrate.
3. Iron (III) chloride and ammonium hydroxide will react to yield iron (III) hydroxide and ammonium chloride.
4. Sodium peroxide when added to water will produce sodium hydroxide and oxygen gas.
5. Iron and water react to form hydrogen gas and iron (III) oxide.
6. Aluminum and sulfuric acid will react to form aluminum sulfate and hydrogen gas.
7. Carbon dioxide and water in the atmosphere will react to form carbonic acid, or acid rain.
8. Calcium chloride and nitric acid mix to form calcium nitrate and hydrochloric acid.
9. Potassium carbonate will react with barium chloride to produce potassium chloride and barium carbonate.
10. Potassium hydroxide will react with phosphoric acid to yield potassium phosphate and water.
11. Water and diphosphorus pentoxide will react to produce phosphoric acid.
12. Fluorine will react with sodium hydroxide to form sodium fluoride, oxygen and water.
13. Potassium fluoride and barium bromide will react to yield barium fluoride and potassium bromide.
14. Ammonia and sulfuric acid will react to produce ammonium sulfate.
15. Hydrochloric acid will react with ammonia to form ammonium chloride.
16. Calcium and water will react to produce calcium hydroxide and hydrogen.
17. Lead (II) nitrate when heated decomposes into lead monoxide, nitrogen dioxide, and oxygen gas.
18. Ammonium bicarbonate when heated decomposes into ammonia, water, and carbon dioxide.
19. Iron and sulfur react to form ferrous sulfide.
20. Hydrogen and oxygen combine to form water.
21. Sodium hydroxide reacts with hydrochloric acid to form sodium chloride and water.
22. Water is decomposed to produce hydrogen gas and oxygen gas.
23. Carbonic acid decomposes to produce water and carbon dioxide.
24. Sodium combines with water to produce sodium hydroxide and hydrogen gas.
25. Nitrogen reacts with hydrogen to produce ammonia.
26. Iron and oxygen combine to produce iron (III) oxide.
27. Potassium chlorate decomposes to produce potassium chloride and oxygen gas.
28. Aluminum and oxygen combine to form aluminum oxide.
29. Iron (III) oxide and carbon combine to form iron and carbon monoxide.
30. Iron (III) chloride and potassium hydroxide react to form potassium chloride and iron (III) hydroxide.
31. Sodium carbonate and calcium hydroxide react to form sodium hydroxide and calcium carbonate.
32. Calcium and water combine to form calcium hydroxide and hydrogen gas.
33. Carbon dioxide and carbon combine to form carbon monoxide.
34. Ammonium chloride and sodium nitrite react to form sodium chloride, nitrogen and water.
35. Ammonia reacts with hydrogen chloride to form ammonium chloride.
36. Calcium carbonate decomposes to form calcium oxide and carbon dioxide.
37. Barium oxide react with water to form barium hydroxide.
38. Acetaldehyde (CH3CHO) decomposes to form methane (CH4) and carbon monoxide.
39. Zinc react with cupric nitrate to form zinc nitrate and copper.
40. Calcium sulfite decomposes to form calcium oxide and sulfur dioxide.
41. Iron reacts with sulfuric acid to form iron (III) sulfate and hydrogen gas.
42. Azomethane (C2H6N2) decomposes to form ethane (C2H6) and nitrogen gas at 297oC.
43. Carbon monoxide reacts with chlorine gas to form phosgene (COCl2)
44. Manganese (II) iodide decomposes when exposed to light to form manganese and iodine.
45. Dinitrogen pentoxide reacts with water to produce nitric acid.
46. Magnesium reacts with titanium (IV) chloride to produce magnesium chloride and titanium
47. Carbon reacts with zinc oxide to produce zinc and carbon dioxide.
48. Bromine reacts with sodium iodide to form sodium bromide and iodine.
49. Phosphorus trichloride reacts with chlorine gas to produce phosphorus pentachloride.
50. Phosphorus reacts with bromine to produce phosphorus tribromide.
51. Calcium hydride reacts with water to produce calcium hydroxide and hydrogen gas.
52. Sulfuric acid reacts with potassium hydroxide to produce potassium sulfate and water.
53. Propane (C3H8) reacts with oxygen gas to produce carbon dioxide and water.
II. Types of Reactions
Identify each of the equations as synthesis, decomposition, single replacement, double replacement, or organic combustion. Some of the equations are not balanced, for extra practice, balance them.
1. HgO à Hg + O2
2. NaCl + AgNO3 à NaNO3 + AgCl
3. Mg + HCl à MgCl2 + H2
4. Zn + H2SO4 à ZnSO4 + H2
5. NaOH + HCl à NaCl + H2O
6. Al2(SO4)3 + Ca(OH)2 à Al(OH)3 + CaSO4
7. H2 + O2 à H2O
8. Cl2 + NaBr à NaCl + Br2
9. Zn + CuSO4 à ZnSO4 + Cu
10. KClO3 à KCl + O2
11. H2O + Fe à Fe2O3 + H2
12. Ca(OH)2 + HNO3 à Ca(NO3)2 + H2O
13. Na2O + CO2à Na2CO3
14. H2 + N2 à NH3
15. HgO + Cl2 à HgCl + O2
16. Na + Br2 à NaBr
17. Al2O3 à Al + O2
18. CuCl2 + H2O à CuS + HCl
19. NaOH + H2SO4 à Na2SO4 + H2O
20. Fe + O2 à Fe2O3
21. Pb(NO3)2 + K2CrO4 à KNO3 + PbCrO4
22. C3H5(NO3)3 à CO2 + N2 + H2O + O2
23. Fe + CuCl2 à FeCl2 + Cu
24. P4 + O2 à P4O10
25. Zn + HCl à ZnCl2 + H2
26. Mg + O2 à MgO
27. FeS2 + O2 à Fe2O3 + SO2
28. Na + O2 à Na2O
29. Na2SO4 + CaCl2 à CaSO4 + NaCl
30. Fe + H2O à Fe3O4 + H2
31. C2H6 + O2 à CO2 + H2O
32. SiCl4 à Si + Cl2
33. C + H2 à CH4
34. CH4 + O2 à CO2 + H2O
35. Na + I2 à NaI
36. N2 + O2 à N2O
37. KI + Cl2 à KCl + I2
38. HCl + Ca(OH)2 à CaCl2 + H2O
39. K3PO4 + HCl à KCl + H3PO4
40. S + O2 à SO3
41. KI + Pb(NO3)2 à KNO3 + PbI2
42. CaSO4 + AlBr3 à CaBr2 + Al2(SO4)3
43. H2O2 à H2O + O2
44. Na + H2O à NaOH + H2
45. Mg(NO3)2 + K3PO4 à Mg3(PO4)2 + KNO3
46. AgNO3 + MgCl2 à AgCl + Mg(NO3)2
47. AlBr3 + K2SO4 à KBr + Al2(SO4)3
48. C3H8 + O2 à CO2 + H2O
49. C8H18 + O2 à CO2 + H2O
50. FeCl3 + NaOH à Fe(OH)3 + NaCl
51. P + O2 à P2O5
52. S8 + O2 à SO3
53. C6H12O6 + O2 à CO2 + H2O
54. HCl + CaCO3 à CaCl + H2O + CO2
III. Predicting Products of Chemical Reactions
Predict the products of the reactions below. Then, write the balanced equation and classify the reaction. For elements that have multiple charges for their ions the oxidation number for the ion you are expected to use is in parentheses.
1. magnesium bromide and chlorine
2. aluminum and iron (III) oxide
3. silver nitrate and zinc chloride
4. hydrogen peroxide
5. zinc and hydrochloric acid
6. sulfuric acid and sodium hydroxide
7. sodium and hydrogen
8. acetic acid and copper (II)
9. lead (II) and cupric nitrate
10. barium chloride and sodium sulfate
11. chlorine gas and sodium iodide
12. magnesium and nitrogen gas
13. cobaltous nitrate and hydrosulfuric acid
14. C2H5OH and oxygen gas
15. chromium (III) and cadmium chloride
16. bromine and potassium chloride
17. aluminum and oxygen gas
18. barium nitrate and sodium phosphate
19. iodine and sodium bromide
20. C3H4 and oxygen gas
IV. Conservation of Mass
Use the law of conservation of matter to solve the following problems.
1. 2KClO3 à 2KCl + 3O2 If 500 g of KClO3 decomposes and produces 303 g of KCl, how many grams of O2 are produced?
2. N2 + 3H2 à 2NH3 How many grams of hydrogen are needed to react with 100 g of nitrogen to produce 121 g of ammonia?
3. 4Fe + 3O2 à 2Fe2O3 How many grams of oxygen are needed to react with 350 g of iron to produce 500 g of iron (III) oxide?
4. CH4 2O2 à CO2 + 2H2O 16 g of methane (CH4) react with 64 g of oxygen producing 44 g of carbon dioxide. How many grams of water are produced?
5. CaCO3 à CaO + CO2 How much carbon dioxide is produced from the decomposition of 200 g of calcium carbonate, if 112 g of calcium oxide are produced?