University:
Winston-Salem Forsyth County Schools
Course:
AP Chemistry
Academic year:

2002
Views:

32

Pages:

11
Author:

cesaraquinojb1i

Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus (V) oxide powder is sprinkled over distilled water. 3. Solid potassium oxide is added to water. 4. Solid calcium oxide is heated in the presence of sulfur trioxide gas. 5. Calcium metal is heated strongly in nitrogen gas. 6. Drops of dinitrogen trioxide are added to distilled water. 7. Excess chlorine gas is passed over hot iron filings. 8. The gases boron trifluoride and ammonia are mixed. 9. Carbon dioxide gas is bubbled into magnesium oxide. 10. Samples of boron trichloride gas and ammonia gas are mixed. 11. Magnesium solid is heated in the presence of nitrogen gas. 12. Sulfur dioxide gas is bubbled into calcium oxide. 13. Solid sodium oxide is added to distilled H2O. 14. Sulfur dioxide gas is bubbled into distilled H2O. 15. Phosphorus trihydride gas is bubbled into liquid boron trichloride. Double Replacement 1. Excess concentrated sulfuric acid is added to solid calcium phosphate. 2. Hydrogen sulfide gas is bubbled into a solution of mercury (II) chloride. 3. Solutions of manganese (II) sulfate and ammonium sulfide are mixed. 4. An excess of sodium hydroxide solution is added to a solution of magnesium nitrate. 5. Solid lithium hydride is added to water. 6. Carbon dioxide is bubbled through water containing a suspension of calcium carbonate. 7. Solutions of ammonia and hydrofluoric acid are mixed. 8. Equal volumes of 0.1 M sulfuric acid and 0.1 M potassium hydroxide are mixed. 9. A solution of copper (II) sulfate is added to a solution of barium hydroxide. 10. Equal volumes of equimolar solutions of disodium hydrogen phosphate and hydrochloric acid are mixed. 11. Ammonia gas is bubbled into a solution of ethanoic (acetic) acid. 12. Solid ammonium carbonate is added to a saturated solution of barium hydroxide. 13. Concentrated hydrochloric acid is added to solid manganese (II) sulfide. 14. Magnesium nitrate is added to hot distilled H2O. 15. A solution of tri-potassium phosphate and zinc nitrate are mixed. 16. Dilute sulfuric acid is added to a solution of lithium carbonate. 17. Hydrogen sulfide gas is bubbled into a solution of nickel (II) nitrate. 18. Equal volumes of equimolar solutions of sodium hydroxide and sodium dihydrogen phosphate are mixed. 19. Solutions of zinc sulfate and sodium phosphate are mixed. 20. Solutions of silver nitrate and lithium bromide are mixed. 21. Excess hydrochloric acid solution is added to a solution of potassium sulfide. 22. Solutions of ammonium sulfate and barium hydroxide are mixed. 23. An acetic acid solution is mixed with a sodium bicarbonate solution. 24. Dilute sulfuric acid is added to solid calcium fluoride. 25. Dilute hydrochloric acid is added to dilute mercury (I) nitrate solution. 26. Solutions of cobalt (II) nitrate and sodium hydroxide are mixed. 27. Equal volumes of equimolar solutions of phosphoric acid and potassium hydroxide are mixed. 28. Excess potassium hydroxide solution is added to a solution of aluminum nitrate. 29. Solid potassium amide is added to distilled H2O. 30. A solution of nickel (II) chloride is added to a solution of sodium sulfide. Redox 1. A stream of chlorine gas is passed through a solution of cold, dilute sodium hydroxide. 2. A solution of iron (II) nitrate is exposed to air for an extended period of time. 3. A concentrated solution of hydrochloric acid is added to solid potassium permanganate. 4. A solution of potassium dichromate is added to an acidified solution of iron (II) chloride. 5. A solution of potassium iodide is electrolyzed. 6. A concentrated solution of hydrochloric acid is added to powdered manganese dioxide and gently heated. 7. Solutions of potassium permanganate and sodium oxalate are mixed. 8. A strip of copper is immersed in dilute nitric acid. 9. Potassium permanganate solution is added to an acidic solution of hydrogen peroxide. 10. A strip of silver is immersed in dilute nitric acid. 11. A solution of Iron (II) nitrate is added to a basic solution of hydrogen peroxide. 12. A solution of tin (II) chloride is added to an acidic solution of potassium permanganate. 13. Solid sodium dichromate is added to an acidified solution of sodium iodide. 14. Solutions of potassium iodide and potassium iodate are mixed in an acidic solution. 15. Hydrogen peroxide is added to an acidified solution of sodium bromide. 16. Solutions of tin (II) chloride and iron (III) chloride are mixed. 17. A solution of sodium bromide is added to an acidified solution of potassium bromate. 18. Hydrogen gas is passed over hot iron (II) oxide powder. Complexation 1. Excess sodium cyanide solution is added to a solution of silver nitrate. 2. An excess of nitric acid solution is added to a solution of tetraamminecopper (II) sulfate. 3. Solid aluminum oxide is added to a solution of sodium hydroxide. 4. Concentrated ammonia solution is added to a solution of zinc iodide. 5. Excess concentrated ammonia solution is added to a suspension of silver chloride. 6. Excess concentrated potassium hydroxide solution is added to a precipitate of zinc hydroxide. 7. Excess concentrated sodium hydroxide solution is added to a precipitate of aluminum hydroxide. 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride. 9. A concentrated solution of ammonia is added to a suspension of zinc hydroxide. 10. Excess hydrochloric acid is added to a solution of diammine silver (I) nitrate. Combustion 1. Ethanol is burned in oxygen gas. 2. Solid copper (II) sulfide is strongly heated in oxygen gas. 3. Propanol is burned in oxygen gas. 4. Carbon disulfide vapor is burned is excess oxygen. 5. Ethene gas is burned in air. Single Reaction 1. A bar of zinc metal is immersed in a solution of copper (II) sulfate. 2. A piece of sodium metal is added to distilled water. 3. A piece of aluminum is added to a solution of silver nitrate. 4. A piece of nickel is immersed in a solution of copper (II) sulfate. 5. Chlorine gas is bubbled into a solution of sodium bromide. 6. A solution of tin (II) chloride is added to a solution of iron (III) sulfate. 7. Solid calcium is added to distilled water. 8. A piece of lead is immersed in a solution of silver nitrate. 9. Hydrogen gas is passed over hot iron (III) oxide. 10. A strip of zinc is added to a solution of 6.0 molar hydrobromic acid. Solutions: Redox 1. C12 + OH- Æ Cl- + ClO- + H2O (89)(95) 2. Fe2+ + O2 + H2O Æ Fe2O3 + Fe(OH)3 (95) 3. H+ + Cl- + KMnO4 Æ K+ + Mn2+ + Cl2 + H2O (94) 4. Cr2O72- + Fe2+ + H+ Æ Cr3+ + Fe3+ + H2O (94) 5. I- + H2O Æ I2 + H2 + OH- (92) 6. H+ + Cl- + MnO2 Æ Mn2+ + Cl 2 + H2O (91) 7. MnO4- + C2O42- Æ MnO2 + CO2 (96) 8. Cu + H+ + N03- Æ Cu2+ + NO2 + H2O (93) 9. MnO4- + H202 Æ Mn2+ + O2 + H2O (93) 10. Ag+ + H+ + N03- Æ Ag0 + NO2 + H20O (87) 11. H2O2 + Fe2+ Æ Fe3+ + H2O (87) 12. Sn2+ + H+ + MnO4- Æ Sn4+ + Mn2+ + H2O (89) 13. Na2Cr2O7 + I- + H+ Æ Cr3+ + I2 + H2O + Na+ (81) 14. H+ + I- + IO3- Æ I2 + H2O (82) 15. H2O2 + Br- + H+ Æ Br2 + H2O (82) 16. Sn2+ + Fe3+ Æ Sn4+ + Fe2+ (98) 17. H+ + Br- + BrO3- Æ Br2 + H2O (97) 18. H2 + FeO Æ H2O + Fe (97) (Fe(OH)3) Single Replacement 1. Zn + Cu2+ Æ Zn2+ + Cu (95) 2. Na + H2O Æ Na+ + OH- + H2 (94)(85) 3. Al + Ag+ Æ Al+3 + Ag (92) 4. Ni + Cu2+ Æ Ni+2 + Cu (96) 5. C12 + Br- Æ Cl- +Br2 (96) 6. Sn2+ + Fe3+ Æ Sn4+ + Fe2+ (85) 7. Ca + H2O Æ Ca(OH)2 + H2 (87) 8. Pb + Ag+ Æ Pb2+ + Ag (81) 9. H2 + Fe2O3 Æ Fe + H2O 10. Zn + H+ Æ Zn2+ + H2 (FeO) (82) (98) Double Replacement Precipitation Reactions, Solubility Rules, Acid-Base Reactions 1. H2SO4 + Ca3(PO4)2 Æ H3PO4 + CaSO4 (95) 2. H2S + Hg+2 Æ HgS + H+ (95) 2+ 2- 3. Mn + S Æ MnS (94) 4. Mg2+ + OH- Æ Mg(OH)2 (92) 5. LiH + H2O Æ Li + OH- + H2 2+ 6. CaCO3 + H20 + C02 Æ Ca + HCO3 (H2CO3) (92) - 7. NH3 + HF Æ NH4+ + F+ - (92) (92) 8. H + OH Æ H2O (91) 9. Cu2+ + SO42- + Ba2+ +OH- Æ Ca(OH)2 + BaSO4 (91) 10. HPO4-2 + H+ Æ H2PO4- (96) 11. NH3 + HC2H3O2 Æ C2H3O2- + NH4+ (96) 12. (NH4)2CO3 + Ba2+ + OH- Æ NH3 + BaCO3 + H2O (96) 13.H+ + MnS Æ H2S + Mn2+ (93) 14. Mg3N2 + H2O Æ Mg(OH)2 + NH3 (93) 15. Zn2+ + PO43- Æ Zn3(PO4)2 (93) 16. H+ + HCO3- Æ H2O + CO2 (85) 17. H2S + Ni2+ Æ NiS + H+ (87) 18. OH- + H2PO4- Æ PO43- + H2O (87) 19. Zn2+ + PO43- Æ Zn3(PO4)2 (89) 20. Ag+ + Br- Æ AgBr (89) 21. H+ + SO32- Æ H2O + SO3 (H2SO3) (89) 22. NH4+ + SO42- + Ba2+ + OH- Æ BaSO4 + NH3 + H2O (81) 23. HC2H3O2 + HCO3- Æ C2H3O2- + H2O + CO2 (81) 24. H+ + SO4-2 + CaF2 Æ HF + CaSO4 (82) 25. Hg2+ + Cl- Æ Hg2Cl2 (82) 26. Co2+ + OH- Æ Co(OH)2 (98) 27. H3PO4 + OH- Æ H2PO4- + H2O (98) 28. A13+ + OH- Æ Al(OH)3 (97) 29. KNH2 + H2O Æ NH3 + K+ + OH- (97) 30. Ni2+ + S2- Æ NiS or (Ni2+ + H2S) (97) Decomposition/Composition Decomposition 1. (NH4)2CO3 Æ NH3 + H2O + CO2 (82)(94) 2. CaCO3 Æ CaO + CO2 (96) 3. CaSO3 Æ CaO + SO2 (98) Composition 1. BaO + H2O ÆBa2+ + 2 OH- (95) 2. P4O10 + H2O Æ H3PO4 (94) + 3. K2O + H2O Æ K + OH - (92) 4. CaO + SO3 Æ CaSO4 (91) 5. Ca + N2 Æ Ca3N2 (91) 6. N2O3 + H2O Æ HNO2 (96) 7. Fe + Cl2 Æ FeCl3 (93) 8. BF3 + NH3 Æ BF3NH3 (85) 9. MgO + CO2 Æ MgCO3 (87) 10. BC13 + NH3 Æ BC13NH3 (89) 11. Mg + N2 Æ Mg3N2 (81) 12. SO2 + CaO Æ CaSO3 + 13. Na2O + H2O Æ Na + OH (81) - (98) 14. SO2 + H2O Æ H2SO3 (97) 15. PH3 + BCl3 Æ H3PBCl3 (97) 16. Mg + N2 Æ Mg3N2 (97) Complex Ion Formations 1. CN- + Ag+ Æ Ag(CN)2- (94) 2. H+ + Cu(NH3)42+ Æ Cu2+ +NH4+ (92) 3. Al2O3 + OH- Æ Al(OH)4- (91) 4. Zn + NH3 --. Zn(NH3)42+ (91) 5. AgCl + NH3 Æ Ag(NH3)2+ + Cl- (93) 6. Zn2+ + OH- Æ Zn(OH)42- (85) 7. OH- + Al(OH)3 Æ Al(OH)4- (87) 8. Fe3+ + SCN- Æ Fe(SCN)2+ (81)(89) 9. Zn(OH)2 + NH3 Æ Zn(NH3)42+ + OH- (82) 10. H+ + Cl- + [ Ag(NH3)2]+ Æ AgCl + NH4+ (98) Combustion 1. C2H5OH + O2 Æ CO2 + H2O 2. CuS+ O2 Æ Cu + SO2 (81)(95) (CuO, Cu2O) (91) 3. SO2+ OH-Æ HSO3- (93) 4. C3H7OH + O2 Æ CO2 + H2O (87) 5. CS2 + O2 Æ CO2 + SO2 (SO3) (89) 6. C2H4 + O2 Æ CO2 + H2O (98)

AP Reactions: Decomposition