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AP Chemistry Free Response AP Chemistry Exam Reactions: Questions and Answers With the new format of the exam in 2007 and the availability of both questions and answers on the web at AP Central (http://apcentral.collegeboard.com:80/apc/public/courses/4606.html), I have determined not to update this page any longer. Please create an account as a teacher at AP Central and navigate to the full exams and scoring rubrics which are available back to 2003 Beginning in 2007, question 4 is no longer 5 out of 8 responses but rather three required responses. Also, in addition to writing the reactants and products, the equation must be balanced and there is a question about the chemical reaction. 2007 (a) A solution of sodium hydroxide is added to a solution of lead(II) nitrate. If 1.0 L volumes of 1.0 M solutions of sodium hydroxide and lead(II) nitrate are mixed together, now many moles of product(s) will be produced? Assume the reaction goes to completion. (b) Excess nitric acid is added to solid calcium carbonate. Briefly explain why statues made of marble (calcium carbonate) displayed outdoors in urban areas are deteriorating. (c) A solution containing silver(I) ion (an oxidixing agent) is mixed with a; solution containing iron(II) ion (a reducing agent). If the contents of the reaction mixture described above are filtered, what substance(s), if any, would remain on the filter paper? - 2+ → (a) (i) Balanced equation: 2OH + Pb Pb(OH)2 (s) (ii) The moles of each reactant are obtained by multiplying the volume times the molarity. OH- is 1 mole. Pb2+ is 1 mole. Since the balanced equation shows that 2 moles of OH- are consumed for each 1 mole of Pb2+, the moles of product would be 0.50 moles. + → 2+ (b) (i) Balanced equation: 2H + CaCO3 Ca + H2CO3 (or CO2 + H2O) (ii) Combustion products from automobiles contain nitrogen oxide compounds. When the nitrogen oxides dissolve in water in the air it turns the rain acidic and the reaction above causes the calcium carbonate to slowly dissolve. (c) (i) Balanced equation: Ag+ + Fe2+ → Ag + Fe3+ (ii) One of the products is solid silver metal. When filtered the solid silver metal would appear on the filter paper. 2006 (a) Solid potassium chlorate is strongly heated. (b) Solid silver chloride is added to a solution of concentrated hydrochloric acid. (c) A solution of ethanoic (acetic) acid is added to a solution of barium hydroxide. (d) Ammonia gas is bubbled into a solution of hydrofluoric acid. (e) Zinc metal is placed in a solution of copper(II) sulfate. (f) Hydrogen phosphide (phosphine) gas is added to boron trichloride gas. (g) A solution of nickel(II) bromide is added to a solution of potassium hydroxide. (h) Hexane is combusted in air. → (a) KClO3 KCl + O2 - - → (b) AgCl + Cl [AgCl2] - - (c) HC H O + OH → H O + C H O 2 3 2 2 2 3 2 1 + - → + (d) NH3 + HF NH4 F 2+ 2+ (e) Zn + Cu → Zn + Cu → (f) PH3 + BCl3 H3PBCl3 2+ - → (g) Ni + OH Ni(OH)2 → (h) C6H14 + O2 CO2 + H2O 2005 (a) A strip of zinc is placed in a solution of nickel (II) nitrate. (b) Solid aluminum hydroxide is added to a concentrated solution of potassium hydroxide. (c) Ethyne (acetylene) is burned in air. (d) Solid calcium carbonate is added to a solution of ethanoic (acetic) acid. (e) Lithium metal is strongly heated in nitrogen gas. (f) Boron trifluoride gas is added to ammonia gas. (g) Sulfur trioxide gas is bubbled into a solution of sodium hydroxide. (h) Equal volumes of 0.1 M solutions of lead(II) nitrate and magnesium iodide are combined. (a) Zn + Ni2+ → Zn2+ + Ni - → - (b) Al(OH)3 + OH Al(OH)4 → (c) C2H2 + O2 CO2 + H2O → 2+ - (d) CaCO3 + HC2H3O2 Ca + C2H3O2 + CO2 + H2O → (e) Li + N2 Li3N → (f) BF3 + NH3 BF3NH3 - → 2- (g) SO3 + OH SO4 + H2O 2+ - → (h) Pb + I PbI2 2005 Form B (a) A solution of potassium carbonate is added to a solution of strontium nitrate. (b) Propene is burned in air. (c) Excess ammonia is added to a solution of zinc nitrate. (d) Ethanoic acid (acetic acid) is added to a solution of barium hydroxide. (e) A small piece of potassium is added to water. (f) Powdered iron metal is strongly heated with powdered sulfur. (g) A solution of sodium fluoride is added to a solution of hydrochloric acid. (h) A strip of lead metal is added to a solution of silver nitrate. 2- 2+ → (a) CO3 + Sr SrCO3 → (b) C3H6 + O2 CO2 + H2O 2+ → 2+ (c) NH3 + Zn Zn(NH3)6 - → - (d) OH + HC2H3O2 C2H3O2 + H2O → - + (e) K + H2O OH + H2 + K (f) Fe + S → FeS (g) H+ + F- → HF (h) Pb + Ag+ → Pb2+ + Ag 2004 (a) A solution of copper(II) sulfate is spilled onto a sheet of freshly polished aluminum metal. (b) Dimethyl ether is burned in air. (c) A 0.1 M nitrous acid solution is added to the same volume of a 0.1 M sodium hydroxide solution. (d) Hydrogen iodide gas is bubbled into a solution of lithium carbonate. 2 (e) An acidic solution of potassium dichromate is added to a solution of iron(II) nitrate. (f) Excess concentrated aqueous ammonia is added to a solution of nickel(II) bromide. (g) A solution os sodium phosphate is added to a solution of aluminum nitrate. (h) Concentrated hydrochloric acid is added to a solution of sodium sulfide. (a) Cu2+ + Al → Cu + Al3+ → (b) C2H6O + O2 CO2 + H2O - → - (c) HNO2 + OH H2O + NO2 2- → - - - (d) HI + CO3 I + CO2 + H2O OR I + HCO3 2- 2+ + → 3+ 3+ (e) Cr2O7 + Fe + H Fe + Cr + H2O 2+ → 2+ (f) Ni + NH3 [Ni(NH3)6] 3- 3+ → (g) PO4 + Al AlPO4 + - → (h) H + HS H2S 2004 Form B (a) Cadmium metal is placed in a solution of tin(II) chloride. (b) Magnesium pellets are placed in 1.0 M hydrochloric acid. (c) Sulfur in its standard state is burned in air. (d) Solutions of silver nitrate and sodium chloride are combined. (e) Solid iron(II) sulfite is heated strongly. (f) Powdered barium oxide is mixed with water. (g) Excess saturated sodium fluoride solution is added to a solution of aluminum sulfate. (h) Solid potassium carbonate is added to 1.0 M sulfuric acid. (a) Cd + Sn2+ → Sn + Cd2+ + → 2+ (b) Mg + H Mg + H2 → → (c) S8 + O2 SO2 OR S + O2 SO2 (d) Ag+ + Cl- → AgCl → (e) FeSO3 FeO + SO2 → 2+ - (f) BaO + H2O Ba + OH - 3+ → 3- (g) F + Al [AlF6] + → + (h) K2CO3 + H CO2 + H2O + K 2003 (a) A solution of potassium phosphate is mixed with a solution of calcium acetate. (b) Solid zinc carbonate is added to 1.0 M sulfuric acid. (c) A solution of hydrogen peroxide is exposed to strong sunlight. (d) A 0.02 M hydrochloric acid solution is mixed with an equal volume of a 0.01 M calcium hydroxide solution. (e) Excess concentrated aqueous ammonia is added to solid silver chloride. (f) Magnesium ribbon is burned in oxygen. (g) A bar of strontium metal is immersed in a 1.0 M copper (II) nitrate solution. (h) Solid dinitrogen pentoxide is added to water. 3- 2+ → (a) PO4 + Ca Ca3(PO4)2 + - → 2+ 2- (b) ZnCO3 + H + HSO4 Zn + CO2 + H2O + SO4 OR, + → 2+ ZnCO3 + H Zn + CO2 + H2O → (c) H2O2 O2 + H2O - + → (d) OH + H H2O 3 → + - (e) AgCl + NH3 Ag(NH3)2 + Cl (f) Mg + O2 → MgO (g) Sr + Cu2+ → Sr2+ + Cu → + - (h) N2O5 + H2O H + NO3 2003 Form B (a) Hot hydrogen gas is passed over heated copper(II) oxide solid. (b) Solid sodium hydride id added to water. (c) Propoanone is burned in air. (d) A solution of lead(II) nitrate is added to a solution of potassium sulfate. (e) Ammonia gas is mixed with hydrogen chloride gas. (f) Sulfur trioxide gas is bubbled into water. (g) Excess concentrated potassium hydroxide solution is added to a solution of nickel(II) chloride. (h) Solid sodium acetate is added to 1.0 M hydrobromic acid. → (a) H2 + CuO Cu + H2O → + - (b) NaH + H2O Na + OH + H2 → (c) C3H6O + O2 CO2 + H2O 2+ 2- → (d) Pb + SO4 PbSO4 → (e) HCl + NH3 NH4Cl → + - (f) SO3 + H2O H + HSO4 - 2+ → 2- (g) OH + Ni Ni(OH)4 + → + (h) NaC2H3O2 + H HC2H3O2 + Na 2002 (a) A solution of sodium iodide is added to a solution of lead (II) acetate. (b) Pure solid phosphorus (white form) is burned in air. (c) Solid cesium oxide is added to water. (d) Excess concentrated hydrochloric acid is added to a 1.0 M solution of cobalt (II) chloride. (e) Solid sodium hydrogen carbonate (sodium bicarbonate) is strongly heated. (f) An excess of hydrochloric acid is added to solid zinc sulfide. (g) Acidified solutions of potassium permanganate and iron(II) nitrate are mixed together. (h) A solution of potassium hydroxide is added to solid ammonium chloride. - 2+ → (a) I + Pb PbI2 → (b) P4 + O2 P4O10 → + - (c) Cs2O + H2O Cs + OH - 2+ → 2- - 2+ → 2- (d) Cl + Co(H2O)6 H2O + CoCl4 OR Cl + Co H2O + CoCl4 → (e) NaHCO3 Na2CO3 + H2O + CO2 + → 2+ (f) H + ZnS Zn + H2S - + 2+ → 3+ 2+ (g) MnO4 + H + Fe H2O + Fe + Mn - → - (h) NH4Cl + OH NH3 + Cl + H2O 2002 Form B (a) A sample of 1-propanol is burned in air. (b) Solutions of sodium chromate and lead nitrate are mixed. (c) A bar of iron metal is added to a solution of iron(III) chloride. (d) Concentrated ammonia solution id added to copper(II) sulfate solution. (e) Sulfur dioxide gas is bubbled into a beaker of water.
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