[chem] Workshop_types Of Chemical Rxn

Types of Chemical Reactions (Homework Answer Key) Workshop on Combustion Reactions Write the formulas to show the reactants and products for the following laboratory situations described below. Assume that solutions are aqueous unless otherwise indicated. 1. A piece of solid bismuth is heated strongly in oxygen. 4Bi(s) + 3O2(g)  2BiO3(s) 2. Butanol (CH3CH2CH2CH2OH) is burned in air. C4H10O(aq) + 6O2(g)  4CO2(g) + 5H2O(g) 3. Solid copper(II) sulfide is heated strongly in oxygen gas. 2CuS(s) + 3O2(g)  2CuO(s) +2SO2(g) 4. Hexane is burned in excess oxygen. 2C6H14(aq) + 19O2(g)  12CO2(g) + 14H2O(g) 5. Sodium metal is burned in excess oxygen gas. Na(s) + O2(g) 2NaO(s) 6. Gaseous silane, SiH4, is burned in oxygen. SiH4(g) + 2O2(g)  SiO2(g) + 2H2O(g) 7. Solid zinc sulfide is heated in an excess of oxygen. 2ZnS(s) + 3O2(g)  2ZnO(s) + 2SO2(g) Workshop on Synthesis and Decomposition Reactions Write the formulas to show the reactants and products for the following laboratory situations described below. Assume that solutions are aqueous unless otherwise indicated. 1. A sample of calcium carbonate is heated. CaCO3 + heat  CaO(s) + CO2(g) 2. Sulfur dioxide gas is bubbled through water. SO2(g) + H2O(l)  H2SO3(aq) 3. Solid potassium oxide is added to a container of carbon dioxide gas. K2O(S) + CO2(g) K2CO3 4. Liquid hydrogen peroxide is warmed. 2H2O2(l) + heat  2H2O(l) + O2(g) 5. A pea-sized piece of sodium is added to a container of iodine vapor. 2Na(s) + I2(g)  NaI(s) 6. A sample of carbonic acid is heated. H2CO3(aq) + heat  H2O(l) + CO2(g) 7. A sample of potassium chlorate is heated. 2KClO3(aq) +heat  2KCl(aq) + 3O2(g) 8. Solid magnesium oxide is added to sulfur trioxide gas. MgO(s) + SO3(g)  Mg2SO4(s) Workshop on Single Replacement/Displacement Reactions

Write the formulas to show the reactants and products for the following laboratory situations described below. Assume that solutions are aqueous unless otherwise indicated. Write NR if no reaction occurs. 1. Liquid bromine is added to sodium iodide crystals. Br2(l) + 2NaI(s)  I2(g) + 2NaBr(aq) 2. An aluminum strip is immersed in a solution of silver nitrate. Al(s) + 3AgNO3(aq)  3Ag(s) + Al(NO3)3(aq) 3. Zinc pellets are added to sulfuric acid (H2SO4). Zn(s) + H2SO4(aq)  ZnSO4(aq) + H2(g) 4. Fluorine gas is bubbled into a solution of aluminum chloride. 3F2(g) + AlCl3(aq)  2AlF3(aq) + 3Cl2(g) 5. Calcium metal is added to nitrous acid (HNO2). Ca(s) + 2HNO2(aq)  Ca(NO2)2(aq) + H2(g) 6. A pea-sized piece of lithium is added to water. Li(s) + 2H2O(l)  Li(OH)2(aq) + 2H2(g) 7. Magnesium turnings are added to a solution of lead(II) acetate. Mg(s) + Pb(CH3COO)2(aq)  Mg(CH3COO)2(aq) + Pb(s) 8. Liquid bromine is reacted with a solution of calcium chloride. Br2(l) + CaCl2(aq)  NR Workshop on Double Displacement Reactions Write the formulas to show the reactants and products for the following laboratory situations described below. Assume that solutions are aqueous unless otherwise indicated. Write NR if no reaction occurs. 1. Silver nitrate combines with potassium chromate. AgNO3(aq) + K2CrO4(aq)  Ag2CrO4(s) + KNO3(aq) 2. Ammonium chloride combines with cobalt(II) sulfate. NH4Cl(aq) + CoSO4(aq) NR 3. Lithium hydroxide reacts with sodium chromate. Li(OH)2(aq) + Na2CrO4(aq)  LiCrO4(s) + NaOH(aq) 4. Zinc acetate is mixed with cesium hydroxide. Zn(CH3COO)2(aq) + CsOH(aq)  Zn(OH)2(s) + CsCH3COO 5. Ammonium sulfide reacts with lead(II) nitrate. (NH4)2S(aq) + PbNO3(aq)  NH4NO3(aq) + PbS(s) 6. Iron(III) sulfate combines with barium iodide. FeSO4(aq) + BaI2(aq)  FeI2(aq) + BaSO4(s) 7. Chromium(III) bromide reacts with sodium nitrate. CrBr3(aq) + NaNO3(aq)  NR 8. Rubidium phosphate mixes with titanium(IV) nitrate. Rb3PO4(aq) + Ti(NO3)4(aq)  RbNO3(aq) + Ti3(PO4)4(s) 9. Ammonium carbonate combines with nickel(II) chloride. (NH4)2CO3(aq) + NiCl2(aq)  NH3Cl(aq) + NiCO3(s) 10. Tin(IV) nitrate reacts with potassium sulfite. Sn(NO3)4(aq) + K2SO3(aq)  Sn(SO2)2(aq) + KNO3(aq)

Workshop on Gas Formation Reactions (Double Displacement Reaction) Write the formulas to show the reactants and products for the following laboratory situations described below. Assume that solutions are aqueous unless otherwise indicated. Write NR if no reaction occurs. 1. Ammonium sulfate & potassium hydroxide are mixed. (NH4)2SO4(aq) + 2KOH(aq)  2NH3(g) + K2SO4(aq) +2H2O(l) 2. Ammonium sulfide reacts with hydrochloric acid. (NH4)2S(aq) + 2HCl(aq)  H2S(g) + 2NH4Cl(aq) 3. Cobalt(II) chloride combines with silver nitrate. (Excluded) 4. Solid calcium carbonate reacts with sulfuric acid. CaCO3(s) +H2SO4(aq)  CO2(g) + H2O(l) + CaSO4(aq) 5. Potassium sulfite reacts with hydrobromic acid. K2SO3(aq) + 2HBr(aq)  2KBr(aq)+ SO2(g) + H2O(l) 6. Potassium sulfide reacts with nitric acid. K2S(aq) + 2HNO3(aq) H2S(g) + 2KNO3(aq) 7. Ammonium iodide mixes with magnesium sulfate. (Excluded) 8. Solid titanium(IV) carbonate reacts with hydrochloric acid. Ti(CO3)2(aq) + 4HCl(aq)  2CO2(g) + 2H2O(l) + TiCl4(aq) 9. Solid calcium sulfite is mixed with acetic acid. CaS(s) + 2HCH3COO(aq)  H2S(g) + Ca(CH3COO)2(aq) 10. Strontium hydroxide combines with ammonium sulfide. Sr(OH)2(aq) + (NH4)2S(aq)  2NH3(g) + 2H2O(l) + SrS(aq)