1. Chemical Formulas Handout 2. Naming Ionic Compounds worksheet 3. Naming Chemical Compounds worksheet 4. Naming Covalent Compounds worksheet 5. Translating Equations into Sentences 6. Translating Sentences into Equations 7. Balancing Chemical Equations 8. Synthesis Reactions 9. Decomposition Reactions 10. Single-Replacement Reactions 11. Double-Replacement Reactions 12. Stoichiometry 13. Boyle's Law
Translating Equations into Sentences 1. NO2(g) + HNO3(l) → HNO3(aq) + NO(g) Nitrogen dioxide gas combines with liquid hydrogen nitrate to produce nitric acid and nitrogen dioxide gas. 2. KClO3(s) → HCl(s) + O2(g) Solid potassium chlorate decomposes into solid hydrogen chloride and oxygen gas. 3. Zn(s) + HCl(aq) → ZnCl2(aq) + H2(g) Solid zinc combines with hydrochloric acid to produce zinc chloride and hydrogen gas. 4. Al2(SO4)3(s) + Ca(OH)2(aq) → Al(OH)3(aq) + CaSO4 (aq) Solid aluminum sulfate combines with aqueous calcium hydroxide to form aqueous aluminum hydroxide and aqueous calcium sulfate. 5. Na(s) + Cl2(g) → NaCl(s) Solid sodium combines with chlorine gas to form solid sodium chloride.
Translating Sentences into Equations 1. Aqueous dihydrogen dioxide decomposes to produce oxygen and water. H2O2(aq) → O2(g) + H2O(l) 2. Solid zinc sulfide and oxygen yield solid zinc oxide and sulfur dioxide gas. ZnS(s) + O2(g) → ZnO(s) + SO2(g) 3. Aqueous hydrogen chloride and aqueous magnesium hydroxide react to produce aqueous magnesium chloride and water. HCl(aq) + Mg(OH)2(aq) → MgCl2(aq) + H2O(l) 4. Aqueous hydrogen nitrate and aqueous calcium hydroxide react to produce aqueous calcium nitrate and water. HNO3(aq) + Ca(OH)2(aq) → CaNO3(aq) + H2O(l) 5. Solid calcium hydroxide and liquid water react to produce aqueous calcium hydroxide and hydrogen gas. Ca(OH)2(s) + H2O(l) → Ca(OH)2(aq) + H2(g)
Balancing Chemical Equations 1. Solid calcium metal reacts with water to form aqueous calcium hydroxide and hydrogen gas. Ca(s) + 2H2O(ℓ) → Ca(OH)2(aq) + H2 (g) 2. Nitrogen dioxide gas reacts with water to form aqueous hydrogen nitrate (nitric acid) and nitrogen monoxide gas. 3NO2(g)+ H2O(ℓ) → 2HNO3(aq) + NO(g) 3. Solid potassium chlorate decomposes to form solid potassium chlorate and oxygen gas. 2KClO3 → 2KCl(s) + 3O2(g) 4. Solid zinc oxide is made by reacting solid zinc sulfide with oxygen gas. Sulfur dioxide gas is also produced. 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g) 5. Solid calcium phosphate is reacted with aqueous sulfuric acid (hydrogen sulfate) to form phosphoric acid (hydrogen phosphate) and solid calcium sulfate. Ca3(PO4)2 (s) + 3H2SO4(aq) → 2H3PO4(aq) + 3CaSO4(s) 6. Solid sodium combines with chlorine gas to produce solid sodium chloride. 2Na(s) + Cl2(g) → 2NaCl(s) 7. When solid copper reacts with aqueous silver nitrate the products are aqueous copper(II) nitrate and solid silver. Cu(s) + 2AgNO3 → Cu(NO3)2(aq) + 2Ag(s) 8. In a blast furnace, the reaction between solid iron(III) oxide and carbon monoxide gas produces solid iron and carbon dioxide gas. Fe2O3(s) +3CO(g)
2Fe(s) + 3CO2(g)
9. When solid lithium reacts with aqueous aluminum sulfate the products are aqueous lithium sulfate and solid aluminum. 6Li(s) + Al2(SO4)3(aq) → 3Li2SO4(aq) + 2Al(s) 10. Hydrogen sulfide gas and oxygen gas produce sulfur dioxide gas and water vapor. 2H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g)
Synthesis Reactions 1. calcium + oxygen → calcium oxide 2Ca + O2 → 2CaO 2. iron (III) + sulfur → iron(III) sulfide 16Fe + 3S8 → 8Fe2S3 3. hydrogen + oxygen → water 2H2 + O2 → 2H2O 4. aluminum + bromine → aluminum bromide 2Al + 3Br2 → 2AlBr3 5. sodium + iodine → sodium iodide 2Na + I2 → 2NaI 6. calcium oxide + water → calcium hydroxide CaO + H2O → Ca(OH)2 7. chromium(III) + oxygen → chromium (III) oxide 4Cr + 3O2 → 2Cr2O3 8. silver + sulfur → silver sulfide 16Ag + S8 → 8Ag2S 9. magnesium + oxygen → magnesium oxide 2Mg + O2 → 2MgO 10. sodium + oxygen → sodium oxide 4Na +O2 → 2Na2O
Decomposition Reactions 1. Iron(III) oxide → iron(III) + oxygen Fe3O2 → 3Fe + O2 2. Barium hydroxide → barium oxide + water Ba(OH)2 → BaO + H2O 3. Magnesium chlorate → magnesium chloride + oxygen Mg(ClO3)2 → MgCl2 + 3O2 4. Potassium carbonate → potassium oxide + carbon dioxide K2CO3 → K2O + CO2 5. Magnesium hydroxide → magnesium oxide + water Mg(OH)2 → MgO + H2O 6. Silver chloride → silver + chlorine 7. strontium chlorate → strontium chloride + oxygen Sr(ClO3)2 → SrCl2 + 3O2 8. Magnesium carbonate → magnesium oxide + carbon dioxide MgCO3 → MgO + CO2 9. Aluminum chlorate → aluminum chloride + oxygen 2Al(ClO3)3 → 2AlCl3 + 9O2 10. beryllium hydroxide → beryllium oxide + water Be(OH)2 → BeO + H2O
Singe-Replacement Reactions 1. silver nitrate + nickel(II) → nickel(II) nitrate + silver 2AgNO3 + Ni → Ni(NO3)2 + 2Ag 2. aluminum bromide + chlorine → aluminum chloride + bromine 2AlBr3 + 3Cl2 → 2AlCl3 + 3Br3 3. Sodium iodide + bromine → sodium bromide + iodine 2NaI + Br2 → 2NaBr + I2 4. Calcium + hydrochloric acid → hydrogen + calcium chloride Ca + 2HCl → CaCl2 + H2 5. Magnesium + nitric acid → magnesium nitrate + hydrogen Mg + 2HNO3 → Mg(NO3)2 + H2 6. Potassium + water → potassium hydroxide + hydrogen 2K + 2H2O → 2KOH + H2 7. Zinc + magnesium chloride → no reaction Zn + MgCl2 → no reaction 8. Aluminum + water → aluminum oxide + hydrogen 2Al + 3H2O → Al2O3 + 3H2 9. Potassium iodide + bromine → potassium bromide + iodine 2KI + Br2 → 2KBr + I2 10. Magnesium + cobalt(II) nitrate → cobalt(II) + magnesium nitrate Mg + Co(NO3)2 → Co + Mg(NO3)2
Double-Replacement Reactions 1. Silver nitrate + hydrochloric acid → silver chloride + nitric acid AgNO3 + HCl → HNO3 + AgCl 2. Copper(II) chloride + sodium sulfide → copper(II) sulfide + sodium chloride CuCl2 + Na2S → CuS + 2NaCl 3. Iron(II) sulfide + hydrochloric acid → iron(II) chloride + hydrogen sulfide FeS + 2HCl → FeCl2 + H2S 4. Sulfuric acid + potassium hydroxide → potassium sulfate + water H2SO4 + 2KOH → K2SO4 + 2H2O 5. Nitric acid + calcium hydroxide → calcium nitrate + water 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O 6. Lithium hydroxide + iron(III) nitrate → lithium nitrate + iron(III) hydroxide 3LiOH + Fe(NO3)3 → 3LiNO3 + Fe(OH)3 7. Lead(II) acetate + hydrogen sulfide → lead sulfide + hydrogen acetate Pb(CH3COO)2 + H2S → PbS +2HCH3COO 8. Aluminum iodide + mercury(II) chloride → aluminum chloride + mercury(II) iodide 2AlI3 + 3HgCl2 → 2AlCl3 + 3HgI2 9. Calcium acetate + sodium carbonate → calcium carbonate + sodium acetate Ca(CH3COO)2 + Na2CO3 → CaCO3 + 2NaCH3COO 10. ammonium chloride + mercury(I) acetate → ammonium acetate + mercury(I) chloride NH4Cl + HgCH3COO → NH4CH3COO + HgCl
Stoichiometry Problem Type 1: mol→mol 1. N2 + 3H2 → 2NH3 Analyze: Given: 6 mol H2 Unknown: mol NH3 Plan: mol H2 → mol NH3 mol H2 x mol NH3 = mol NH3 mol H2 Compute: 6 mol H2 x 2 mol NH3 = 4 mol NH3 3 mol H2 Evaluate: Significant figures: correct Units: correct Reasonable: The answer is two-thirds of six. 2. 2KClO3 → 2KCl + 3O2 Analyze: Given: 15 mol O2 Unknown: mol KClO3 Plan: mol O2 → mol KClO3 mol O2 x mol KClO3 = mol KClO3 mol O2 Compute: 15 mol O2 x 2 mol KClO3 = 10 mol KClO3 3 mol O2 Evaluate: Significant figures: correct Units: correct Reasonable: The answer is two-thirds of fifteen. 3. 2H2 + O2 → 2H2O Analyze: Given: 5.0 mol H2O Unknown: mol O2 Plan: mol H2O → mol O2 mol H2O x mol O2 = mol O2 mol H2O Compute: 5.0 mol H2O x 1 mol O2 = 2.5 mol O2 2 mol H2O
Evaluate: Significant figures: correct Units: correct Reasonable: The answer is half of five. 4. 4NH3 + 3O2 → 2N2 + 6H2O Analyze: Given: 4 mol N2 Unknown: mol NH3 Plan: mol N2 → mol NH3 mol N2 x mol NH3 = mol NH3 mol N2 Compute: 4 mol N2 x 4 mol NH3 = 8 mol NH3 2 mol N2 Evaluate: Significant figures: correct Units: correct Reasonable: The answer is the double of four. 5. Mg + 2HCl → MgCl2 + H2 Analyze: Given: 2.50 mol MgCl2 Unknown: mol HCl Plan: mol MgCl2 → mol HCl mol MgCl2 x mol HCl = mol HCl mol MgCl2 Compute: 2.50 mol MgCl2 x 2 mol HCl = 5.00 mol HCl 1 mol MgCl2 Evaluate: Significant figures: correct Units: correct Reasonable: The answer is twice two and a half. Problem Type 2: mol → mass 1. 6CO2 + 6H2O → C6H12O6 + 6O2 Analyze: Given: 3.00 mol H2O Unknown: mass(g) C6H12O6 Plan: mol H2O→ g C6H12O6 mol H2O x mol C6H12O6 x g C6H12O6 = g C6H12O6 mol H2O mol C6H12O6 Compute: 3.00 mol H2O x 1 mol C6H12O6 x 180.18 g C6H12O6 ≈ 90.1 g C6H12O6 6 mol H2O 1 mol C6H12O6
Evaluate: Significant figures: correct Units: correct Reasonable: The answer is about one-half of the molar mass of glucose. 2. 2NaN3 → 2Na + 3N2 Analyze: Given: .500 mol NaN3 Unknown: mass(g) N2 Plan: mol NaN3→ g N2 mol NaN3 x mol N2 x g N2 = g N2 mol NaN3 mol N2 Compute: .500 mol NaN3 x 3 mol N2 x 28.02 g N2 ≈ 21.0 g N2 2 mol NaN3 1 mol N2 Evaluate: Significant figures: correct Units: correct Reasonable: The answer is about three-fourths the mass of dinitrogen. 3. 2Mg + O2 → 2MgO Analyze: Given: 2.00 mol O2 Unknown: mass(g) MgO Plan: mol O2 → g MgO mol O2 x mol MgO x g MgO = g MgO mol O2 mol MgO Compute: 2.00 mol O2 x 2 mol MgO x 40.31 g MgO ≈ 161 g MgO 1 mol O2 1 mol MgO Evaluate: Significant figures: correct Units: correct Reasonable: The answer is about four times the molar mass of magnesium oxide. 4. SiO2 + 3C → SiC + 2CO Analyze: Given: 2.00 mol C Unknown: mass(g) SiC Plan: mol C→ g SiC mol C x mol SiC x g SiC = g SiC mol C mol SiC Compute: 2.00 mol C x 1 mol SiC x 40.1 g SiC ≈ 26.7 g SiC 3 mol C 1 mol SiC
Evaluate: Significant figures: correct Units: correct Reasonable: The answer is about two-thirds the mass of silicon carbide. 5. 2ZnO + C → 2Zn + CO2 Analyze: Given: 5.00 mol C Unknown: mass(g) ZnO Plan: mol C→ g ZnO mol C x mol ZnO x g ZnO = g ZnO mol C mol ZnO Compute: 5.00 mol C x 2 mol ZnO x 81.39 g ZnO ≈ 813.9 g ZnO 1 mol C 1 mol ZnO Evaluate: Significant figures: correct Units: correct Reasonable: The answer is ten times the mass of zinc oxide. Problem Type 3: mass → mol 1. 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) Analyze: Given: 824 g NH3 Unknown: mol NO Plan: g NH3 → mol NO g NH3 x mol NH3 x mol NO = mol NO g NH3 mol NH3 Compute: 824 g NH3 x 1 mol NH3 x 4 mol NO ≈ 48.4 mol NO 17.04 g NH3 4 mol NH3 Evaluate: Significant figures: correct Units: correct Reasonable: The answer is more than twenty times the molar mass, so this large answer makes sense. 2. 2H2O + 2NaCl Cl2 + 2NaOH + H2 Analyze: Given: 250. g NaCl Unknown: mol Cl2 Plan: g NaCl → mol Cl2 g NaCl x mol NaCl x mol Cl2 = mol Cl2 g NaCl mol NaCl
Compute: 250. g NaCl x 1 mol NaCl x 1 mol Cl2 ≈ 2.14 mol Cl2 58.44 g NaCl 2 mol NaCl Evaluate: Significant figures: correct Units: correct Reasonable: There are about five moles of sodium chloride. The answer is about half of that so it is reasonable. 3. Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g) Analyze: Given: 4000 g Fe2O3 Unknown: mol CO Plan: g Fe2O3 → mol CO g Fe2O3 x mol Fe2O3 x mol CO = mol CO g Fe2O3 mol Fe2O3 Compute: 4000 g Fe2O3 x 1 mol Fe2O3 x 3 mol CO ≈ 75.1 mol CO 159.7 g Fe2O3 1 mol Fe2O3 Evaluate: Significant figures: correct Units: correct Reasonable: There are about twenty moles of iron(III) oxide present and then three times that would be the answer. 4. H2SO4 + 2NaHCO3 → 2CO2 + Na2SO4 + 2H2O Analyze: Given: 150.0 g H2SO4 Unknown: mol NaHCO3 Plan: g H2SO4 → mol NaHCO3 g H2SO4 x mol H2SO4 x mol NaHCO3 = mol NaHCO3 g H2SO4 mol H2SO4 Compute: 150.0 g H2SO4 x 1 mol H2SO4 x 2 mol NaHCO3 ≈ 3.058 mol NaHCO3 98.09 g H2SO4 1 mol H2SO4 Evaluate: Significant figures: correct Units: correct Reasonable: There are a little less than two mole of sulfuric acid present, so that doubled would be a little less than four. Therefore this answer is reasonable. 5. Fe2O3 + 2Al → 2Fe + Al2O3 Analyze: Given: 99.0 g Al Unknown: mol Fe2O3 Plan: g Al → mol Fe2O3 g Al x mol Al x mol Fe2O3 = mol Fe2O3 g Al mol Al
Compute: 99.0 g Al x 1 mol Al x 1 mol Fe2O3 ≈ 1.83 mol Fe2O3 26.98 g Al 2 mol Al Evaluate: Significant figures: correct Units: correct Reasonable: There are a little less than four moles of aluminum. That halved would be less than two so the answer is reasonable. Problem Type 4: mass → mass 1. Sn(s) + 2HF(g) → SnF2(s) + H2 Analyze: Given: 30.00 g HF Unknown: g SnF2 Plan: g HF → g SnF2 g HF x mol HF x mol SnF2 x g SnF2= g SnF2 g HF mol HF mol SnF2 Compute: 30.00 g HF x 1 mol HF x 1 mol SnF2 x 156 g SnF2 ≈ 116.94 g SnF2 20.01 g HF 2 mol HF 1 mol SnF2 Evaluate: Significant figures: correct Units: correct 2. 2Na2O2 + 2H2O → 4NaOH + O2 Analyze: Given: 50.0 g Na2O2 Unknown: g O2 Plan: g Na2O2 → g O2 g Na2O2 x mol Na2O2 x mol O2 = mol SnF2 g Na2O2 mol Na2O2 Compute: 50.0 g Na2O2 x 1 mol Na2O2 x 1 mol O2 x 32 g O2 ≈ 116.94 g SnF2 77.98 g Na2O2 2 mol Na2O2 1 mol O2 Evaluate: Significant figures: correct Units: correct 3. H3PO4 + 2NH3 → (NH4)2HPO4 Analyze: Given: 2800000 g H3PO4 Unknown: g NH3 Plan: g H3PO4 → g NH3 g H3PO4 x mol H3PO4 x mol NH3 x g NH3 = mol NH3 g H3PO4 mol H3PO4 mol NH3
Compute: 2800000 g H3PO4 x 1 mol H3PO4 x 2 mol NH3 x 17.04 g NH3 ≈ 970000 g NH3 98 g H3PO4 1 mol H3PO4 1 mol NH3 Evaluate: Significant figures: correct Units: correct 4. 2NH4NO3 → 2N2 + O2 + 4H2O Analyze: Given: 36.0 g NH4NO3 Unknown: g N2 Plan: g NH4NO3 → g N2 g NH4NO3 x mol NH4NO3 g NH4NO3
x mol N2 x g N2 = g N2 mol NH4NO3 mol N2
Compute: 36.0 g NH4NO3 x 1 mol NH4NO3 x 2 mol N2 x 28.02 g N2 ≈ 12.6 g N2 80.06 g NH4NO3 2 mol NH4NO3 1 mol N2 Evaluate: Significant figures: correct Units: correct 5. 2H2O(l) + O2(g) + 2SO2(g) → 2H2SO4(aq) Analyze: Given: 50.0 g SO2 Unknown: g H2SO4 Plan: g SO2 → g H2SO4 g SO2 x mol SO2 x mol H2SO4 x g H2SO4= g H2SO4 g SO2 mol SO2 mol H2SO4 Compute: 50.0 g SO2 x 1 mol SO2 x 2 mol H2SO4 x 98.09 g H2SO4 ≈ 76.5 g H2SO4 64.07 g SO2 2 mol SO2 1 mol H2SO4 Evaluate: Significant figures: correct Units: correct
Boyle's Law 1. Analyze Given: P1= 700. torr V1= 200. mL P2= 350. torr Unknown: V2 Plan V1 = V2 P1 P2 Compute 200 mL = V2 700. torr 350 torr V2 = 100. mL Evaluate significant figures: correct units: correct reasonable: the pressure is doubled, so the volume is halved. 2. Analyze Given: P1= 0.48 atm V1= 435 mL P2= 0.75 atm Unknown: V2 Plan V1 = V2 P1 P2 Compute 435 mL = V2 0.48 torr 0.75 torr V2 = 278 mL Evaluate significant figures: correct units: correct reasonable: the pressure is almost doubled, so the volume is almost halved. 3. Analyze Given: P2= 180 mmHg V1= 2.4 x 105 mL V2= 1.8 x 103 mL
Unknown: P1 Plan V1 = V2 P1 P2 Compute 2.4 x 105 mL = P1
1.8 x 103 mL 180 mmHg
P1 = 1.35 mmHg Evaluate significant figures: correct units: correct reasonable: the volume is decreased very greatly, so the pressure is increased very greatly 4. Analyze Given: P1= 0.428 atm V1= 240. mL P2= 0.724 atm Unknown: V2 Plan V1 = V2 P1 P2 Compute 240. mL = V2 0.724 atm 0.428 atm V2 = 405 mL Evaluate significant figures: correct units: correct reasonable: the pressure is almost halved, so the volume is almost doubled. 5. Analyze Given: P1= 0.960 atm V1= 200.0 mL V2= 50.0 mL Unknown: P2 Plan V1 = V2 P1 P2 Compute
200.0 mL = 0.960 atm
50.0 mL P2
V2 = 3.84 atm Evaluate significant figures: correct units: correct reasonable: the volume is divide by four so the pressure must be multiplied by four.