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Chemistry Review Packet Name: Molar Mass 1. CaCl2 2. HNO3 3. C8H10N4O2 4. Al2(SO4)3 5. Zn (NO3)2 Formula Writing 6. sodium phosphate 7. ammonium carbonate 8. aluminum chromate 9. calcium hydroxide 10. iron (II) fluoride Period: Date: Equation Writing and Balancing 11. Magnesium chloride is the product of a reaction between magnesium and chlorine. 12. Copper (II) hydroxide and potassium sulfate are produced when potassium hydroxide reacts with copper (II) sulfate. 13. Aluminum nitrate + sodium hydroxide -----> aluminum hydroxide + sodium nitrate 14. Iron (III) oxide + carbon monoxide -----> iron + carbon dioxide 15. Hydrogen chloride reacts with potassium hydroxide to produce water and potassium chloride. Mole Conversions 16. 12.4 moles of CO2 = ? grams 17. 3.7 moles of MgCl2 = ? grams 18. 14 grams of PbO = ? moles 19. 19 grams of HCl = ? moles 20. 22 moles of NH4C2H3O2 = ? grams Stoichiometry **YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.** BALANCE THE FOLLOWING EQUATIONS TO USE IN QUESTIONS 5 – 14: 1. ____ Al + ____ O2 → ____ Al2O3 2. ____ Cu + ____ AgNO3 → ____ Ag + ____ Cu(NO3)2 3. ____ Zn + ____ HCl → ____ ZnCl2 + ____ H2 4. ____ Fe + ____ Cl2 → ____ FeCl3 PERFORM THE FOLLOWING STOICHIOMETRIC CALCULATIONS: 5. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen. How many moles of HCl are required to produce 7.50 moles of ZnCl2? 6. Copper metal reacts with silver nitrate to form silver and copper(II) nitrate. How many grams of copper are required to form 250 g of silver? 7. When aluminum is burned in excess oxygen, aluminum oxide is produced. How many grams of oxygen are required to produce 0.75 moles of Al2O3? 8. How many grams of iron(III) chloride are produced when 15.3 g of iron react with excess chlorine gas? 9. Copper metal reacts with silver nitrate to form silver and copper(II) nitrate. How many moles of silver will be produced from 3.65 moles of silver nitrate? 10. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas. How many milliters of 3.00M HCl are required to react with 12.35 g of zinc? 11. How many grams of iron are needed to react with 31.0 L of chlorine gas at STP to produce iron(III) chloride? 12. When 9.34 g of zinc react with excess hydrochloric acid how many grams of zinc chloride will be produced? 13. How many liters of oxygen gas at STP are required to react with 65.3 g of aluminum in the production of aluminum oxide? 14. Copper reacts with silver nitrate to form silver and copper(II) nitrate. How many grams of copper are required to react with 50.0 mL of 8.0M AgNO3? 15. Nickel nitrate and potassium carbonate react to form nickel carbonate and potassium nitrate. How many milliliters of 0.55M Ni(NO3)2 are needed to react with 85 mL of 0.25M K2CO3? First, write a balanced equation. 16. Zinc metal reacts with chromium(III) nitrate in a single replacement reaction. How many grams of zinc are required to react with 425 mL of 0.25M Cr(NO3)3? First, write a balanced equation. PERFORM THE FOLLOWING LIMITING REACTANT PROBLEMS: 17. When 16.3 g of magnesium and 4.52 g of oxygen gas react, how many grams of magnesium oxide will be formed? Identify the limiting and excess reactants. 2 Mg + O2 → 2 MgO 18. If 25.3 g of aluminum reacts with 25.3 g of copper(II) sulfate, how many grams of copper are formed? Identify the limiting and excess reactants in this single replacement reaction. 2 Al + 3 CuSO4 → 3 Cu + Al2(SO4)3 19. Identify the limiting and excess reactants when 1.00 g of zinc reacts with 150 mL of 0.250M Pb(NO3)2. How many grams of lead are formed in this single replacement reaction? Zn + Pb(NO3)2 → Pb + Zn(NO3)2 20. If 24.5 g of iron are placed in 1.00 L of 0.25M HCl, how many grams of FeCl2 are obtained? Identify the limiting and excess reactants in this single replacement reaction. Fe + 2 HCl → FeCl2 + H2 PERFORM THE FOLLOWING PERCENT YIELD CALCULATIONS: 21. If 12.5 g of copper react with excess chlorine gas, then 25.4 g of copper(II) chloride are produced. Find the theoretical and percent yields. Cu + Cl2 → CuCl2 22. If 6.57 g of iron react with an excess of hydrochloric acid, HCl, then 11.2 g of iron(II) chloride are obtained in addition to hydrogen gas. Find the theoretical and percent yields. Fe + 2 HCl → FeCl2 + H2 23. If 5.45 g of potassium chlorate are decomposed to form potassium chloride, 1.75 g of oxygen gas are also given off. Find the theoretical and percent yields. 2 KClO3 → 2 KCl + 3O2 Name ----------------- Date _ Class _ 11-2 Practice Problems 1. Determine the mass of lithium hydroxide produced when 0.38 g of lithium nitride reacts with water according to the following equation: Li3N + 3H20 -+ NH3 + 3LiOH 7. Determine the mass of sodium nitrate produced when 0.73 g of nickel(II) nitrate reacts with sodium hydroxide according to the following equation: Ni(N03)2 + 2NaOH -+ Ni(OH)2 + 2NaN03 2. What mass of sodium chloride is produced when chlorine reacts with 0.29 g of sodium iodide? 8. Determine the mass of calcium hydroxide produced when calcium carbide reacts with 0.64 g of water according to the following equation: CaC2 + 2H20 ---> Ca(OH)2 + C 2H 2 3. Determine the mass of carbon dioxide produced when 0.85 g of butane reacts with oxygen according to the following equation: 2C4H lO + 1302 -+ 8C02 + 10H20 9. How many grams of ozone (03) must decompose to produce 0.87 g of oxygen? 4. Determine the mass of antimony produced when 0.46 g of antimony(III) oxide reacts with carbon according to the following equation: 5b20 3 + 3C ---> 25b + 3CO 10. Find the mass of sugar (C6H 120 6) required to produce 1.82 L of carbon dioxide gas at 5TP from the reaction described by the following equation: C 6H 120 6 -+ 2C2H 60 + 2C02 5. What mass of hydrogen peroxide (H 20 2) must decompose to produce 0.77 g of water? 11. How many liters of oxygen are necessary for the combustion of 425 g of sulfur, assuming that the reaction occurs at 5TP? The balanced equation is 5 + 02 ---> 502' 6. What mass of carbon monoxide must react with oxygen to produce 0.69 g of carbon dioxide? 12. Find the mass of benzene (C6H 6) required to produce 2.66 L of carbon dioxide gas at 5TP from the reaction described by the following equation: 2C6H 6 + 1502 -+ 6H20 + 12C02 © Prentice-Hall, Inc. Chapter 11 13 !\Jame - - - - - - - - - - - - - - - - - Date _ Class _ 11-2 Practice Problems (continued) 13. Find the mass of sodium required to produce 5.68 L of hydrogen gas at STP from the reaction described by the following equation: 2Na + 2H 20 ---+ 2NaOH + H 2 14. How many liters of oxygen are necessary for the combustion of 277 g of carbon monoxide, assuming that the reaction occurs at STP? The balanced equation is 2CO + 02 ---+ 2C02 20. What volumes of H 2S gas and oxygen are necessary to produce 14.2 L of sulfur dioxide gas? The balanced equation is 2H2S + 302 ---+ 2S02 + 2H20 21. What volumes of sulfur dioxide and dihydrogen sulfide gases are necessary to produce 11.4 L of water vapor? The balanced equation is S02 + 2H2S ---+ 3S + 2H20 15. How many liters of oxygen are necessary for the combustion of 134 g of magnesium, assuming that the reaction occurs at STP? The balanced equation is 2Mg + 02 ---+ 2MgO 16. Find the mass of aluminum required to produce 4.72 L of hydrogen gas at STP from the reaction described by the following equation: 2Al + 3H2S04 ---+ AliSO4)3 + 3H2 17. How many liters of hydrogen are produced if 225 g of iron reacts with hydrochloric acid, assuming that the reaction occurs at STP? The balanced equation is Fe + 2HCl ---+ FeCl2 + H 2 22. Glucose (C 6H 12 0 6 ) burns in oxygen to produce carbon dioxide and water vapor as described in the following equation: C 6H 120 6 + 602 ---+ 6H20 + 6C02. What volume of carbon dioxide is produced when 3.7 L of oxygen are consumed? 23. The compound TNT (trinitrotoluene) decomposes explosively into carbon, carbon monoxide, hydrogen, and nitrogen. What volumes of hydrogen and nitrogen are produced if 5.8 L of CO is produced? The balanced equation is 2C 7H s(N0 2)3 ---+ 2C + 12CO + 5H2 + 3N2 24. Nitroglycerin decomposes explosively to 18. Find the mass of S8 required to produce 2.47 L of sulfur dioxide gas at STP from the reaction described by the following equation: produce carbon dioxide, water, nitrogen, and oxygen. What volumes of nitrogen and oxygen are produced if 4.3 L of carbon dioxide is produced? The balanced equation is 4C3H s(N03 )3 -> 12C02 + 10H20 + 02 + 6N2 19. Propane (C 3H 8) burns in oxygen to produce carbon dioxide and water vapor. The balanced equation for this reaction is C3 H g + 502 ---+ 4H 20 + 3C02· What volume of carbon dioxide is produced when 2.8 L of oxygen are consumed? 14 Chapter 11 25. Acetylene (C 2H 2) burns in oxygen to produce carbon dioxide and water. The balanced equation for this reaction is 2C2H 2 + 502 ---+ 2H20 + 4C02" What volume of carbon dioxide is produced when 1.6 L of oxygen are consumed? © Prentice-Hall, Inc.