ࡱ> [ &bjbj<< 6^\^\> > rrrr4Dr׃BQ$Q$Q$$ψ4]Q$"Q$Q$Q$4I6I6I6Q$2 I6Q$I6I6.zHTn@$, /2|@0׃}Te4ennexQ$Q$I6Q$Q$Q$Q$Q$445Q$Q$Q$׃Q$Q$Q$Q$eQ$Q$Q$Q$Q$Q$Q$Q$Q$> > |: Reactions/Equations Name: Goal: Students gain an understanding of chemical formulas, solutions, molecular formulas, and balanced equations and reactions. Objectives: Demonstrate knowledge of the mole concept/stoichiometry. Upon completion of the reading and problems, and when asked to demonstrate their understanding either orally or on a written test, students will: 1. Define or identify the following: chemical equation coefficient double replacement single replacement decomposition products reactants synthesis activity series limiting reagent percent yield 2. Write chemical equations 3. Balance chemical equations 4. Identify types of chemical equations Day 55 Thursday, November 14, 2013 What is an equation? What has to be true? Intro to equations Formula equations Balancing equations (wkst 2) Balancing Equations Trial and Error vs. Algebraically Follow The Yellow Brick Road (A) cw/hw: worksheets 1 & 2 ChemThink Chemical Reactions Tutorial (11/17/13) ChemThink Chemical Reactions Questions (due 11/18/13) Day56 Friday, November 15, 2013 What are the types of reactions? Test on Atomic Stoichiometry Word Equations (wkst 3) cw/hw - balancing (wkst 4) Classification of chemical reactions (wkst 5) if you made below a C (less than 52/67) on the last polyatomic ion quiz write the each ions 5x Worksheets 1-5 due Monday Day57, Monday, November 18, 2013 What are the products of combustion reactions? Quiz Polyatomic Ions Race - Balancing Chemical Equations Synthesis Decomposition Combustion cw/hw Synthesis and Decomposition worksheet 6 combustion worksheet 7 ChemThink Chemical Reactions Questions due 11/18/13 Day58, Tuesday, November 19, 2013 Why is an activity series needed for single replacement reactions? 1. Go over homework 2. Single replacement/displacement 3. Activity series 4. double replacement/displacement (wkst 9) 5. cw/hw: Single Replacement (wkst 8) worksheet 4 and 10 (identify the type of reaction for worksheet 4 complete worksheet 10) Pre-LAB - TYPES OF CHEMICAL REACTIONS (B) Day 59, Wednesday, November 20, 2013 What is the activity series? Go over homework Predicting products of chemical reactions (wkst 11) Lab activity (no contacts) Types of Chemical Reactions (B) cw/hw: Complete types of reactions lab Predicting equations worksheet 12 Day60, Thursday, November 21, 2013 Why are pre-labs required? What is a copper cycle? Go over homework Writing Complete Equations Practice cw/hw: Study for test Complete labs including conclusions That Useful Ratio Pre-Lab required (C) Day 61, Friday, November 22, 2013 What is the useful ratio? begin stoichiometry - Mol - Mol conversions Lab- That Useful Ratio Pre-Lab required(C) cw/hw Mole Mole worksheet 13 Day 62 Monday, November 25, 2013 Compare and contrast atomic stoichiometry to rxn stoichiometry. 1. Go over homework 2. stoichiometry - Mol - Mass conversions - Mass - Mol conversions - Mass - Mass conversions -Vol - Vol conversions 3. cw/hw Wks 14- 16(Mixed Mol; Vol - Vol; Mass-Mass) Day 63 Tuesday, November 26, 2013 What is a limiting reagent? Check homework Limiting Reagent Labs- Bicarbonate Dilemma (D) Pre-Lab required hw Worksheet 17 Limiting Reagent Day 64 Monday, December 2, 2013 How do you calculate percent yield? 1. Go over homework 2. Limiting Reagent 3. percent yield 4. hw worksheet 18 Limiting Reagent and Percent Yield Day 65 Tuesday, December 3, 2012 How do I prepare to demonstrate my knowledge of reaction stoichiometry? Go over homework One REALLY big problem Cw/hw make a review sheet Day 66 Wednesday, December 4, 2013 How do I demonstrate my knowledge of reaction stoichiometry? TEST ***ALL WORKSHEETS MUST BE COMPLETED ON NOTEBOOK PAPER*** Use your notes, text and ChemThink to complete the following worksheet. Worksheet 1 chemical equation chemical reaction synthesis coefficient decomposition subscript double displacement products reactants single displacement ____________________ 1. The starting substances in a chemical reaction are ____________________ 2. Two or more substances combine to form one new substance in ____ reactions. ____________________ 3. The process by which one or more substances are changed into one or more different substances is called _____ _____________________ 4. In the chemical reaction known as ______, one element displaces another in a compound. ____________________ 5. The breaking up of substances into simpler substances upon the supplying of energy is called ____________________ 6.The term referring to the substances formed by a chemical reaction, is . ____________________ 7. The positive and negative portions of two compounds are interchanged in ___ reactions. ____________________ 8. The number appearing before the formulas in a chemical equation that stands for the ratio of the substances involved is the _____ ____________________ 9. A(an) ___ is used to show how many ions of each type are in the formula and should NEVER be changed to balance an equation. Write the following word equation, but do not balance them. 1. A compound composed of 52.5% potassium and 47.5% chlorine reacts with silver nitrate to yield potassium nitrate and silver chloride 2. sodium and bromine yields sodium bromide. 3. zinc metal and oxygen gas produces zinc oxide. 4. sodium chloride yields chlorine gas and sodium metal 5. sodium bromide plus chlorine yields sodium chloride and bromine. 6. sodium hydrogen carbonate yields sodium carbonate and carbon dioxide plus water Balancing Equations Worksheet 2 1)________HNO3 + ___________Ba(OH)2 !_________H20 + ______________ Ba(NO3)2 2) _______C2H30H + _______O2 ! _________ CO2 + _________ H20 3) _________SiF4 + _________H20 ! _________ H2SiF6 +_________H2SiO3 4)__________ Mg3B2 + ________ H2O !_________ Mg(OH)2 + ___________ B2H6 5)____________ *2$3 + ___________ % !_________ *% + ____________ $2 6)___________ Si02 + _________ HF !_________ SiF4 + ____________ H2O 7)___________ XeF6 + __________ Si02 !_________ SiF4 + __________ XeOF4 Write and balance equations for each of the following: 8) Iron (III) iodide reacts with copper (II) nitrate to produce iron (III) nitrate and copper (II) iodide. 9) Ammonium phosphate reacts with lithium hydroxide to produce ammonium hydroxide and lithium phosphate. Word Equations Write the equations below as chemical equations and balance. Worksheet 3 Zinc + lead (II) nitrate yield zinc nitrate + lead Aluminum bromide + chlorine yield aluminum chloride + bromine Sodium phosphate + calcium chloride yield calcium phosphate + sodium chloride Potassium chlorate when heated yields potassium chloride + oxygen Aluminum + hydrochloric acid yield aluminum chloride + hydrogen gas Calcium hydroxide + phosphoric acid yield calcium phosphate + water Copper + sulfuric acid yield copper (II) sulfate + water + sulfur dioxide Hydrogen + nitrogen monoxide yield water and nitrogen Silver nitrate + sodium chloride yield silver chloride and sodium nitrate Write a balanced equation and indicate the reaction type. Worksheet 4 Aluminum nitrate (aq) + sodium hydroxide (aq) ( aluminum hydroxide (s) + sodium nitrate (aq) Potassium chlorate (s) ( potassium chloride (s) + oxygen (g) Phosphoric acid (aq) + magnesium hydroxide (aq) ( magnesium phosphate (s) + water (l) Ammonium nitrite (s) ( nitrogen (g) + water (l) Ammonia (g) + oxygen (g) ( nitrogen monoxide (g) + water (g) Barium chloride (aq) + sodium sulfate (aq) ( sodium chloride (aq) + barium sulfate(s) Iron (III) oxide (s) + carbon monoxide (g) ( iron (s) + carbon dioxide (g) Magnesium hydroxide(aq) + ammonium phosphate(aq) ( magnesium phosphate(s) + ammonia(g) + water(l) Iron (III) bromide (aq) + ammonium sulfide (aq) ( iron (III) sulfide (s) + ammonium bromide (aq) Calcium oxide (s) + diphosphorus pentoxide (s) ( calcium phosphate (s) Magnesium chloride (aq) + sulver nitrate (aq) ( magnesium nitrate (aq) + silver chloride (s) Sodium carbonate (aq) + sulfuric acid (aq) ( sodium sulfate (aq) + carbon dioxide (g) + water (l) Aluminum hydroxide (s) + acetic acid (aq) ( aluminum acetate (g) + water(l) Lead (II) nitrate (aq) + copper (II) sulfate(aq) ( lead (II) sulfate (s) + copper (II) nitrate (aq) Aluminum (s) + copper (II) chloride (aq) ( aluminum chloride (aq) + copper Iron (s) + silver acetate (aq) ( iron (II) acetate (aq) + silver (s) Aluminum acetate (aq) + sodium hydroxide (aq) ( aluminum hydroxide (s) + sodium acetate (aq) Bromine (l) _ calcium iodide (aq) ( calcium bromide (aq) + iodine (s) Copper (s) + sulfuric acid(aq) ( copper (II) sulfate (aq) + sulfur dioxide (g) + water (l) Calcium hydroxide (aq) + phosphoric acid (aq) ( calcium phosphate (s) + water (l) Magnesium nitrate (aq) + sulfuric acid(aq) ( magnesium sulfate (aq) + nitric acid(aq) Potassium carbonate (aq) + barium chloride (aq) ( potassium chloride (aq) + barium carbonate(s) Aluminum chloride (aq) + sulfuric acid (aq) ( aluminum sulfate (aq) + hydrogen chloride (g) Cadmium phosphate(s) + ammonium sulfide(aq) ( cadmium sulfide(s) + ammonium phosphate(aq) Sodium hydroxide (aq) + sulfuric acid (aq) ( sodium sulfate (aq) + water (l) Classification of Chemical Reactions Classify the reaction below as synthesis, decomposition, single replacement (cationic or anionic) or double replacement. Worksheet 5 2H2 + O2 ( 2H2O 2H2O ( 2H2 + O2 Zn + H2SO4 (ZnSO4 + H2 2CO + O2 ( 2CO2 2HgO ( 2Hg + O2 2KBr + Cl2 ( 2KCl + Br2 CaO + H2O ( Ca(OH)2 AgNO3 + NaCl ( AgCl + NaNO3 2H2O2 ( 2H2O + O2 Ca(OH)2 + H2SO4 ( CaSO4 + 2H2O Synthesis and Decomposition Problems Worksheet 6 A. Write and balance the following equations. 1. potassium oxide plus water 2. sodium plus fluorine 3. carbon dioxide plus water 4. hydrogen plus chlorine 5. potassium bicarbonate (heated) 6. sodium chloride (electrolyzed) 7. magnesium chlorate(heated) 8. calcium hydroxide(heated) 9. aluminum chloride(electrolyzed) 10. water(electrolyzed) 11. Lithium bromide dihydrate (heated) 12. lead(IV) oxide(heated) Complete and balance these combustion reactions. Worksheet 7 1) _________C3H8(g) + _________O2 ! 2) _________ CH3OH + _________O2 ( 3) ___________ CH4(g) + _________O2 ( 4) ___________ C4H10(g) + _________O2 ( Single-Replacement Reactions Worksheet 8 Step 1 - Write the formulas of the reactants on the left of the yield sign Step 2 - Look at the Activity Series to determine if the replacement can happen Step 3 - If the replacement can occur, complete the reaction and balance it. If the reaction cannot happen, put an "X" through the yield sign. 1. lead + zinc acetate ( 2. iron + aluminum oxide ( 3. silver nitrate + nickel ( 4. sodium bromide + iodine ( 5. aluminum bromide + chlorine ( 6. sodium iodide + bromine ( 7. calcium + hydrochloric acid ( 8. magnesium + nitric acid ( 9. silver + sulfuric acid ( 10. potassium + water ( sodium + water ( copper + calcium chloride ( Double-Replacement Reactions Worksheet 9 Examine the products of the following reactions, and determine in each whether a gas, water, or a precipitate is formed. Use solubility table to determine the solubilities of the reaction products. If there is no gas, water, or precipitate produced, put an "X" through the yield sign, because no reaction occurs. 1. aluminum iodide + mercury(II) chloride ( 2. silver nitrate + potassium phosphate ( 3. copper(II) bromide + aluminum chloride ( 4. calcium acetate + sodium carbonate ( 5. ammonium chloride + mercury(I) acetate ( 6. calcium nitrate + hydrochloric acid ( 7. iron(II) sulfide + hydrochloric acid ( 8. copper(II) hydroxide + acetic acid ( 9. calcium hydroxide + phosphoric acid ( 10. calcium bromide + potassium hydroxide ( Write a balanced equation and indicate the reaction type. Worksheet 10 magnesium (s) + oxygen (g) ( Aluminum (s) + hydrochloric acid ( Sodium oxide + sulfur dioxide ( Phosphoric acid ( Sodium chlorate (s) ( Zinc chloride (aq) + ammonium sulfide (aq) ( Zinc sulfide (s) + oxygen (g) ( Calcium carbonate ( Mercury (II) sulfate + ammonium nitrate ( Iron + copper (II) sulfate ( Zinc + sulfuric acid ( Dinitrogen pentoxide + water ( Chlorine + magnesium iodide ( Potassium + water ( Iron + hydrochloric acid ( Cobalt (III) hydroxide + nitric acid ( Bromine (l) + sodium iodide (aq) ( Sodium hydroxide + phosphoric acid ( Ammonium sulfate + calcium hydroxide ( Silver nitrate + potassium chloride ( Magnesium hydroxide + phosphoric acid ( Iron (II) sulfide + hydrochloric acid ( Ammonium sulfide + iron (II) nitrate ( Predicting Products of Chemical Reactions Predict the products of the reactions below. Then, write the balanced equation and classify the reaction. Worksheet 11 Magnesium bromide and chlorine Aluminum and iron (III) oxide Silver nitrate and zinc chloride Hydrogen peroxide (catalyzed by manganese dioxide MnO2 special substance) Zinc and hydrochloric acid Sulfuric acid and sodium hydroxide Sodium and hydrogen Acetic acid and copper Predicting reactions and balancing equations worksheet 12 I. Circle the appropriate reaction abbreviation indicating each reaction as a C = combustion SR = single-replacement reaction DR-ppt = double-replacement-ppt reaction Neut = neutralization reaction S = synthesis D = decomposition NR = no reaction II. Complete and balance each chemical equation, including all subscripts indicating physical state. C SR DR-ppt Neut S D NR 1. AgNO3(aq) + KI (aq) ( C SR DR-ppt Neut S D NR 2. Ba(NO3)2(aq) + Na2SO4 (aq) ( C SR DR-ppt Neut S D NR 3. Au (s) + FeCl2 (aq) ( C SR DR-ppt Neut S D NR 4. Ca(OH)2 (aq) + HC2H3O2 (aq) ( C SR DR-ppt Neut S D NR 5. Na (s) + H2O (l) ( C SR DR-ppt Neut S D NR 6. Zn (s) + S8(s) ( C SR DR-ppt Neut S D NR 7. K (s) + Na3PO4 (aq) ( C SR DR-ppt Neut S D NR 8. H2SO4 (aq) + Ni (s) ( C SR DR-ppt Neut S D NR 9. CaS (aq) + Ba(OH)2 (aq) ( C SR DR-ppt Neut S D NR 10. KCl (aq) + Cu (s) ( C SR DR-ppt Neut S D NR 11. H3PO4 (aq) + NaOH (aq) ( C SR DR-ppt Neut S D NR 12. Na (s) + Br2(l) ( C SR DR-ppt Neut S D NR 13. Pb(NO3)2 (aq) + BaS (aq) ( C SR DR-ppt Neut S D NR 14. HCl (aq) + Ag (s) ( C SR DR-ppt Neut S D NR 15. Zn (s) + H2O (l) ( C SR DR-ppt Neut S D NR 16. Mg(NO3)2 (aq) + KOH (aq) ( C SR DR-ppt Neut S D NR 17. Pb(C2H3O2)2 (aq) + LiBr (aq) ( C SR DR-ppt Neut S D NR 18. Li (s) + Al2(SO4)3(aq) ( C SR DR-ppt Neut S D NR 19. H3PO4(aq) + Na (s) ( C SR DR-ppt Neut S D NR 20. H2S (aq) + Ba(OH)2 (aq) ( C SR DR-ppt Neut S D NR 21. BaS (aq) + NaCl (aq) ( C SR DR-ppt Neut S D NR 22. ZnI2(aq) + AgNO3 (aq) ( C SR DR-ppt Neut S D NR 23. K (s) + P4(s) --> C SR DR-ppt Neut S D NR 24. KClO3 ( C SR DR-ppt Neut S D NR 25. C3H8 + O2 ( C SR DR-ppt Neut S D NR 26. HNO3 + RbOH ( C SR DR-ppt Neut S D NR 27. Sn + O2 ( C SR DR-ppt Neut S D NR 28 Li2O2 ( C SR DR-ppt Neut S D NR 29 NiO + CO2 ( C SR DR-ppt Neut S D NR 30. NH3 + H2SO4 ( C SR DR-ppt Neut S D NR 31. C4H10 + O2 ( C SR DR-ppt Neut S D NR 32. W + O2 ( Stoichiometry: Mole-Mole Problems Worksheet 13 How many moles of hydrogen are needed to completely react with two moles of nitrogen? How many moles of oxygen are produced by the decomposition of six moles of potassium chlorate? How many moles of hydrogen are produced from the reaction of three moles of zinc with an excess of hydrochloric acid? How many moles of oxygen are necessary to react completely with four moles of propane (C3H8)? How many moles of potassium nitrate are produced when two moles of potassium phosphate react with two moles of aluminum nitrate? 6 moles H2 9 moles O2 3 moles H2 20 moles O2 6 moles KNO3 Stoichiometry: Volume Volume Problems Worksheet 14 What volume of hydrogen is necessary to react with five liters of nitrogen to produce ammonia? (Assume constant temperature and pressure.) What volume of ammonia is produced in the reaction in problem 1? If 20. Liters of oxygen are consumed when propane (C3H8) completely combusts, how many liter of carbon dioxide are produced? If 30.0 mL of hydrogen are produced from the decomposition of water, how many milliliters of oxygen are produced? How many liter of carbon dioxide are produced if 75 liters of carbon monoxide are burned in oxygen? How many liters of oxygen are necessary? 15 L hydrogen 10. L ammonia 12 L CO2 15 mL oxygen 75L CO2, 37.5L O2 Stoichiometry: Mass Mass Problems Worksheet 15 How many grams of potassium chloride are produced if 25 g of potassium chlorate decomposes? How many grams of hydrogen are necessary to react completely with 50.0 g of nitrogen to produce ammonia? How many grams of ammonia are produced in the reaction in problem 2? How many grams of silver chloride are produced from 5.0 g of silver nitrate reaction with an excess of barium chloride? How much barium chloride is necessary to react with the silver nitrate in #4? 15 g KCl 10.7 g hydrogen 60.7 g ammonia 4.2 g AgCl 3.1 g BaCl2 Stoichiometry: Mixed Problems Worksheet 16 What volume of ammonia at STP is produced if 25.0 g of nitrogen is reacted with an excess of hydrogen? If 5.0 grams of potassium chlorate is decomposed, what volume of oxygen is produced at STP? How many gram of potassium chloride are produced in problem 2? What volume of hydrogen at STP is produced when 2.5 grams of zinc react with an excess of hydrochloric acid? NaOH + H2SO4 ( Na2SO4 + H2O How many molecules of water are produced if 2.0 g of sodium sulfate are produced in the above reaction? If 10.0 g of aluminum chloride are decomposed, how many molecules of chlorine are produced? 40.0 L Hydrogen 1.4 L oxygen 3.0g KCl 0.86 L hydrogen 8.5E21 waters 6.77E22 AlCl3 Stoichiometry: Limiting Reagent Worksheet 17 How many grams of ammonia can be produced from the reaction of 28 g of nitrogen and 25 grams of hydrogen? How much of the excess reagent in problem 1 is left over? What volume of hydrogen at STP is produced from the reaction of 50.0 g of magnesium and the equivalent of 75 g of hydrochloric acid? How much of the excess reagent in problem 3 is left over? Silver nitrate and sodium phosphate are reacted in equal amounts of 200. g each. How many grams of silver phosphate are produced? How much of the excess reagent in problem 5 is left? 34 g (substance omitted on purpose) 19 g 23 L 25.0 g 164 g 136 g Stoichiometry - Percent Yield Worksheet Worksheet 18 1) Balance the equation for the reaction of iron (III) phosphate with sodium sulfate to make iron (III) sulfate and sodium phosphate. a) If I perform this reaction with 25 grams of iron (III) phosphate and an excess of sodium sulfate, how many grams of iron (III) sulfate can I make? 33 grams b) If 18.5 grams of iron (III) sulfate are actually made when I do this reaction, what is my percent yield? c) Is the answer from problem #3 reasonable? Explain. 56% yes d) If I do this reaction with 15 grams of sodium sulfate and get a 65.0% yield, how many grams of sodium phosphate will I make? 7.48 g 2) LiOH + KCl ( LiCl + KOH a) I began this reaction with 20. grams of lithium hydroxide and 100.g potassium chloride. What is my theoretical yield of lithium chloride? 35g b) I actually produced 6 grams of lithium chloride. What is my percent yield? 17% 3) C3H8 + 5 O2 ( 3 CO2 + 4 H2O a) If I start with 5 grams of C3H8 and 5 grams oxygen, what is my theoretical yield of water? b) I got a percent yield of 75% How many grams of water did I make? 4) Be + 2 HCl ( BeCl2 + H2 My theoretical yield of beryllium chloride was 10.7 grams. If my actual yield was 4.5 grams, what was my percent yield? Follow The Yellow Brick Road Lab A For this activity you must complete each part in order. When you finish a part you will need to have your teacher initial that part. PART I: Write and balance each of the following equations. If it is already balanced, write the word balanced to the right of the equation. 1. Hydrogen peroxide (H2O2) reacts to produce water and oxygen gas. 2. HCl + NaOH ( NaCl + H2O 3. CaCl2 + F2 ( CaF2 + Cl2 4. Potassium chlorate decomposes upon heating to form potassium chloride and oxygen gas. 5. (NH4)2SO4 + Ba(NO3)2 ( BaSO4 + NH4NO3 6. C6H6 + O2 ( CO2 + H2O 7. Nitrogen gas and oxygen gas combine to form dinitrogen pentoxide. 8. SO3 + H2O ( H2SO4 9. C8H18 + O2 ( CO2 + H2O 10. Na2O + H2O ( NaOH 11. Potassium iodide and bromine react to form potassium bromide and iodine. 12. C4H8 + O2 ( CO2 + H2O 13. Zn + FeCl3 ( ZnCl2 + Fe 14. CaCO3 ( CaO + CO2 15. Phosphoric acid combines with calcium hydroxide to form calcium phosphate and water. PART II: Using the balanced equations, try to group them into five separate groups. Each group must contain exactly 3 equations that are related to one another in some way. You must explain why you grouped them into your categories.    Types of Chemical Reactions Lab B In this experiment, you will learn to differentiate among five general types of chemical reactions. You will carry out certain reactions yourself, while others will be demonstrated by your teacher. From your observations you will attempt to identify the products of each reaction and to determine the type of reaction that has taken place. The types of reactions you will consider are the following: combination reactions, decomposition reactions, single-replacement reactions, double-replacement reactions, and combustion reactions. The majority of common chemical reactions can be classified as belonging to one of these categories. A brief description of each reaction type is provided below. Sometimes there is a need to speed up a reaction. One way to do this is to heat the reaction. For most types of reactions, when heat is provided, the reaction speeds up. Another way to speed up the reaction is to use a catalyst. A catalyst is a compound or element that speeds up a reaction without being used up in the reaction. One type of catalyst your body uses is called enzymes. In this lab you will see a reaction that uses a catalyst that is an enzyme called catalase found in potatoes. Synthesis Reactions are reactions in which two or more substances combine to form a single product. The reactants may be elements or compounds, but the product is always a single product. An example of a combination reaction is the reaction of sulfur trioxide and water to form sulfuric acid. SO3 + H2O H2SO4 Decomposition Reactions are reactions in which a single substance breaks down into two or more simpler substances. There is always just a single reactant in a decomposition reaction. An example of a decomposition reaction is the breakdown of calcium carbonate upon heating: CaCO3 + heat CaO + CO2 Single-replacement Reactions are reactions in which an element within a compound is displaced by a separate element. This type of reaction always has two reactants, one of which is always an element. An example of a single-replacement reaction is the reaction of zinc metal with hydrochloric acid. Zn + 2HCl ZnCl2 + H2 Double-replacement Reactions are reactions in which a positive ion from one ionic compound exchanges with the positive ion of another ionic compound. These reactions typically occur in aqueous solution and result in either the formation of a precipitate, the production of a gas, or the formation of a molecular compound such as water. An example of a double-replacement reaction is the reaction that occurs between aqueous silver nitrate and aqueous sodium chloride. A precipitate of solid silver chloride is formed in this reaction. AgNO3 + NaCl AgCl + NaNO3 Combustion Reactions are reactions in which an element or compound reacts rapidly with oxygen gas to liberate heat and light energy. Commonly, the compounds combining with oxygen in these reactions are hydrocarbons, compounds consisting wholly of hydrogen and carbon. The well-known combustible fuels kerosene and gasoline, for instance, are hydrocarbon mixtures. The complete combustion of hydrocarbon yields carbon dioxide and water as the reaction products. If insufficient oxygen is available, combustion is not complete and carbon monoxide and elemental carbon may be obtained as additional products of the reaction. An example of a combustion reaction is the burning of methane gas to give water (in the form steam), carbon dioxide, heat, and light. CH4 + 2O2 CO2 + 2H2O + heat + light When testing for the identity of a gas you will be asked to use a glowing wooden splint or a burning splint to identify the gas. The gases you will be testing for are the following: Hydrogen, H2 = an explosion accompanies this reaction. It is an example of a combustion reaction. Oxygen, O2 = the splint will glow brighter. Carbon dioxide, CO2 = the wooden splint will go out. OBJECTIVES: To observe chemical reactions in order to determine the reaction type. To write balanced chemical equations for each reaction. To learn how to use the computer to type a lab report. EQUIPMENT: 5 test tubes (1 must be large) Mg ribbon 1 test tube holder Mg turnings 1 gas burner 6M HCl, hydrochloric acid 1 ring stand 3% peroxide solution 1 utility clamp (test tube clamp) raw potato piece 1 dropper pipet copper (II) sulfate 1 set of crucible tongs sodium hydroxide 2 beakers wooden splints matches SAFETY: Wear safety goggles. Hydrochloric acid is corrosive and can cause severe injury. If you spill acid on yourself, immediately flush the affected area with water for 2-3 minutes and notify the teacher. If acid should get into your eyes, begin flushing your eyes with water immediately and continue doing so for at least 20 minutes. Use the eyewash. If acid is spilled on the laboratory bench or on the floor, neutralize the spill with solid sodium bicarbonate, NaHCO3, before wiping it up with sponges or paper towels. The acid will be neutralized when bubbles of gas no longer form after addition of sodium bicarbonate. If you need to dispose of a small quantity of acid, neutralize the sample with sodium bicarbonate before pouring it down the drain. PROCEDURE: As you perform the experiment, record your observations in a data table. Copper (II) sulfate and sodium hydroxide. Place about 2mL of copper (II) sulfate in a test tube (1 dropper full). Place about 2mL of sodium hydroxide in a test tube. Mix pour one test tube into other. Record your observations in data table. Discard the solution into the sink with plenty of water. Magnesium metal and hydrochloric acid. Fill one medium size test tube halfway with 6M Hydrochloric acid. Place the test tube in a test tube rack. Put several magnesium turnings into the acid solution. If you observe a gas forming, test for its identity by collecting the gas and then holding a burning wood splint into the mouth of the test tube. Do not put the splint into the solution. Record your observations. Decant the liquid portion of the test tube contents into the sink; discard the solid into the waste container provided. Action of heat on hydrogen peroxide. Add 3mL of the 3% hydrogen peroxide solution to a medium test tube. Use a utility clamp to secure the tube to a ring stand. CAUTION: Make sure that the mouth of the tube is pointed away from you and away from everyone else. Heat the solution very gently. If you observe a gas forming, test for its identity by inserting a glowing wood splint into the mouth of the test tube. (Test must be done immediately, before solution boils, to get correct results). Do not put the splint into the solution. Record your observations. Rinse the contents of the test tube into the sink. The action of a catalyst on hydrogen peroxide. Fill the large test tube one-third with 3% hydrogen peroxide. Add a slice of raw potato that you can obtain form your teacher. Place the potato into the test tube and observe. Look specifically for bubbles of gas. The action of magnesium burning in air. WARNING: You must not look directly at this reaction. DO NOT TOUCH ANY PART OF THE MAGNESIUM RIBBON DURING THIS EXPERIMENT. You can see what you need to without looking directly at this reaction. Using tongs, obtain a piece of magnesium, 1 to 2 inches long, from the teacher. Hold the magnesium in a burner flame for approximately 1-2 seconds. Place the magnesium over a watch glass write down all observations. Discard the remaining product into the waster container provided. RESULTS: Decide which type of reaction is represented by each reaction observed in this experiment and write a balanced chemical equation for each reaction observed. Label each of the chemical equations you just wrote as one of the 5 reaction types. Although no combustion reactions were described in the procedure section, one combustion reaction did occur in the course of this experiment. (Actually, more than one occurred.) What was this reaction? Write the equation for this reaction. That Useful Ratio Lab C Question; How does the ratio of masses of substances in a chemical reaction compare with the ratio of their coefficients in a balanced equation? Materials; Metric balance Bunsen burner 250 mL Erlymyer flask Na2CO3 3M HC1 Hazard Warning: Wear safety goggles throughout this entire experiment. HC1 is extremely corrosive to skin and eyes. Sodium carbonate, Na2CO3/ may be a skin irritant. Procedure; Before beginning, read through the entire procedure and prepare a data table that will hold all of the required data. Find the mass of a clean Erlenmeyer flask dish and record this value in your data table. Add about 2 g of sodium carbonate (Na2CO3) to the Erlenmeyer flask and find the mass, again recording your data in the table. Obtain about 10 mL of 3M HC1 in a small beaker. Using a dropper pipet, slowly add 3M HCl to the flask by dropping the acid through the pour spout. Continue to add acid until an additional drop of acid no longer reacts. Carefully dry the contents to a constant mass by heating. Summing up: 1. Attach your data table to this worksheet. Be sure to double check to make certain that you have clearly labeled the column and that all of your numbers have units. 2. Write a balanced equation for the reaction between the sodium carbonate and the HC1. 3. From their masses, determine the number of moles of NaaC03 and NaCl. Hint: use your periodic table. 4. How does the ratio of the coefficients of NaaCO3: NaCl in the balanced equation compare with the ratio of their masses? 5. How does the ratio of the coefficients of Na2C03: NaCl compare with the ratio of their moles? 6. How do you explain the differences in the ratio in #4 above compared to the ratio in #5? The Bicarbonate Dilemma Lab D Question: How can you determine the products of a chemical reaction? Materials: Sodium bicarbonate (solid) metric balance Bunsen burner ring stand crucible Hazard Warning: Wear your safety goggles for this entire laboratory Procedure: One of the most appetizing smells in the world might be that of freshly baked cakes and muffins. In order to make such tasty morsels light and fluffy, the substance known as sodium bicarbonate (NaHCO3) must be included in the recipe. Sodium bicarbonate, alias baking soda, is the substance that causes many baked goods to rise. One of the reasons this rising action occurs is because when strongly heated in the oven, baking soda decomposes producing carbon dioxide (C02) gas. The carbon dioxide becomes trapped within the mixture to form the "air pockets" which provide the fluffy texture. A problem many beginning chemistry students face, is the ability to predict the products for a particular reaction. The decomposition of sodium bicarbonate presents an interesting dilemma. Interestingly, it seems to have four plausible, but different products as shown below. a. NaHCO3(s) ( NaOH (s) + CO2(g) b. NaHC03(s) ( Na(s) + H2(g) + C(s) + O2(g) c. NaHC03(s) ( Na2CO3(s) + CO2(g) + H20(g) d. NaHC03(s) ( Na2O(s) + CO2(g) + H20(g) Using a known amount of NaHCO3 and the laboratory equipment provided, your task is to determine which of the above equations predicts the correct products. Before beginning the heating process, decide what data you will need to collect to determine the number of grams of solid product produced in the reaction. In the space provided prepare a table in which to record your data. Ask your teacher to look over your data table before beginning. Remember, the fate of the free world is in your hands. So work carefully! Prelab: (This is in addition to the standard prelab) 1. Write a balanced equation for each of the equations listed above. 2. 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