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Essential Curriculum Menezes Unit 10: Chemical Reactions Author: J. Galinski, S. Menezes Unit 10 Chemical Reactions Page 1 of 28 Packet Grade: _______/_______ WS: 10pts each SWS: 20pts each Reading: 30pts Introductory Resources: Addison-Wesley v.5 - Chapter 8 Addison-Wesley v.4 - Chapter 7 Addison-Wesley v.3 - Chapter 7 Main Idea Summary: A chemical reaction can be concisely represented by a chemical equation. The substances that undergo a chemical reaction are the reactants. The new substances formed are the products. Special symbols are written after formulas in equations to show a substance’s state. The designations for solid, liquid, or gas, are (s), (l), and (g), respectively. A substance dissolved in water is designated (aq). A catalyst is a substance that increases reaction rate without being used up by the reaction. If a catalyst is used, its formula is written above the arrow. In accordance with the law of conservation of mass, a chemical equation must be balanced. In balancing an equation, coefficients are used so the same number of atoms of each element are on each side of the equation. In a synthesis reaction, there is always a single product. A decomposition reaction involves the breakdown of a single reactant. In a single replacement reaction, the reactants and products are an element and a compound. The activity series of metals can be used to predict whether single replacement reactions will take place. A double replacement reaction involves the exchange of cations between two compounds. This reaction generally takes place between two ionic compounds in aqueous solution. The solubility rules can be used to predict whether double replacement reactions will take place, and what product will be insoluble in water. A combustion reaction always involves oxygen. The products of the complete combustion of a hydrocarbon are carbon dioxide and water. A complete ionic equation shows all dissolved ionic compounds as their free ions. A net-ionic equation shows only the ions that take part in the actual reaction, and not the spectator ions, ions that do not participate in the reaction. Essential Curriculum Menezes Unit 10 Chemical Reactions Page 2 of 28 Unit 10– Chemical Equations NAME: _____________________ Laboratory Activity 10A – Balancing Categories Inquiry Activity A chemical equation sums up what occurs during a chemical reaction. All chemical reactions, whether simple or complex, desirable or undesirable, involve changing substances. One or more substances, the reactants, change into one or more new substances, the products. In writing reactions, you separate the reactants from the products by writing an arrow (→). The arrow means “yields” or “reacts to produce.” Reactants → Products Consider for a moment the number of possible chemical reactions. Since there are millions of known compounds, it is logical to expect that millions of different chemical reactions can occur in nature or be done in the laboratory. You learned to name many compounds in Unit 07 by following a system of nomenclature rather than memorizing common names for thousands of different compounds. Similarly, you can learn to recognize patterns of chemical behavior that allow you to predict the products in many chemical reactions. Laboratory Activity Instructions: 1. 2. 3. 4. 5. 6. 7. 8. Form a group of two students. Get construction paper, scissors, and glue from your instructor. Cut out the numbered chemical equations from the next page. Study each of the equations, looking for similarities and patterns. Based on any similarities or patterns that you recognize, put the equations into categories. Write out the rules that you used to create the categories on a sheet of paper or notecard. Glue the rules that you used to the center of the sheet of construction paper. Glue the equations onto the construction paper near other equations of the same type. Essential Curriculum Menezes Unit 10 Chemical Reactions Page 3 of 28 Unit 10 – Chemical Equations NAME: _____________________ Laboratory Activity 10A – Balancing Categories Inquiry Activity Equations (01) CH4 + 2O2 → CO2 + 2H2O (02) H2SO4 + 2KOH → 2H2O + K2SO4 (03) C2H4 + O2 → CO2 + H2O (04) Zn + 2HCl → ZnCl2 + H2 (05) 2Mg + O2 → 2MgO (06) 2C4H10 + 13O2 → 8CO2 + 10H2O (07) Fe + CuSO4 → FeSO4 + Cu (08) CaCO3 → CaO + CO2 (09) BaO + H2O → Ba(OH)2 (10) H2SO4 → H2O + SO3 (11) FeS + HCl → FeCl2 + H2S (12) 2NaCl → 2Na + Cl2 (13) AgNO3 + NaCl → AgCl + NaNO3 (14) Pb(NO3)2 + 2 KI → PbI2 + 2KNO3 (15) 2Na + 2H2O → 2NaOH + H2 (16) MgO + H2O → Mg(OH)2 (17) C3H8 + O2 → CO2 + H2O (18) Cl2 + 2NaBr → 2NaCl + Br2 (19) 2Na + Cl2 → 2NaCl (20) 2KClO3 → 2KCl + 3O2 Essential Curriculum Menezes Unit 10 Chemical Reactions Page 4 of 28 Name: _________________________________________ Period: _______________ Date: _________ SWS Word Equations Word equations: an equation in which the reactants and the products are written by words Ex: aluminum reacts with oxygen to produce aluminum oxide Word equation: writing out the chemical names and putting in the correct symbols aluminum + oxygen → aluminum oxide Skeleton equation: putting in the correct formulas for the chemical names Al(s) + O2(g) → Al2O3(s) Balanced Equation: using coefficients to balance the equation _4_ Al(s) + _3_ O2(g) → _2_ Al2O3(s) For each of the following, write the word equation, skeleton equation, and balanced equation. REMEMBER THE DIATOMIC MOLECULES AND TO CRISS CROSS CHARGES FOR IONIC COMPOUNDS! 1. hydrogen plus oxygen yield water Word Equation Skeleton Equation Balanced Equation 2. nitrogen plus hydrogen yield ammonia Word Equation Skeleton Equation Balanced Equation 3. aluminum bromide plus chloride yield aluminum chloride and bromine Word Equation Skeleton Equation Balanced Equation 4. hydrochloric acid (HCl) plus sodium hydroxide yield sodium chloride plus water Word Equation Skeleton Equation Balanced Equation 5. iron plus lead (II) sulfate react forming iron (II) sulfate plus lead Word Equation Skeleton Equation Balanced Equation Essential Curriculum Menezes Unit 10 Chemical Reactions Page 5 of 28 6. potassium chlorate when heated produces potassium chloride plus oxygen gas Word Equation Skeleton Equation Balanced Equation 7. sulfuric acid decomposes to form sulfur trioxide gas plus water Word Equation Skeleton Equation Balanced Equation 8. sodium oxide combines with water to make sodium hydroxide Word Equation Skeleton Equation Balanced Equation 9. potassium iodide reacts with bromine forming potassium bromide plus iodide Word Equation Skeleton Equation Balanced Equation 10. sodium phosphate reacts with calcium nitrate to produce sodium nitrate plus calcium phosphate Word Equation Skeleton Equation Balanced Equation 11. zinc and chromium (II) nitrate react to form zinc nitrate and chromium Word Equation Skeleton Equation Balanced Equation Essential Curriculum Menezes Unit 10 Chemical Reactions Page 6 of 28 12. hydrogen and nitrogen monoxide produce water and nitrogen Word Equation Skeleton Equation Balanced Equation 13. calcium hydroxide and phosphoric acid yield calcium phosphate and water Word Equation Skeleton Equation Balanced Equation 14. lithium plus oxygen combine to form lithium oxide Word Equation Skeleton Equation Balanced Equation 15. hydrogen reacts with nitrogen to form ammonia Word Equation Skeleton Equation Balanced Equation 16. ethane (C2H6) reacts with oxygen to form carbon dioxide and water Word Equation Skeleton Equation Balanced Equation 17. carbon tetrahydride reacts with oxygen to produce carbon dioxide and water Word Equation Skeleton Equation Balanced Equation Essential Curriculum Menezes Unit 10 Chemical Reactions Page 7 of 28 18. fluorine reacts with sodium chloride to produce sodium fluoride and chlorine Word Equation Skeleton Equation Balanced Equation 19. tricarbon octahydride combines with oxygen to produce carbon dioxide and water Word Equation Skeleton Equation Balanced Equation 20. magnesium sulfide reacts with lithium phosphide to yield magnesium phosphide and lithium sulfide Word Equation Skeleton Equation Balanced Equation 21. copper (II) chloride plus sodium hydroxide produces copper hydroxide and sodium chloride Word Equation Skeleton Equation Balanced Equation 22. zinc (II) chlorate yields zinc chloride and oxygen Word Equation Skeleton Equation Balanced Equation Essential Curriculum Menezes Unit 10– Chemical Equations Worksheet 10.01 – Balancing Basics Unit 10 Chemical Reactions Page 8 of 28 NAME: _____________________ Put numbers in the blanks to balance the following equations. Learn to recognize the distinguishing features of each reaction type. SYNTHESIS (also known as COMBINATION): ___S + ___O2 → ___SO2 ___S + ___O2 → ___SO3 ___P + ___O2 → ___P2O5 DECOMPOSITION: ___KClO3 → ___KCl + ___O2 ___H2O2 → ___H2O + ___O2 ___NaNO3 → ___NaNO2 + ___O2 SINGLE REPLACEMENT (also known as DISPLACEMENT): ___Na + ___H2O → ___NaOH + ___H2 ___Zn + ___NaOH → ___Na2ZnO2 + ___H2 ___Zn + ___HCl → ___ZnCl2 + ___H2 DOUBLE REPLACEMENT (also known as METATHESIS): ___Fe(OH)3 + ___H2SO4 → ___Fe2(SO4)3 + ___H2O ___MgCl2 + ___NaOH → ___Mg(OH)2 + ___NaCl ___AgNO3 + ___H2S → ___Ag2S + ___HNO3 COMBUSTION: ___C3H8 + ___O2 → ___CO2 + ___H2O ___C6H14 + ___O2 → ___CO2 + ___H2O ___C9H20 + ___O2 → ___CO2 + ___H2O Essential Curriculum Menezes Unit 10 Chemical Reactions Page 9 of 28 Unit 10 – Chemical Equations NAME: _____________________ Worksheet 10.02 – Synthesis and Decomposition Put numbers in the blanks to balance the following equations. Learn to recognize the distinguishing features of each reaction type. SYNTHESIS (also known as COMBINATION): ___Mg + ___N2 → ___Mg3N2 ___N2 + ___O 2 → ___NO 2 ___Cu + ___S → ___Cu 2S ___Na + ___O2 → ___Na2O ___Al + ___N2 → ___AlN ___Hg + ___I 2 → ___HgI2 ___Fe + ___O 2 → ___Fe2O3 ___NO + ___O2 → ___NO2 ___H2 + ___Cl2 → ___HCl DECOMPOSITION: ___HgO → ___Hg + ___O2 ___CaCO3 → ___CaO + ___CO2 ___CuSO 4∙5H2O → ___CuSO4 + ___H2O ___NH4NO3 → ___N2O + ___H2O ___BaO2 → ___BaO + ___O2 ___NO 2 → ___N2 + ___O 2 ___H2O → ___H2 + ___O2 ___NH3 → ___N2 + ___H2 ___NCl3 → ___N2 + ___Cl2 Essential Curriculum Menezes Unit 10 Chemical Reactions Page 10 of 28 Lab 10B: Balancing Equations with Gumdrops Name:___________________________ Introduction Balancing equations is an essential part of chemistry. If equations were not balanced the Law of Conservation of Matter would be broken. In this lab you will use gum drops and toothpicks to help you balance equations. Materials Data sheet Paper towels Gum drops Colored pencils Toothpicks Procedure Define the following: Balance-______________________________________________________________________________ Coefficient- __________________________________________________________________________ Subscript-___________________________________________________________ 1. Obtain a bag of gum drops for each color. Each color represents an element. 2. Look at your equation and identify the reactants and products. 3. Using the tooth picks and gum drops construct each compound. 4. On your data sheet make a sketch showing what each compound looks like in the equation. 5. Now evaluate if your equation is following the Law of Conservation of Matter by identifying the number of each type of atom for the reactant and product sides. 6. If your equation is not balanced build more compounds using tooth picks and gum drops until it is balanced. Remember you CANNOT change the compound only how many of each compound. 7. Sketch a picture to reflect how many of each compound was needed to make a balanced equation. 8. Write the balanced equation using chemical formulas and coefficients. 9. Repeat these steps with remaining equations. Data H2 + O 2 H2O Reactants Chemical Formula Sketch Products Balanced Equation Essential Curriculum Menezes Unit 10 Chemical Reactions Page 11 of 28 N2 + H 2 NH3 Reactants Products Balanced Equation Chemical Formula Sketch CO2 + H2O C6H12O6+ O2 Reactants Products Balanced Equation Chemical Formula Sketch P2 + O2 P2O5 Reactants Products Balanced Equation Chemical Formula Sketch N2 + Cl2 NCl3 Reactants Chemical Formula Sketch Products Balanced Equation Essential Curriculum Menezes Unit 10 Chemical Reactions Page 12 of 28 NAME: _____________________ Worksheet 10.03 – Synthesis Prediction Use the General Cases to predict the products of each reaction. Balance each equation when done. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B → AB AB → A + B AX + B → BX + A AX + BY → BX + AY CxHy + O2 → CO2 + H2O 1. Solid beryllium is left in a container with liquid bromine. 2. Solid bismuth is burned in air. 3. Cesium is put in a container with chlorine gas. 4. Phosphorus trichloride is placed in a chlorine rich atmosphere. 5. Solid magnesium oxide is placed in water 6. Sulfur trioxide is bubbled through water. 7. Solid gold is added to fluorine gas. 8. Solid calcium oxide is added to water. 9. Nitrogen monoxide gas is bubbled through water. 10. Hydrogen and oxygen gases are mixed. Essential Curriculum Menezes Unit 10 Chemical Reactions Page 13 of 28 Unit 10 – Chemical Equations Worksheet 10.04 – Decomposition Prediction NAME: _____________________ Use the General Cases to predict the products of each reaction. Balance each equation when done. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B → AB AB → A + B AX + B → BX + A AX + BY → BX + AY CxHy + O2 → CO2 + H2O 1. Potassium hydroxide is heated. 2. Lithium chlorate decomposes by heating. 3. Sodium carbonate is heated. 4. Sulfurous acid is boiled. 5. Molten aluminum chloride is electrolyzed. 6. A sample of magnesium carbonate is heated. 7. A sample of ammonium carbonate is heated. 8. Carbonic acid is boiled. 9. Hydrogen peroxide decomposes. 10. Ammonium hydroxide is heated. Essential Curriculum Menezes Unit 10 – Chemical Equations Laboratory Activity 10C – Synthesis Unit 10 Chemical Reactions Page 14 of 28 NAME: _____________________ 1. Wear Goggles 2. Observe a strip of magnesium ribbon. Write down any and all observed physical properties. 3. Use the sparklighter to ignite the Bunsen burner. 4. Use the crucible tongs to hold the magnesium ribbon in the Bunsen burner flame. Caution: DO NOT look directly at the chemical reaction, because it may cause damage to your eyes and permanently harm your vision. Remove the magnesium from the flame. 5. When the magnesium oxide has cooled, observe its properties. 6. Clean up your equipment and return it to your teacher. 7. Write a balanced equation explaining what happened in lab, causing the transformation of magnesium into magnesium oxide. Unit 10– Chemical Equations Laboratory Activity 10D – Decomposition 1. Wear Goggles. 2. Use a wooden splint to add a pinch of iodine crystals to a plastic cup that is ¾ full of water. Stir with a stirring rod. Make note of your observations. 3. Use a wooden splint to add a pinch of zinc dust to the same plastic cup. Stir with a stirring rod. Make n ote of your observations. 4. Attach electrical leads to a 9V battery while the solution settles. 5. Dip the wires into the solution and observe what happens. Record your observations. 6. Hold the wires in place for five minutes. Continue to observe and record. 7. When the reaction has occurred, and all necessary observations have been made, discard the wooden splints into the trash, discard the zinc iodide solution into the waste container, wash out the plastic cup, and clean up any other equipment and return it to your teacher. 8. Write a balanced equation explaining what happened in lab, regarding the decomposition of zinc iodide. Essential Curriculum Menezes Unit 10 Chemical Reactions Page 15 of 28 Unit 10 – Chemical Equations Worksheet 10.05 – Single Replacement NAME: _____________________ Put numbers in the blanks to balance the following equations. Use the Activity Series to answer the question at the right. (more reactive replaces less reactive in compounds.) SINGLE REPLACEMENT (also known as DISPLACEMENT): REACTION: WILL IT OCCUR? (Yes or No) ___Fe2O3 + ___Al → ___Al 2O 3 + ___Fe ________ ___Al + ___CuSO4 → ___Al2(SO4) 3 + ___Cu ________ ___Ca + ___LiNO 3 → ___Li + ___Ca(NO 3)2 ________ ___Al + ___H2SO4 → ___Al2(SO4)3 + ___H2 ________ ___Zn(NO3)2 + ___Ag → ___AgNO3 + ___Zn ________ ___MgCl2 + ___K → ___KCl + ___Mg ________ ___MgCl2 + ___Ag → ___AgCl + ___Mg ________ ___Cu + ___AgNO3 → ___Ag + ___Cu(NO3)2 ________ ___Mn + ___Pb(C2H3O 2)4 → ___Pb + ___Mn(C 2H3O2)2 ________ ___PtO 2 + ___H2 → ___Pt + ___H 2O ________ ___Fe + ___CuSO4 → ___Cu + ___FeSO4 ________ ___Co + ___Ba(NO3)2 → ___Ba + ___Co(NO3) 2 ________ ___Hg + ___Pt(OH) 2 → ___Pt + ___Hg(OH)2 ________ ___Al(C2H3O2) 3 + ___Mg → ___Al + ___Mg(C 2H3O2)2 ________ ___Sr(NO 3)2 + ___Na → ___NaNO 3 + ___Sr ________ ___AlF3 + ___Cl2 → ___AlCl3 + ___F 2 ________ ___HI + ___Br 2 → ___HBr + ___I 2 ________ ___Br2 + ___NaCl → ___NaBr + ___Cl 2 ________ Essential Curriculum Menezes Unit 10 Chemical Reactions Page 16 of 28 Unit 10 – Chemical Equations Worksheet 10.06 – Single Replacement Prediction NAME: _____________________ Use the General Cases to predict the products of each reaction. Balance each equation when done. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B → AB AB → A + B AX + B → BX + A AX + BY → BX + AY CxHy + O2 → CO2 + H2O 1. A piece of copper is dropped into a container of water. 2. Liquid bromine is added to a container of sodium iodide crystals. 3. An aluminum strip is immersed in a solution of silver nitrate. 4. Zinc pellets are added to a sulfuric acid solution. 5. Fluorine gas is bubbled into a solution of aluminum chloride. 6. Magnesium turnings are added to a solution of lead (II) acetate. 7. Iodine crystals are added to a solution of sodium chloride. 8. Calcium metal is added to a solution of nitrous acid. 9. A pea-size piece of lithium is added to water. 10. A solution of iron (III) chloride is poured over a piece of platinum wire. Essential Curriculum Menezes Unit 10 – Chemical Equations SWS Double Replacement Unit 10 Chemical Reactions Page 17 of 28 NAME: _____________________ Put numbers in the blanks to balance the following equations. Using the Solubility Rules, predict whether or not an insoluble product will be formed, and identify the predicted solid precipitate (or if none, the words “no reaction”) in the blank at the right. DOUBLE REPLACEMENT (also known as METATHESIS): REACTION: ___Pb(NO3)2 + ___NaBr → ___NaNO3 + ___PbBr2 ________ ___AgHCO3 + ___NaCl → ___NaHCO 3 + ___AgCl ________ ___K2SO4 + ___BaCl2 → ___BaSO4 + ___KCl ________ ___Ba(NO3)2 + ___Li2SiF6 → ___BaSiF6 + ___LiNO3 ________ ___AgF + ___Ca(NO3) 2 → ___AgNO 3 + ___CaF 2 ________ ___(NH4)2CrO4 + ___Fe(NO3)3 → ___NH4NO3 + ___Fe2(CrO4)3 ________ ___AgMnO4 + ___KCl → ___AgCl + ___KMnO 4 ________ ___KOH + ___Al2(SO4)3 → ___Al(OH)3 + ___K2SO4 ________ ___(NH4)2S + ___SrO → ___(NH 4)2O + ___SrS ________ ___AgClO4 + ___NaSCN → ___AgSCN + ___NaClO 4 ________ ___Na 2CO3 + ___BaCl2 → ___NaCl + ___BaCO 3 ________ Essential Curriculum Menezes Unit 10 – Chemical Equations WS 10.07 Double Replacement Unit 10 Chemical Reactions Page 18 of 28 NAME: _____________________ Put numbers in the blanks to balance the following equations. Using the Solubility Rules, rewrite the equations as overall equations, ionic equations, and net-ionic equations. Be sure to include identification of phases, like (s), (l), (g), or (aq) in the reactions. DOUBLE REPLACEMENT (also known as METATHESIS): REACTION: ___CaCl2 + ___K2CO3 → ___CaCO3 + ___KCl Ionic Equation: Spectator Ions: Net-Ionic Equation: ___AgNO 3 + ___FeCl3 → ___AgCl + ___Fe(NO3)3 Ionic Equation: Spectator Ions: Net-Ionic Equation: ___Al(OH)3 + ___HC2H3O2 → ___Al(C2H3O2) 3 + ___H2O Ionic Equation: Spectator Ions: Net-Ionic Equation: ___NaNO3 + ___K2SO3 → No Reaction (Answer the following to demonstrate why) Ionic Equation: Spectator Ions: Net-Ionic Equation: Essential Curriculum Menezes Unit 10 – Chemical Equations Worksheet 10.08– Double Replacement II Unit 10 Chemical Reactions Page 19 of 28 NAME: _____________________ Put numbers in the blanks to balance the following equations. Using the Solubility Rules, rewrite the equations as overall equations, ionic equations, and net-ionic equations. Be sure to include identification of phases, like (s), (l), (g), or (aq) in the reactions. DOUBLE REPLACEMENT (also known as METATHESIS): REACTION: ___Na 2SO4 + ___Ba(NO3)2 → ___NaNO 3 + ___BaSO4 Ionic Equation: Spectator Ions: Net-Ionic Equation: ___CuHCO3 + ___KBr → ___CuBr + ___KHCO 3 Ionic Equation: Spectator Ions: Net-Ionic Equation: ___MgCrO4 + ___BaI2 → ___MgI2 + ___BaCrO4 Ionic Equation: Spectator Ions: Net-Ionic Equation: ___NH4CN + ___Fe(NO3)3 → ___NH4NO3 + ___Fe(CN)3 Ionic Equation: Spectator Ions: Net-Ionic Equation: Essential Curriculum Menezes Unit 10 Chemical Reactions Page 20 of 28 Unit 10– Chemical Equations NAME: _____________________ Worksheet 10.09 – Double Replacement Prediction Use the General Cases to predict the products of each reaction. Balance each equation when done. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B → AB AB → A + B AX + B → BX + A AX + BY → BX + AY CxHy + O2 → CO2 + H2O 1. Ammonium sulfate and potassium hydroxide are mixed together. 2. Ammonium sulfide is reacted with hydrochloric acid. 3. Cobalt (II) chloride is combined with silver nitrate. 4. Solid calcium carbonate is reacted with sulfuric acid. 5. Potassium sulfite is reacted with hydrobromic acid. 6. Potassium sulfide is reacted with nitric acid. 7. Ammonium iodide is mixed with magnesium sulfate. 8. Solid titanium (IV) carbonate is added to hydrochloric acid. 9. Solid calcium sulfite is mixed with acetic acid. 10. Strontium hydroxide is added to ammonium sulfide. Essential Curriculum Menezes Unit 10 – Chemical Equations Laboratory Activity 10E – Single Replacement Unit 10 Chemical Reactions Page 21 of 28 NAME: _____________________ 1. Wear Goggles. 2. Place a test tube in the test tube rack and fill it one third of the way up with 6 M Hydrochloric acid (WARNING: Hydrochloric acid is very caustic! If you get any on you, wash it off immediately and tell the teacher). 3. Drop the strip of Magnesium into the acid. Observe what happens. Record your observations. 4. Cover the mouth of the test tube with the second test tube to capture any gas that is produced in the tube. 5. Use a lit match to test the gas for flammability by putting it in the mouth of the inverted tube. 6. Rinse all glassware thoroughly before returning it. 7. Write a balanced equation for the reaction of magnesium metal with hydrochloric acid. Remember to include symbols after each chemical formula to represent the phase of each reactant and product. Step 5 of the lab should give a hint as to the identity of one of the products. Unit 10 – Chemical Equations Laboratory Activity 10F – Double Replacement NAME: _____________________ 1. Wear Goggles. 2. Observe a solution of Lead (II) Nitrate, Pb(NO3) 2. 3. Fill a test tube about 1/3 of the way up with Pb(NO 3)2. 4. Observe a solution of Barium Chloride, BaCl 2. 5. Add an equal amount of BaCl 2 to the tube. 6. Record your observations of what occurs in the tube for the next several minutes. 7. Write out a balanced equation for what occurs in the tube. Predict the identity of the precipitate. 8. Clean up your station. Discard the contents of the tube in the solution waste container provided by the teacher. Essential Curriculum Menezes Unit 10 – Chemical Equations SWS Combustion Unit 10 Chemical Reactions Page 22 of 28 NAME: _____________________ Put numbers in the blanks to balance the following equations. COMBUSTION: REACTION: ___C3H8 + ___O2 → ___CO2 + ___H2O ___C4H10 + ___O2 → ___CO2 + ___H2O ___C5H12 + ___O2 → ___CO2 + ___H2O ___C7H16 + ___O2 → ___CO2 + ___H2O ___C7H14 + ___O2 → ___CO2 + ___H2O ___C9H20 + ___O2 → ___CO2 + ___H2O ___C6H14 + ___O2 → ___CO2 + ___H2O ___CH4 + ___O 2 → ___CO2 + ___H2O ___C2H2 + ___O2 → ___CO2 + ___H2O ___C2H4 + ___O2 → ___CO2 + ___H2O ___C2H6 + ___O2 → ___CO2 + ___H2O ___C8H18 + ___O2 → ___CO2 + ___H2O ___C6H6 + ___O2 → ___CO2 + ___H2O ___C6H12 + ___O2 → ___CO2 + ___H2O ___C6H12O6 + ___O2 → ___CO2 + ___H2O ___C12H22O 11 + ___O2 → ___CO2 + ___H2O ___C8H16 + ___O2 → ___CO2 + ___H2O ___C85H172 + ___O 2 → ___CO2 + ___H2O Essential Curriculum Menezes Unit 10 Chemical Reactions Page 23 of 28 Unit 10 – Chemical Equations Worksheet 10.10 – Combustion Prediction General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B → AB AB → A + B AX + B → BX + A AX + BY → BX + AY CxHy + O2 → CO2 + H2O 1. Ethanol is burned completely in air. 2. Propane is heated with oxygen gas. 3. Octane is burned in oxygen gas. 4. Copper (II) Sulfide is burned in air. 5. Solid Phosphorus is burned in air. 6. Barium sulfide is burned in air. 7. Iron is added to an oxygen rich environment. 8. Ethane is burned in oxygen gas. 9. Methane is burned in air. 10. Propanol is burned in air. NAME: _____________________ Essential Curriculum Menezes Unit 10 – Chemical Equations Laboratory Activity 10G – Combustion Unit 10 Chemical Reactions Page 24 of 28 NAME: _____________________ 1. Wear Goggles. 2. Use a dropper pipet to transfer 10 drops of Ethanol into a watch glass. 3. Drop a lit match into the watch glass and observe the flame. 4. Smother the flame by covering it with an inverted plastic cup. Observe the sides of the cup. What compound builds up on the sides of the cup? 5. Wash and dry the glassware you used. 6. Ethanol has a formula of CH 3CH2OH. Write a balanced equation for the combustion of ethanol. Essential Curriculum Menezes Unit 10 Chemical Reactions Page 25 of 28 Unit 10 – Chemical Equations SWS Basic Predictions NAME: _____________________ Use the General Cases to predict the products of each reaction. Balance each equation when done. Identify each reaction type in the blank at the right. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B → AB AB → A + B AX + B → BX + A AX + BY → BX + AY CxHy + O2 → CO2 + H2O REACTION: ___C5H12 + ___O2 → _________________ ___Zn + ___HCl → _________________ ___Na 2O → _________________ ___Li + ___Cl2 → _________________ ___Na 2SO4 + ___LiCl → _________________ ___C4H10 + ___O2 → _________________ ___Al2O3 → _________________ ___Al + ___I2 → _________________ ___Zn(OH)2 + ___Al2(CO3) 3 → _________________ ___FeCl3 → _________________ Essential Curriculum Menezes Unit 10 Chemical Reactions Page 26 of 28 Unit 10– Chemical Equations Worksheet 10.11 – More Predictions NAME: _____________________ Use the General Cases to predict the products of each reaction. Balance each equation when done. Identify each reaction type in the blank at the right. General Case: Synthesis: Decomposition: Single Replacement: Double Replacement: Combustion: A + B → AB AB → A + B AX + B → BX + A AX + BY → BX + AY CxHy + O2 → CO2 + H2O REACTION: ___CuCl2 + ___Na3PO 4 → _________________ ___C12H26 + ___O2 → _________________ ___FeCl3 → _________________ ___K2SO4 + ___Li → _________________ ___Na + ___O2 → _________________ ___C3H8 + ___O2 → _________________ ___KMnO4 + ___Li → _________________ ___Na 3P + ___Ba(OH)2 → _________________ ___H2O → _________________ ___HCl + ___Ca(OH)2 → _________________ Essential Curriculum Menezes Unit 10 – Chemical Equations SWS– Still More Predictions Unit 10 Chemical Reactions Page 27 of 28 NAME: _____________________ Predict the products of each reaction. Balance each equation when done. Identify each reaction type in the blank at the right. REACTION: ___Mg + ___O2 → _________________ ___AlCl3 → _________________ ___Na + ___O2 → _________________ ___HCl + ___NaOH → _________________ ___Pb(SO4) 2 + ___Al(C2H3O2)3 → _________________ ___C4H10 + ___O2 → _________________ ___H3PO4 + ___MgCO3 → _________________ ___HgCl2 + ___NaSCN → _________________ ___PtO 2 + ___H2 → _________________ ___CaCO3 + ___NaCl → _________________ ___Ag + ___HNO3 → _________________ ___NCl3 → _________________ ___MgSO 4∙7H2O → _________________ Essential Curriculum Menezes Unit 10 – Chemical Equations Worksheet 10.12 – Yet More Predictions Unit 10 Chemical Reactions Page 28 of 28 NAME: _____________________ Predict the products of each reaction. Balance each equation when done. Identify each reaction type in the blank at the right. REACTION: ___Sr + ___O 2 → ________________ ___Na + ___H2O → ________________ ___Zn + ___HCl → ________________ ___ICl → ________________ ___Fe(OH)3 + ___H2SO4 → ________________ ___C6H14 + ___O2 → ________________ ___Au(OH)3 + ___Na2CO3 → ________________ ___SrCl2 + ___NaOH → ________________ ___OCl2 → ________________ ___AgNO 3 + ___H2SO4 → ________________ ___Zn + ___O2 → ________________ ___Mg(OH)2 + ___NaF → ________________ ___C30H62 + ___O2 → ________________ ___Mg(NO3)2 + ___H2O → ________________ ___Au2S3 → ________________ ___Ti(MnO4)4 + ___Fe2O 3 → ________________ ___MnF2 + ___O2 → ________________ ___CO2 → ________________