ࡱ>  ABC} Fbjbj55 __A,FEE%%%DiiimiQjqL''';Q=Q=Q=Q=Q=Q=Q&TV=Q9%3(&'3(3(=QEE vQ8883(ZE%;Q83(;Q88wM@OZi,/N'QQ0QGN\PWg5PW0OPW%O''8' 'S'''=Q=Q6'''Q3(3(3(3(PW''''''''' :   EMBED PBrush   UNIT 4: Chemical Reactions Stoichiometry and Thermodynamics Part A: Chemical Reactions  Big Picture Ideas: The identity of the reactants helps scientists to predict the products in a chemical reaction. Quantitative relationships exist with all chemical reactions that allow scientists to predict amounts of products formed, reactants consumed, and percent yield based on theoretical maximum. Big Picture Question: How can you predict the products in a chemical reaction? Suggested Resources Homework Assignments Classwork Assignments Laboratory Activities Formative Assessments Textbook pages: Chapter 9 Websites:  HYPERLINK "http://www.webelements.com" www.webelements.com Key Terms: chemical reaction chemical equation reactants yields products coefficient/mole subscript diatomic molecules synthesis/direct combination decomposition single replacement/displacement double replacement/displacement combustion activity series aqueous kinetics catalyst surface area  Directions: Use this information as a general reference tool to guide you through this unit. Dont hesitate to ask your teacher for help! By the conclusion of this unit, you should know the following: There are five basic types of chemical reactions (S, D, SR, DR, Comb.) that exhibit distinct patterns for the prediction of products. Experimental evidence can be used to identify products in a reaction. All reactions follow the Law of Conservation of Matter (balancing equations). Symbols are used to identify different aspects of a chemical reaction (states of matter, catalysts, heat, etc.). Collision theory describes characteristics for a successful reaction. Factors can be altered to affect the rate of a reaction (temperature, surface area, catalyst, concentration). By the conclusion of this unit, you should be able to do the following: Balance chemical reactions. Identify type of chemical reaction. Identify if a reaction will occur using an activity series. Predict products for a reaction. Write balance formula equation given chemical equation (words). Using the collision theory, explain how altering the temperature, surface area, concentration and the addition of a catalyst affects the rate of a reaction.  1. What type of reaction is it? a. element + element ( b. ionic compound + ionic compound ( c. element + ionic compound ( d. compound ( e. compound + oxygen ( 2. How can you tell if a chemical change has taken place? List examples. 3. Define a chemical reaction. Why must we balance chemical equations? (if it is a must there must be a law governing the concept). 4. Balance each reaction below. Identify each type the following reactions are: a) NaOH(aq) + Pb(NO3)2(aq) --> NaNO3(aq) + Pb(OH)2(s) b) CH4(g) + O2(g) --> CO2(g) + H2O(l) c) Fe(s) + NaBr(aq) --> FeBr3(aq) + Na(s) d) Pb(s) + O2(g) --> PbO (g) e) Na2CO3(s) --> Na2O(s) + CO2(g) 5. Complete and balance each reaction below: a) Mg + HCl ( _________ + ____________ b) C2H6 + O2 ( _________ + ____________ c) CaF2 + Na2SO4 ( _________ + ____________ d) Sr + N2 ( __________ 6. List three factors effecting the rate of a chemical reaction. Know why they effect the reaction rate (collision theory!) NOTES: CHEMICAL REACTIONS VOCABULARY: Products what is formed in a chemical reaction; right of arrow Reactants what goes into a chemical reaction; left of arrow ( yields + and (s) solid (l) liquid (g) gas (aq) aqueous only works when dissolved in water Catalyst a substance that speeds up a reaction but is not itself consumed; provides an easier reaction pathway that requires less activation energy Activation Energy (Ea) energy necessary to initiate a chemical reaction ENERGY OF CHEMICAL REACTIONS: Exothermic Reaction: H is  Endothermic Reaction: H = + (heat is a  product ) (heat is a  reactant )  SHAPE \* MERGEFORMAT  KINETICS: RATE OF CHEMICAL REACTIONS Collision Theory: for a reaction to occur, the reactants must collide with sufficient energy and with the proper orientation (and in the correct ratio) Factors Affecting Reaction Rate: Temperature if temperature is increased, the reaction will be quicker. faster moving particles collide more often, and more particles will have enough energy (Ea) when they collide Particle size (surface area) more exposed particles causes more collisions, so there will be more collisions with the correct orientation Nature of Reaction reaction rate is also determined by the properties of the reactants Adding a Catalyst or Inhibitor a catalyst speeds up a reaction by lowering the required activation energy an inhibitor slows down a reaction by raising the activation energy BALANCED CHEMICAL REACTIONS Law of Conservation of Matter: matter cannot be created or destroyed in a chemical reaction WORD ( FORMULA ( BALANCED EQUATIONS word equation: Hydrogen gas reacts with oxygen gas to form water formula equation: ____ H2 + O2 ( H2O ___________________________________________ diagram: H H + O = O ( O + O H H H H H H balanced reaction ____2 H2 + O2 ( 2 H2O ___________________________________________ word equation: Magnesium reacts with hydrochloric acid solution (HCl in water) to form magnesium chloride and hydrogen. Formula equation: ____ Mg + HCl ( MgCl2 + H2 __________________________________ diagram: Mg + H Cl ( Cl-1Mg+2Cl-1 + H H H Cl balanced reaction _______ Mg + 2 HCl ( MgCl2 + H2 ________________________________ Try balancing these chemical reactions: a. 2Na + H2SO4 ( Na2SO4 + H2 b. 2 K + Cl2 ( 2 KCl c. S8 + 8 O2 ( 8SO2 d. 3F2 + 2 FeBr3 ( 2 FeF3 + 3Br2 e. 3H2SO4 + 2 Al ( Al2(SO4)3 + 3H2 f. 2 C2H6 + 7 O2 ( 4CO2 + 6H2O g. 2 NaNO3 + Ca(MnO4)2 ( 2 NaMnO4 + Ca(NO3)2 h. SKIP P4 + KClO3 ( KCl + P2O5  EMBED Word.Document.12  ANSWERS: 1 + 3 ( 2 2 ( 2 + 3 2 + 1 ( 2 + 1 2 + 1 ( 2 1 + 2 ( 2 + 1 2 + 3 ( 6 + 1 1 + 2 ( 1 + 2 1 + 5 ( 3 + 4 2 + 25 ( 16 + 18 1 + 3 ( 1 + 3 4 + 5 ( 2 2 + 2 ( 2 + 1 2 ( 4 + 1 1 + 12 ( 8 6 + 6 ( 1 + 6 2 + 1 ( 2 + 1 2 + 1 ( 1 + 1 + 1 1 + 1 ( 1 + 1 + 1 2 + 1 ( 2 2 + 1 ( 2 + 1 SYNTHESIS, DECOMPOSITION AND COMBUSTION REACTIONS Types of Reactions: Synthesis, Decomposition and Combustion Synthesis A + B ( AB (1 product only) Decomposition AB ( A + B (1 reactant only) Combustion of a hydrocarbon CxHy + O2 ( CO2 + H2O Practice: Balance each reaction below. Then identify the reaction type. a. H2 + Br2 ( 2 HBr __synthesis______________ b. C4H8 + 6 O2 ( 4 CO2 + 4 H2O __combustion____________ c. 2 NaOH ( Na2O + H2O __decomposition__________ d. Ba(ClO3)2 ( BaCl2 + 3 O2 __decomposition__________ First write and balance the equation. Then identify the reaction type. e. phosphorus + oxygen ( tetraphosphorus decoxide __ synthesis _____________ 4 P + 5 O2 ( P4O10 f. pentane (C5H12) + oxygen ( carbon dioxide + water __ combustion ____________ C5H12 + 8 O2 ( 5 CO2 + 6 H2O g. magnesium chlorate ( magnesium chloride + oxygen ___ decomposition _________ Mg(ClO3)2 ( MgCl2 + 3 O2 h. when solid calcium carbonate is heated calcium oxide and carbon dioxide are formed ___ decomposition _________ CaCO3 ( CaO + CO2 i. the formation of calcium nitride from calcium and nitrogen ___ synthesis _____________ 3 Ca + N2 ( Ca3N2 j. sulfur trioxide mixes with water in the atmosphere to form sulfuric acid ___ synthesis ________ SO3 + H2O ( H2SO4 NOTES: SINGLE DISPLACEMENT REACTIONS & DOUBLE DISPLACEMENT REACTIONS 1. Single Displacement Reactions (aqueous ONLY) metals: standard: A(s) + BX (aq) ( AX (aq) + B(s) example: Cu + 2 AgNO3 ( Cu(NO3)2 + 2 Ag metal + acid: standard: A(s) + HX (aq) ( AX (aq) + H2(g) example: Mg + 2 HCl ( MgCl2 + H2 metal + water: standard: A(s) + H2O(l) ( AOH(aq) + H2(g) example: 2 K + 2 H2O ( 2 KOH + H2 halogens: standard: X2 + AY ( AX + Y2 example: F2 + 2 KI ( 2 KF + I2 2. Double Displacement (aqueous only) standard: AX (aq) + BY (aq) ( AY(aq) + BX(s) example: Ba(NO3)2 + NaI ( BaI2 + NaNO3 3. Identify the reaction type for each reaction below. Then complete and balance the reaction. _single displacement_ a. Ba + 2 AgNO3 ( Ba(NO3)2 + 2Ag __single displacement________b. F2 + 2KI ( 2 KF + I2 __double displacement c. NaOH + CaCl2 ( _2 NaCl + Ca(OH)2 ___single displacement d. Zn + H2SO4 ( ZnSO4 + H2 WRITING WORD EQUATIONS __decomposition_______________1. aluminum chlorate ( aluminum chloride + oxygen 2 Al(ClO3)3 ( 9 O2 + 2 AlCl3 __SR_______________ 2. lithium + iron (III) nitrate ( lithium nitrate + iron 3 Li + Fe(NO3)3 ( 3 LiNO3 + Fe __decomposition_______________ 3. magnesium carbonate ( magnesium oxide + carbon dioxide MgCO3 ( MgO + CO2 __synthesis____________ 4. tin + nitrogen ( tin (IV) nitride 3 Sn + 2 N2 ( Sn3N4 __SR____________ 5. Zinc reacts with nitric acid to form zinc nitrate and hydrogen Zn + 2 HNO3 ( Zn(NO3)2 + H2 __decomposition__________6. calcium hydroxide breaks down to form calcium oxide and water Ca(OH)2 ( CaO + H2O WRITING WORD EQUATIONS WITH PREDICTING PRODUCTS __synthesis_______________ 1. aluminum + oxygen ( 4 Al + 3 O2 ( 2 Al2O3 __SR____________ 2. sodium + silver nitrate ( Na + AgNO3 ( NaNO3 + Ag __SR_______________ 3. magnesium + hydrochloric acid ( Mg + 2 HCl ( MgCl2 + H2 ___DR______________ 4. solutions of iron (III) nitrate + potassium sulfate are mixed ( 2 Fe(NO3)3 + 3 K2SO4 ( Fe2(SO4)3 + 6 KNO3 ____SR_____________ 5. Chlorine gas is bubbled through a solution of lithium iodide ( Cl2 + 2 LiI ( 2 LiCl + I2 Fun With Predicting Reaction Products Predict the products of each of the following chemical reactions. If a reaction will not occur, explain why not: 1) ____ Ag2SO4 + __2__ NaNO3 ( 2 AgNO3 + Na2SO4 2) __2__ NaI + ____ CaSO4 ( CaI2 + Na2SO4 3) __2__ HNO3 + ____ Ca(OH)2 ( 2 H2O + Ca(NO3)2 4) ____ Zn + ___2__ HNO3 ( Zn(NO3)2 + H2 5) ____ AlCl3 + ____ (NH4)3PO4 ( AlPO4 + 3 NH4Cl 6) ___3_ Pb + ___2_ Fe(NO3)3 ( 3 Pb(NO3)2 + 2 Fe 7) ___2_ C3H6 + __9__ O2 ( 6 CO2 + 6 H2O 8) __2__ Na + ____ CaSO4 ( Na2SO4 + Ca WRITING WORD EQUATIONS a. lithium + nitrogen ( lithium nitride 6 Li + N2 ( 2 Li3N b. aluminum + oxygen ( aluminum oxide 4 Al + 3 O2 ( 2 Al2O3 c. sodium carbonate ( sodium oxide + carbon dioxide Na2CO3 ( Na2O + CO2 d. zinc + phosphoric acid ( zinc phosphate + hydrogen gas 3 Zn + 2 H3PO4 ( Zn3(PO4)2 + 3 H2 e. chlorine gas + lithium iodide ( lithium chloride + iodine Cl2 + 2 LiI ( 2 LiCl + I2 f. sodium hydroxide ( sodium oxide + water 2 NaOH ( Na2O + H2O g. magnesium reacts with hydrochloric acid to form magnesium chloride and hydrogen gas Mg + 2 HCl ( MgCl2 + H2 h. solutions of iron (III) chloride and sodium hydroxide react to form iron (III) hydroxide and sodium chloride FeCl3 + 3 NaOH ( Fe(OH)3 + 3 NaCl i. when sodium is added to water, sodium hydroxide and hydrogen gas are produced\ 2 Na + 2 H2O ( 2NaOH + H2 j. when zinc is placed in a solution of lead (II) nitrate, zinc nitrate and solid lead metal are formed Zn + Pb(NO3)2 ( Zn(NO3)2 + Pb HOMEWORK: BALANCING CHEMICAL REACTIONS NAME: DATE: 1. ___P4 + _5__O2 ( _2__P2O5 2. _2__Al + _6__HCl ( _2__AlCl3 + _3__H2 3. ___Al2(SO4)3 + _3__Ca(OH)2 ( _2__Al(OH)3 + _3__CaSO4 4. _8__H2S + _8__Cl2 ( ___S8 + _16__HCl 5. _3___Mg + ____N2 ( ____Mg3N2 6. _3___Fe + _4___H2O ( ____Fe3O4 + _4___H2 7. _2___NaOH + ____Cl2 ( ____NaCl + ____NaClO + ____H2O 8. _2___C4H10 + _13___O2 ( _8___CO2 + _10___H2O 9. __2___CH3OH + __3___O2 ( _2___CO2 + __4___ H2O HOMEWORK: SYNTHESIS, DECOMPOSITION AND COMBUSTION REACTIONS 1. Classify each equation below as synthesis, decomposition or combustion. Then balance each equation. __decomposition_________________ 1. 2 NaClO3 ( 2 NaCl + 3 O2 __synthesis______________________ 2. 2 Cu + S ( Cu2S __synthesis______________________ 3. 2 S + 3 O2 ( 2 SO3 __combustion___________________ 4. 2 C3H6 + 9 O2 ( 6 CO2 + 6 H2O 2. Classify each equation below as synthesis, decomposition or combustion. Write and balance the equation for the reaction. water _decomposition_______________________ 1. potassium hydroxide ( potassium oxide + hydrogen 2 KOH ( K2O + H2O __combustion______________________ 2. dicarbon tetrahydride + oxygen ( carbon dioxide + water C2H4 + 3 O2 (2 CO2 + 2 H2O __decomposition_____________________ 3. lithium chlorate ( lithium chloride + oxygen 2 LiClO3 ( 2 LiCl + 3 O2 __synthesis______________________ 4. magnesium + nitrogen ( magnesium nitride 3 Mg + N2 ( Mg3N2 __synthesis_____________________ 5. aluminum burns in pure oxygen to form aluminum oxide 4 Al + 3 O2 (2 Al2O3 __decomposition__________ 6. sodium carbonate is heated to form sodium oxide and carbon dioxide Na2CO3 ( Na2O + CO2 __synthesis_____________________ 7. water and dinitrogen pentoxide combine to form nitric acid H2O + N2O5 ( 2 HNO3 CLASSIFICATION OF CHEMICAL REACTIONS Classify the reactions below as synthesis, decomposition, single replacement or double replacement: 1. 2H2 + O2 ( 2H2O _____synthesis_& combustion ______ 2. 2H2O ( 2H2 + O2 ______decomposition_______________ 3. Zn + H2SO4 ( ZnSO4 + H2 ______single____________________ 4. 2CO + O2 ( 2CO2 ______synthesis__& combustion_____ 5. 2HgO ( 2Hg + O2 _____decomposition__________ 6. 2 KBr + Cl2 ( 2 KCl + Br2 _____single_____________________ 7. CaO + H2O ( Ca(OH)2 ____synthesis______________________ 8. AgNO3 + NaCl ( AgCl + NaNO3 ____double______________________ 9. 2 H2O2 ( 2H2O + O2 ____decomposition_______________ 10. Ca(OH)2 + H2SO4 ( CaSO4 + 2H2O ___double_______________________ 11. Copper metal is put into a solution of silver nitrate. Solid silver precipitates, and copper (II) nitrate solution is formed. Cu + 2 AgNO3 ( 2 Ag + Cu(NO3)2 single displacement 12. Methane gas burns in pure oxygen to give carbon dioxide and water CH4 + 2 O2 ( CO2 + 2 H2O combustion of a hydrocarbon 13. When sodium carbonate is heated, it breaks down to form sodium oxide and carbon dioxide. Na2CO3 ( Na2O + CO2 decomposition HOMEWORK PRACTICE REACTION WRITING Identify the reaction type for each reaction written below. Then write the balanced equation for each reaction. ____single displacement___ 1. Magnesium is placed in a solution of aluminum nitrate 3 Mg + 2 Al(NO3)3 (3 Mg(NO3)2 + 2 Al _______synthesis________________ 2. Calcium burns in pure oxygen. 2 Ca + O2 ( 2CaO ____combustion hydrocarbon_____ 3. The combustion of propane (C3H8) __________C3H8 + 5 O2 ( 3 CO2 + 4 H2O_________________ ____single displacement_____ 4. Fluorine is bubble through a solution of sodium bromide __________F2 + 2 NaBr ( 2 NaF + Br2 _______________________________________ ___double displacement______ 5. 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