Math Tutor. Answers 1. C 3. Balancing Chemical Equations 3CO 2 + 5O 2 + 4H 2. a. KI(aq) + Cl 2 (g) KCl(aq) + I 2 (s)
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1 Math Tutor A chemical equation is a written expression of an actual chemical reaction in which certain atoms, ions, or molecules become rearranged in a specific way. Therefore, the equation must represent exactly what happens in the reaction. Problem-Solving TIPS Balancing Chemical Equations Recall that atoms are never created or destroyed in chemical reactions. A balanced chemical equation shows that all of the atoms present in reactants are still present in products. Math Tutor Answers 1. C C a. 2KI + Cl 2 2KCl + I 2 b. 2Al + 3 S 4 Al 2 (S First, identify reactants and products. (You may find it helpful to write a word equation first.) Using correct formulas and symbols, write an unbalanced equation for the reaction. Balance atoms one element at a time by inserting coefficients. Identify elements that appear in only one reactant and one product, and balance the atoms of those elements first. If a polyatomic ion appears on both sides of the equation, treat it as a single unit. Double-check to be sure that the number of atoms of each element is the same on both sides of the equation. Sample When an aqueous solution of ammonium sulfate, (NH 4 S 4, is combined with an aqueous solution of silver nitrate, AgN 3, a precipitate of solid silver sulfate, Ag 2 S 4, forms, leaving ammonium nitrate, NH 4 N 3, in solution. Balance the equation for this reaction. As before, first write an equation with correct formulas for all reactants and products. (NH 4 S 4 + AgN 3 NH 4 N 3 + Ag 2 S 4 If you compare the number of silver atoms on each side, you can see that the equation is not balanced. This equation may look very complex, but it is really fairly simple. In many reactions involving polyatomic ions such as sulfate, nitrate, and ammonium, the ions do not change. In the equation above, you can see that N 3 is present on both sides, as are S 4 and NH 4. You can balance the equation by treating the groups as if they were single atoms. To balance the NH 4 groups, place a 2 in front of NH 4 N 3. This gives you two ammonium groups on the left and two on the right. Now, because you have two nitrate groups on the right, place a 2 in front of AgN 3 to give two nitrate groups on the left. Finally, check silver atoms and sulfate groups, and you find that they balance. (NH 4 S 4 + 2AgN 3 2NH 4 N 3 + Ag 2 S 4 1. When propane burns completely in air, the reaction forms carbon dioxide and water vapor. Balance the equation for this reaction. 2. Balance the following chemical equations: C C 2 + a. KI + Cl 2 KCl + I 2 b. Al + S 4 Al 2 (S 4 + Math Tutor 275 led /10/2011 5:12:39 AM Chemical Equations and Reactions 275
2 Chapter summary Review Answers 1. the evolution of energy, the production of a gas, the formation of a precipitate, and a color change 2. It must represent the known facts, contain the correct formulas for the reactants and products, and satisfy the law of conservation of mass. 3. a. a number that appears in front of a formula in a chemical equation. b. The number of atoms of each type in the formula is multiplied by the coefficient. 4. methane + oxygen carbon dioxide + water; CH C 2 + ; CH C the number of molecules, moles, and atoms of each element or compound composing the reactants and products as well as the mole ratios of the reactants to each other and to the products 6. They have only qualitative meaning; they do not express the relative quantities reactants or products. 7. a. a solution in water b. a substance that accelerates a chemical reaction but can be recovered unchanged c. a reaction in which the products re-form the original reactants CHAPTER 8 Summary SECTIN 1 Describing Chemical Reactions Four observations that suggest a chemical reaction is taking place are the evolution of energy as heat and light, the production of gas, a change in color, and the formation of a precipitate. A balanced chemical equation represents, with symbols and formulas, the identities and relative amounts of reactants and products in a chemical reaction. SECTIN 2 Types of Chemical Reactions Synthesis reactions are represented by the general equation A + X AX. Decomposition reactions are represented by the general equation AX A + X. Single-displacement reactions are represented by the general equations A + BX AX + B and Y + BX BY + X. Double-displacement reactions are represented by the general equation AX + BY AY + BX. In a combustion reaction, a substance combines with oxygen, releasing energy in the form of heat and light. SECTIN 3 Activity Series of the Elements PREMIUM CNTENT Activity series list the elements in order of their chemical reactivity and are useful in predicting whether a chemical reaction will occur. Chemists determine activity series through experiments. Interactive Review HMDScience.com KEY TERMS chemical equation precipitate coefficient word equation formula equation reversible reaction KEY TERMS synthesis reaction decomposition reaction electrolysis single-displacement reaction double-displacement reaction combustion reaction KEY TERMS activity series Review Games Concept Maps 8. a. KH d. CCl 4 b. Ca(N 3 e. MgBr 2 c. Na 2 C 3 9. (1) Balance different types of atoms one at a time; (2) balance types of atoms that appear only once on each side first; (3) balance as single units any polyatomic ions that appear on both sides; (4) balance H and last. 276 Chapter 8 Untitled /10/2011 5:12: Chapter 8
3 titled CHAPTER 8 Review SECTIN 1 Describing Chemical Reactions 1. List four observations that indicate that a chemical reaction may be taking place. 2. List the three requirements for a correctly written chemical equation. 3. a. What is meant by the term coefficient in relation to a chemical equation? b. How does the presence of a coefficient affect the number of atoms of each type in the formula that the coefficient precedes? 4. Give an example of a word equation, a formula equation, and a chemical equation. 5. What quantitative information is revealed by a chemical equation? 6. What limitations are associated with the use of both word and formula equations? 7. Define each of the following terms: a. aqueous solution b. catalyst c. reversible reaction 8. Write formulas for each of the following compounds: a. potassium hydroxide b. calcium nitrate c. sodium carbonate d. carbon tetrachloride e. magnesium bromide 9. What four guidelines are useful in balancing an equation? 10. How many atoms of each type are represented in each of the following? a. 3N 2 f. 5Fe(N 3 b. 2 g. 4Mg 3 (P 4 c. 4HN 3 h. 2(NH 4 S 4 d. 2Ca(H i. 6Al 2 (Se 4 e. 3Ba(Cl 3 j. 4C 3 PRACTICE PRBLEMS 11. Write the chemical equation that relates to each of the following word equations. Include symbols for physical states in the equation. a. solid zinc sulfide + oxygen gas solid zinc oxide + sulfur dioxide gas b. aqueous hydrochloric acid + aqueous barium hydroxide aqueous barium chloride + water c. aqueous nitric acid + aqueous calcium hydroxide aqueous calcium nitrate + water 12. Translate each of the following chemical equations into a sentence. a. 2ZnS Zn + 2S 2 b. Ca + 2 (l ) Ca(H + 2 c. AgN 3 + KI AgI + KN Balance each of the following: a. + Cl 2 HCl b. Al + Fe 2 3 Al Fe c. Pb(CH 3 C + S PbS + CH 3 CH 14. Identify and correct each error in the following equations, and then balance each equation. a. Li + 2 Li 2 b. + Cl 2 Cl 2 c. MgC 3 Mg 2 + C 2 d. NaI + Cl 2 NaCl + I 15. Write chemical equations for each of the following sentences: a. Aluminum reacts with oxygen to produce aluminum oxide. b. Phosphoric acid, H 3 P 4, is produced through the reaction between tetraphosphorus decoxide and water. c. Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. 16. Carbon tetrachloride is used as an intermediate chemical in the manufacture of other chemicals. It is prepared in liquid form by reacting chlorine gas with methane gas. Hydrogen chloride gas is also formed in this reaction. Write the balanced chemical equation for the production of carbon tetrachloride. (Hint: See Sample Problems C and D.) Chapter Review 277 5/10/2011 5:12:41 AM 10. a. 6N b. 4H, 2 c. 4H, 4N, 12 d. 2Ca, 4, 4H e. 3Ba, 6Cl, 18 f. 5Fe, 10N, 30 g. 12Mg, 8P, 32 h. 4N, 16H, 2S, 8 i. 12Al, 18Se, 72 j. 12C, 32H 11. a. 2ZnS Zn + 2S 2 b. 2HCl + Ba(H BaCl (l) c. 2HN 3 + Ca(H Ca(N (l) 12. a. Solid zinc sulfide reacts with oxygen gas to form solid zinc oxide and sulfur dioxide gas. b. When solid calcium hydride is added to water, aqueous calcium hydroxide and hydrogen gas are formed. c. Aqueous silver nitrate mixed with aqueous potassium iodide produces a precipitate of silver iodide and aqueous potassium nitrate. 13. a. + Cl 2 2HCl b. 2Al + Fe 2 3 Al Fe c. Pb(CH 3 C + S PbS + 2CH 3 CH 14. a. Li 2 is an inco rrect formula; 4Li + 2 2Li 2 b. Cl 2 is an inco rrect formula; + Cl 2 2HCl c. Mg 2 is an incorrect formula, and the equation as written is not balanced; MgC 3 Mg + C 2 d. I is an incorrect formula for iodine; the equation is not balanced; 2NaI + Cl 2 2NaCl + I a. 4Al Al 2 3 b. P H 3 P 4 c. Fe C 2Fe + 3C CH 4 + 4Cl 2 CCl 4 (l) + 4HCl 17. a. 2Mg + 2 2Mg b. 4Fe Fe 2 3 c. 2Li + Cl 2 2LiCl d. Ca + I 2 CaI 2 Chemical Equations and Reactions 277
4 chapter review 18. (1) Synthesis: two or more substances combine to form a new substance; A + X AX (2) Decomposition: a single compound undergoes a reaction that produces two or more simpler substances; AX A + X (3) Single-displacement: one element replaces another element in a compound; A + BX AX + B or Y + BX BY + X (4) Double-displacement: the ions of two compounds exchange places in an aqueous solution to form two new compounds; AX + BY BX + AY (5) Combustion: a substance combines with oxygen, releasing a large amount of energy in the form of light and heat; for example, C C by the addition of energy in the form of electricity or heat 20. electrolysis 21. a. aqueous solutions b. They generally involve less energy. 22. a. Sodium and oxygen react to form sodium oxide; 4Na + 2 2Na 2 b. Magnesium and fluorine combine to form magnesium fluoride; Mg + F 2 MgF a. 2Hg 2Hg + 2 b. 2 (l) electricity c. 2Ag 2 4Ag + 2 d. CuCl 2 electricity Cu + Cl a. Zn + Pb(N 3 Pb + Zn(N 3 b. 2Al + 3Hg(CH 3 C 17. For each of the following synthesis reactions, identify the missing reactant or product, and then balance the resulting equation. a. Mg + Mg b. + 2 Fe 2 3 c. Li + Cl 2 d. Ca + CaI 2 SECTIN 2 Types of Chemical Reactions 18. Define and give general equations for the five basic types of chemical reactions. 19. How are most decomposition reactions initiated? 20. A substance is decomposed by an electric current. What is the name of this type of reaction? 21. a. In what environment do many single-displacement reactions commonly occur? b. In general, how do single-displacement reactions compare with synthesis and decomposition reactions in terms of the amount of energy involved? PRACTICE PRBLEMS 22. Complete each of the following synthesis reactions by writing both a word equation and a chemical equation. a. sodium + oxygen b. magnesium + fluorine 23. Complete and balance the equations for the following decomposition reactions: a. Hg electricity b. (l) c. Ag 2 electricity d. CuCl Complete and balance the equations for the following single-displacement reactions: a. Zn + Pb(N 3 b. Al + Hg(CH 3 C c. Al + NiS 4 d. Na Complete and balance the equations for the following double-displacement reactions: a. AgN 3 + NaCl b. Mg(N 3 + KH c. LiH + Fe(N Complete and balance the equations for the following combustion reactions: a. CH b. C 3 H c. C 5 H Write and balance each of the following equations, and then identify each by type. a. hydrogen + iodine hydrogen iodide b. lithium + hydrochloric acid lithium chloride + hydrogen c. sodium carbonate sodium oxide + carbon dioxide d. mercury(ii) oxide mercury + oxygen e. magnesium hydroxide magnesium oxide + water 28. Identify the compound that could undergo decomposition to produce the following products, and then balance the final equation. a. magnesium oxide and water b. lead(ii) oxide and water c. lithium chloride and oxygen d. barium chloride and oxygen e. nickel chloride and oxygen 29. In each of the following combustion reactions, identify the missing reactant, product, or both, and then balance the resulting equation. a. C b C 2 c. C 2 H 5 H Complete and balance the equations for the following reactions, and then identify each by type. a. zinc + sulfur b. silver nitrate + potassium iodide c. toluene, C 7 + oxygen d. nonane, C oxygen SECTIN 3 Activity Series of the Elements 31. a. What is meant by the activity of an element? b. How does this description differ for metals and nonmetals? 3Hg + 2Al(CH 3 C c. 2Al + 3NiS 4 3Ni + Al 2 (S 4 d. 2Na + 2 2NaH a. AgN 3 + NaCl NaN 3 + AgCl b. Mg(N 3 + 2KH Mg(H + 2KN 3 c. 3LiH + Fe(N 3 Fe(H + 3LiN a. CH C b. 2C 3 H C 2 c. C 5 H C Chapter a. + I 2 2HI; synthesis b. 2Li + 2HCl 2LiCl + ; single Untitled /10/2011 5:12:42 displacement c. Na 2 C 3 Na 2 + C 2 ; decomposition d. 2Hg 2Hg + 2 ; decomposition e. Mg(H Mg + ; decomposition 28. a. magnesium hydroxide; Mg(H Mg + b. lead(ii) hydroxide; Pb(H Pb + c. lithium chlorate; 2LiCl 3 2LiCl d. barium chlorate; Ba(Cl 3 BaCl e. nickel chlorate; Ni(Cl 3 NiCl a. oxygen, carbon dioxide; C C b. pentane; C 5 H C 2 c. oxygen, carbon dioxide, water; C 2 H 5 H C a. Zn + S ZnS; synthesis b. AgN 3 + KI AgI + KN 3 ; double displacement 278 Chapter 8
5 titled a. What is an activity series of elements? b. What is the basis for the ordering of the el ements in the activity series? 33. a. What chemical principle is the basis for the activity series of metals? b. What is the significance of the distance between two metals in the activity series? PRACTICE PRBLEMS 34. Based on the activity series of metals and halogens, in Figure 3.1, which element within each pair is more likely to replace the other in a compound? a. K and Na e. Au and Ag b. Al and Ni f. Cl and I c. Bi and Cr g. Fe and Sr d. Cl and F h. I and F 35. Using the activity series in Figure 3.1, predict whether each of the possible reactions listed below will occur. For the reactions that will occur, write the products and balance the equation. a. Ni + CuCl 2 b. Zn + Pb(N 3 c. Cl 2 + KI d. Cu + FeS 4 e. Ba + (l) 36. Use the activity series in Figure 3.1 to predict whether each of the following synthesis reactions will occur, and write the chemical equations for those predicted to occur. a. Ca + 2 b. Ni + 2 c. Au + 2 Mixed Review 37. Ammonia reacts with oxygen to yield nitrogen and water. 4NH N 2 (l) Given this chemical equation, as well as the number of moles of the reactant or product indicated below, determine the number of moles of all remaining reactants and products. a. 3.0 mol 2 c. 1.0 mol N 2 b. 8.0 mol NH 3 d mol c. C C ; combustion d. C C ; combustion 38. Complete the following synthesis reactions by writing both the word and chemical equation for each: a. potassium + chlorine b. hydrogen + iodine c. magnesium + oxygen 39. Use the activity series in Figure 3.1 to predict which metal Sn, Mn, or Pt would be the best choice as a container for an acid. 40. Aqueous sodium hydroxide is produced commercially by the electrolysis of aqueous sodium chloride. Hydrogen and chlorine gases are also produced. Write the balanced chemical equation for the production of sodium hydroxide. Include the physical states of the reactants and products. 41. Balance each of the following: a. Ca(H + (NH 4 S 4 CaS 4 + NH 3 + b. C 2 H C 2 + c. Cu 2 S + 2 Cu 2 + S 2 d. Al + S 4 Al 2 (S Use the activity series in Figure 3.1 to predict whether each of the following reactions will occur, and write the balanced chemical equations for those predicted to occur. a. Al + 2 b. Pb + ZnCl Complete and balance the equations for the following reactions, and identify the type of reaction that each equation represents. a. (NH 4 S + ZnCl 2 + ZnS b. Al + Pb(N 3 c. Ba + (l) d. Cl 2 + KBr e. NH Pt N + (l) f. (l) Write and balance each of the following equations, and then identify each by type. a. copper + chlorine copper(ii) chloride b. calcium chlorate calcium chloride + oxygen c. lithium + water lithium hydroxide + hydrogen d. lead(ii) carbonate lead(ii) oxide + carbon dioxide Chapter Review a. the element s ability to react b. For metals, the ability to lose electrons; for nonmetals, the ability to gain them. 32. a. a set of elements listed according to the ease with which the elements undergo certain chemical reactions b. Elements are usually listed in order of their tendency to undergo singledisplacement reactions. An element can replace any element listed below it. 5/10/2011 5:12:42 AM 33. a. The activity series of metals is based on the ease with which metal atoms lose electrons to form ions in aqueous solution; the higher a metal is in the series, the more easily its atoms lose electrons and the greater its reactivity. b. The greater the distance is, the greater the likelihood that one metal will replace the other in a reaction. 34. a. K c. Cr e. Ag g. Sr b. Al d. F f. Cl h. F 35. a. Ni + CuCl 2 NiCl 2 + Cu b. Zn + Pb(N 3 Zn(N 3 + Pb c. Cl 2 + 2KI 2KCl + I 2 d. no reaction e. Ba + 2 (l) + Ba(H 36. a. 2Ca + 2 2Ca b. 2Ni + 2 2Ni c. no reaction 37. a. 4.0 mol NH 3, 2.0 mol N 2, and 6.0 mol b. 6.0 mol 2, 4.0 mol N 2, and 12.0 mol c. 2.0 mol NH 3, 1.5 mol 2, and 3.0 mol d mol NH 3, 0.20 mol 2, and 0.13 mol N a. Potassium and chlorine react to form potassium chloride; 2K + Cl 2 2KCl b. Hydrogen and iodine react to produce hydrogen iodide; + I 2 2HI c. Magnesium and oxygen react to produce magnesium oxide; 2Mg + 2 2Mg 39. Pt 40. 2NaCl + 2 (l) electricty 2NaH + + Cl a. Ca(H + (NH 4 S 4 CaS 4 + 2NH b. 2C 2 H C 2 c. 2Cu 2 S Cu 2 + 2S 2 d. 2Al + 3 S 4 Al 2 (S a. 4Al Al 2 3 b. no reaction 43. a. (NH 4 S + ZnCl 2 2NH 4 Cl + ZnS; double-displacement reaction b. 2Al + 3Pb(N 3 3Pb + 2Al(N 3 ; single-displacement reaction c. Ba + 2 (l) Ba(H + ; single-displacement reaction d. Cl 2 + 2KBr 2KCl + Br 2 (l); single-displacement reaction pt e. 4NH N (l); combustion reaction f. 2 (l) ; decomposition reaction Chemical Equations and Reactions 279
6 chapter review 44. a. Cu + Cl 2 CuCl 2 ; synthesis reaction b. Ca(Cl 3 CaCl ; decomposition reaction c. 2Li + 2 (l) 2LiH + ; single-displacement reaction d. PbC 3 Pb + C 2 ; decomposition reaction mol HCl a. Pb(N 3 + 2NaH Pb(H + 2NaN 3 b. C (l) C (l) c. 2Al(H + 3 S 4 Al 2 (S 4 (l) 48. The most reactive metals are on the left side in Groups 1 and 2. These metals have one (Group 1) or two (Group 2) electrons in their outer energy level. The energy needed to lose these electrons and achieve a stable configuration is much less than the energy needed to gain electrons. The least reactive metals are in the lower right of the transition metal block. The d sublevel of the fifth energy level is more than half full in these metals. These metals are much more stable than metals on the left side of the periodic table. 49. Q is most reactive, followed by A, then Z, and then J. 50. a. Rb 2 + (l) 2RbH b. 2Cs + I 2 2CsI c. Both are synthesis reactions. d. Solid rubidium oxide reacts with water to yield an aqueous solution of rubidium hydroxide. Solid cesium reacts with solid iodine to yield solid cesium iodide. 51. a. 2Ga + 6HBr 2GaBr b. 4Ga Ga 2 3 c. The first reaction is a single-displacement reaction; the second reaction is a synthesis reaction. d. Solid gallium reacts with hydrobromic acid to yield aqueous gallium bromide and hydrogen gas. Solid gallium reacts with oxygen gas to yield solid gallium oxide. 45. How many moles of HCl can be made from 6.15 mol and an excess of Cl 2? 46. What product is missing in the following equation? Mg + 2HCl MgCl Balance the following equations: a. Pb(N 3 + NaH Pb(H + NaN 3 b. C (l) + 2 C 2 + (l) c. Al(H + S 4 Al 2 (S 4 + (l) CRITICAL THINKING 48. Inferring Relationships Activity series are prepared by comparing single-displacement reactions between metals. Based on observations, the metals can be ranked by their ability to react. However, reactivity can be explained by the ease with which atoms of metals lose electrons. Using information from the activity series, identify the locations in the periodic table of the most reactive metals and the least reactive metals. Using your knowledge of electron configurations and periodic trends, infer possible explanations for the metals reactivity and position in the periodic table. 49. Analyzing Results Formulate an activity series for the hypothetical elements A, J, Q, and Z by using the following reaction information: A + ZX AX + Z J + ZX no reaction Q + AX QX + A USING THE HANDBK 50. Find the common-reactions section for Group 1 metals in the Elements Handbook in Appendix A. Use this information to answer the following: a. Write a balanced chemical equation for the formation of rubidium hydroxide from rubidum oxide. b. Write a balanced chemical equation for the formation of cesium iodide. c. Classify the reactions you wrote in (a) and (b). d. Write word equations for the reactions you wrote in (a) and (b). 280 Chapter 8 Visit HMDScience.com for appropriate scoring rubrics for items 52 and 53. Look for the following points in each report. 52. Students may discover that tin(ii) fluoride and sodium fluoride harden tooth enamel when the fluoride ion participates in a double-displacement reaction with the principal constituent of tooth enamel, hydroxyapatite. Ca 5 (P 4 H. Ca 5 (P 4 H + NaF Ca 5 (P 4 F+ NaH Fluoroapatite is harder, stronger, and 51. Find the common-reactions section for Group 13 in the Elements Handbook (Appendix A). Use this information to answer the following: a. Write a balanced chemical equation for the formation of gallium bromide prepared from hydrobromic acid. b. Write a balanced chemical equation for the formation of gallium oxide. c. Classify the reactions you wrote in (a) and (b). d. Write word equations for the reactions you wrote in (a) and (b). RESEARCH AND WRITING 52. Trace the evolution of municipal water fluoridation. What advantages and disadvantages are associated with this practice? 53. Research how a soda-acid fire extinguisher works, and write the chemical equation for the reaction. Check your house and other structures for different types of fire extinguishers, and ask your local fire department to verify the effectiveness of each type of extinguisher. ALTERNATIVE ASSESSMENT 54. Performance Assessment For one day, record situations that show evidence of a chemical change. Identify the reactants and the products, and determine whether there is proof of a chemical reaction. Classify each of the chemical reactions according to the common reaction types discussed in the chapter. more resistant to bacterial attack than hydroxyapatite. 53. The soda-acid fire extinguisher has been generally replaced by extinguishers consisting of liquid C 2. However, students can write the equation: S 4 + 2NaHC 3 2C 2 + Na 2 S Students may see evidence of chemical changes that are too complex to incorporate into a simple equation. Ask them to include the evidence. Students could summarize their findings in a chart. Untitled /10/2011 5:12: Chapter 8
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