Chemical Reactions Chapter 8 Assignment & Problem Set

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1 Chemical Reactions Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8.

2 Chemical Reactions 2 Study Guide: Things You Must Know Vocabulary (know the definition and what it means): chemical reaction yields reversible reaction catalyst balancing (chemical equations) solubility combination or synthesis reaction decomposition reaction single replacement reaction double replacement reaction combustion reaction electrolysis precipitate active element free element net ionic equation complete combustion incomplete combustion Learning Objectives (you should know:) observation that indicate a chemical reaction takes place. symbols used to write chemical equations. how to balance the mass in a chemical equation. how to use Table F to determine which ionic compounds are soluble in water. how to use Table J to predict products in single replacement reactions. how to recognize the five classes of reactions (combination or synthesis, decomposition, single replacement, double replacement, combustion) and how to predict the products. Honors: nonmetal oxides react with water to form acids, and metal oxides react with water to form bases; both are examples of combination reactions. Honors: how to write net ionic chemical equations. how to write reversible chemical equations. the difference between complete and incomplete combustion of carbon containing compounds. Key Reference Tables Table E: Selected Polyatomic Ions Table F: Solubility Guidelines for Aqueous Solutions Table J: Activity Series

3 Chemical Reactions 3 Read Chapter 8: Chemical Reactions Lab 6: Types of Chemical Reactions Lab 7: Precipitation Reactions Regents Tables Table F: Solubility Guidelines Table J: Activity Series Warm-ups and problems will be collected before you take the test. Answer all problems in the space provided. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units. 3. Show the final answer with units. There is no credit without showing work. Word Equations and Balancing 1. How is the law of conservation of mass related to balancing a chemical equation? 2. The equation for the formation of water from its elements, H 2(g) + O 2(g) H 2O(l) can easily be "balanced by changing the formula of the product to H 2O 2. Explain why this is incorrect. 3. Write formulas and other symbols for these substances. a. sulfur trioxide gas b. potassium nitrate dissolved in water c. heat supplied to a chemical reaction d. metallic copper e. liquid mercury f. zinc chloride as a catalyst 4. What is the purpose of a catalyst? 5. Write a balanced equation for this chemical reaction: heating potassium chlorate in the presence of the catalyst manganese dioxide produces oxygen gas. Potassium chloride is left as a solid. 6. Balance the following equations: a. SO 2 + O 2 SO 3 b. Fe 2O 3 + H 2 Fe + H 2O 7. Write a balanced chemical equation for each reaction. Use the necessary symbols. a. Bubbling chlorine gas through a solution of potassium iodide gives elemental iodine and a solution of potassium chloride. b. Bubbles of hydrogen gas and aqueous iron(iii) chloride are produced when metallic iron is dropped into hydrochloric acid.

4 Chemical Reactions 4 8. Use Table F to determine whether these ionic compounds are soluble or insoluble in water. If the compound is soluble, write (aq) after the compound, and if the compound is insoluble, write (s) after the compound. a. potassium iodide b. calcium chromate c. NH 4Br d. silver sulfate e. sodium phosphate f. CaCO 3 g. calcium sulfide f. silver nitrate g. Zn(C 2H 3O 2) 2 Combination or Synthesis Reactions 9. How do you recognize a combination reaction? 10. Write balanced chemical equations for the following combination reactions. a. Mg + O 2 b. Ca + S Decomposition Reactions 11. How do you recognize a decomposition reaction? 12. Write a balanced chemical equation for each decomposition reaction. a. nickel(ii) carbonate heat nickel(ii) oxide + carbon dioxide b. ammonium nitrate heat dinitrogen monoxide + water Single Replacement Reactions 13. How do you recognize a single replacement reaction? 14. Complete the equations for these single-replacement reactions that take place in aqueous solution. Balance each equation. If a reaction does not occur, write NR. a. Fe(s) + Pb(NO 3) 2(aq) b. Zn(s) + AgNO 3(aq) c. Cl 2(g) + NaI(aq) d. Ca(s) + H 2O(l) 15. Write a balanced chemical equation for each single-replacement reaction that takes place in aqueous solution. Write NR if a reaction does not occur. a. A piece of steel wool(iron) is placed in sulfuric acid. b. Bromine reacts with aqueous barium iodide.

5 Chemical Reactions 5 Double Replacement Reactions 16. How do you recognize a double replacement reaction? 17. What three types of products drive double replacement reactions? 18. Identify the precipitate formed when solutions of these ionic compounds are mixed. a. H 2SO 4(aq) + BaCl 2(aq) b. CaCl 2(aq) + Pb(NO 3) 2(aq) c. Ca(NO 3) 2(aq) + Na 2CO 3(aq) 19. Write the products for these double replacement reactions. Then balance each equation. a. NaOH(aq) + Fe(NO 3) 3 (aq) b. Ba(NO 3) 2(aq) + H 3PO 4(aq) c. HCl(aq) + Ca(OH) 2(aq) Net Ionic Reactions 20. Honors: Write a net ionic equation for each of these reactions and identify the spectator ions: a. HCl(aq) + AgNO 3(aq) b. Pb(C 2H 3O 2) 2(aq) + LiCl(aq) Combustion Reactions 21. Write a balanced equation for the complete combustion of each compound: a. ethane (C 2H 6) b. octene (C 8H 16) c. acetone (C 3H 6O) Any Reaction Class is Possible! 22. Complete and balance an equation for each reaction. State the reaction class. a. Al + Cl 2 b. Ag + HCl

6 Chemical Reactions 6 c. C 4H 4 + O 2 d. MgCl 2 e. Pb(NO 3) 2 + K 2CrO 4 PbCrO 4 + KNO 3 f. Cl 2 + KI KCl + I Name the class of reaction, predict the products and write a balanced chemical equation. a. Magnesium reacts with a solution of lead(ii) nitrate. b. An aqueous solution of magnesium nitrate reacts with an aqueous solution of sodium carbonate. c. Butane (C 4H 10) undergoes complete combustion. d. Calcium carbonate is heated to yield calcium oxide and carbon dioxide. e. Bromine reacts with an aqueous solution of potassium iodide. f. Honors: Write a net ionic equation for the reaction between an aqueous solution of copper(ii) chloride and an aqueous solution of ammonium hydroxide. Identify the spectator ions. Review 24. Calculate the number of moles in each substance: a L of nitrogen dioxide at (STP) b. 1.68g of magnesium ions c x molecules of carbon monoxide 25. Many coffees and colas contain the stimulant caffeine. The percent composition of caffeine is 49.5% C, 5.20% H, 16.5% O, and 28.9% N. What is the molecular formula of caffeine if its molar mass is g/mol?

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