Chemical Reactions Chapter 8 PART TWO
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1 NAME Hour Date Chemical Reactions Chapter 8 PART TWO Practice A Assessment 1
2 Objective 5: Predict the product of a combination reaction by writing a complete balanced equation. Directions: Write a complete balanced equation for the following combination reactions, predicting the correct product. 1. Magnesium metal reacting with iodine crystals 2. Solid aluminum oxide reacting with water 3. Gaseous sulfur trioxide reacting with water 4. The white power phosphorus reacting with oxygen from the air forming a yellow powder of diphosphorus pentoxide. 5. Copper metal reacts with sulfur powder forming a copper (I) product. 2
3 Objective 6: Predict the products of a decomposition reaction by writing a complete balanced equation. Directions: Write a complete balanced equation for the following decomposition reactions, predicting the correct products. 1. Phosphoric acid, when heated, decomposes 2. Solid magnesium hydroxide, when heated, decomposes 3. The white powder sodium chlorate, when heated, decomposes 4. Solid lithium carbonate is placed into a test tube and heated to cause decomposition 5. Solid mercury II oxide is treated with electricity to cause decomposition 3
4 Objective 7: Using the activity series, predict the products of a singlereplacement reaction by writing a complete balanced equation. Directions: Write a complete balanced equation for the following single-replacement reactions, predicting the correct products. Be sure to check the activity series to make sure the reaction occurs. 1. Zinc metal is dropped into sulfuric acid 2. Chlorine gas is bubbled into a solution of lithium iodide 3. Barium metal is dropped into water 4. Copper metal is dropped into a solution aluminum sulfate 5. Pieces of aluminum foil are dropped into a solution of copper (II) sulfate 4
5 Objective 8: Predict the products of a double-replacement reaction by writing a complete balanced equation and indicating the driving force of the reaction. Use the solubility chart to help predict precipitates. Directions: Write a complete balanced equation for the following double-replacement reactions, predicting the correct products. Include all the appropriate symbols that represent adjectives in your chemical sentence. 1. Aqueous potassium hydroxide reacts with sulfuric acid Driving Force 2. Aqueous potassium iodide reacts with aqueous lead (II) nitrate Driving Force 3. Acetic acid is placed into a solution of sodium bicarbonate, creating bubbles of carbon dioxide gas, as well as two other products. Driving Force 4. A solution of sodium hydroxide is placed into a solution of iron (III) nitrate Driving Force 5. Phosphoric acid is neutralized by a solution of calcium hydroxide Driving Force 5
6 Objective 9: Predict the products of either a complete or an incomplete combustion reaction by writing a complete balanced equation. Directions: Write a complete balanced equation for the following combustion reactions, predicting the correct products. 1. Butene (C 4 H 8 ) completely combusts. 2. Octane (C 8 H 18 ) incompletely combusts. 3. Acetone (C 3 H 6 O) completely combusts. 4. Glycerol (C 3 H 8 O 3 ) incompletely combusts. 5. Propene, (C 3 H 6 ) combusts completely. 6
7 Objective 10: Distributed Practice. Directions: Answer the following questions correctly. Show all work, including units, for mole calculations. 1. Classify the following as an element, compound, solution, or heterogeneous mixture. a. The air in this room. b. The mercury in a thermometer. c. The baking soda in my refrigerator. d. The chocolate chip ice cream I ate for lunch. 2. How many liters would 60 grams of krypton gas occupy at STP? 3. What is the mass of nitrogen atoms in a 160 gram sample of ammonium nitrate fertilizer? 4. What is the density of molecular bromine gas at STP? 5. Calculate the percent composition of iron (III) chlorate 7
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