Stoichiometry Chapter 9 Practice Assessment B
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1 NAME Hour Date Stoichiometry Chapter 9 Practice Assessment B
2 Objective 1: Interpret balanced chemical equations in terms of interacting moles, representative particles, masses, and gas volume at STP. Directions: Answer the following questions. 1. Write the balanced equation for the formation of gaseous dichlorine pentaoxide from its elements. Include the adjectives. 2. Interpret this equation in terms of the numbers of representative particles: 3. Interpret this equation in terms of numbers of moles 4. Interpret this equation in terms of mass 5. Interpret this equation in terms of volume
3 Objective 2: Calculate stoichiometric quantities from balanced chemical equations using units of moles, mass, representative particles, and volumes of gases at STP. Directions: Solve the following problems, showing all work. Be sure to include UNITS in the problems, as well as on your answer for credit. 1. Write the equation for the reaction of gaseous fluorine and aqueous lithium chloride. 2. How many moles of fluorine gas are needed to form 84 moles of lithium fluoride? 3. How many grams of lithium chloride are necessary to produce 37.2 grams of chlorine? 4. How many formula units of lithium chloride are necessary to react completely with 394 liters of fluorine, assuming STP conditions? 5. How many liters of fluorine are necessary to produce 5.1 x formula units of lithium chloride?
4 Objective 3: Identify and use the limiting reagent in a reaction to calculate the maximum amount of product(s) produced and the amount of excess reagent. Directions: Solve the following problems, showing all work. Be sure to include UNITS in the problems, as well as on your answer for credit. 1. Magnesium reacts with iron (III) bromide in a single replacement reaction. a. Write the balanced equation for this reaction. b. How many grams of magnesium bromide can be produced from the reaction of 332 grams of iron (III) bromide with 403 grams of magnesium? c. How many grams of excess reagent are left over, unused? 2. C 2 H 5 OH gas incompletely combusts. a. Write the balanced equation for this reaction. b. How many molecules of carbon dioxide are produced when liters of C 2 H 5 OH reacts with 411 grams of oxygen? Assume STP. c. How many moles of excess reagent are left over, unused?
5 Objective 4: Calculate the theoretical yield, actual yield, or percent yield given appropriate information. Directions: Solve the following problems, showing all work. Be sure to include UNITS in the problems, as well as on your answer for credit. 1. Aluminum oxide combines with water to form a base. a. Write the balanced equation for this reaction. b. In an experiment, 930 grams of aluminum oxide was reacted with excess water. If 1.35 kilograms of base are produced, what is the percent yield of this reaction? 2. Aqueous tin (IV) nitrate reacts with aqueous sodium hydroxide. a. Write the balanced equation for this double replacement reaction. b. If the reaction proceeds with a 96.3% yield, how many grams of precipitate are formed when 46 moles of tin (IV) nitrate reacts with excess sodium hydroxide? c. How many formula units of sodium hydroxide are consumed when the reaction from part b proceeds?
6 Objective 5: Distributed Practice: Part 1: Write a balanced equation for the following reactions. Also, indicate what category of reaction it is; (combination, decomposition, single-replacement, doublereplacement, or combustion.) 1. Solutions of copper sulfate and barium nitrate are mixed. 2. Mercury (II) oxide is heated. 3. Silver oxide is formed. 4. Potassium metal is placed into nitric acid. 5. Propanol, CH 3 CH 2 CH 2 OH, is burned.
7 Objective 6: Distributed Practice Part 2: Chemical and Physical Changes: Directions: a. Indicate if the following is a physical or a chemical change. b. Explain the reason(s) for your choice. c. For each chemical change, write a complete balanced equation. a. Nickel is dropped into water: b. Potassium is dropped into water: c. A solution of ammonium carbonate is placed into a solution of magnesium chloride: d. A solution of magnesium chloride is placed into a solution of sodium sulfate. e. Calcium and sulfur are placed in a test tube together, and heated.
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