Unit 3 Chemical Quantities THE MOLE
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1 Chemistry NAME Date Hour Unit 3 Chemical Quantities THE MOLE Practice Test Form C Second Half of Chapter 7
2 Objective 7 Use the mole to convert among measurements of mass, volume, and number of particles. 1. Calculate the number of molecules in 10 grams of carbon tetraoxide. 2. Calculate the volume, in Liters, of 6.95 x atoms of Argon gas at STP. 3. Calculate the mass of 23 Liters of disulfur pentaoxide at STP. 4. Determine the number of sulfur atoms in 45 grams of aluminum sulfate. A [] All work is shown using dimensional analysis. [] 4 out of 4 answered correctly. B [] All work is shown using dimensional analysis. [] 3 out of 4 are answered correctly. Not Yet []
3 Objective 8 Calculate the percent composition of a substance from its chemical formula or experimental data. 1. When a 13.5 gram sample of tin (II) oxide is decomposed into its elements by heating, 10.2 grams of tin is obtained. What is the percent composition of this compound? 2. Calculate the percent composition of sodium selenide. 3. An 10.2 gram piece of magnesium combines completely with 5.4 grams of oxygen to form a compound. What is the percent composition of this compound? B [] All work is shown using dimensional analysis. Not Yet []
4 Objective 9 Use a percent to calculate the number of grams of an element contained in a specific amount of a compound. 1. Calculate the mass of carbon in 50 grams of propane, C 3 H Calculate the mass of sulfur in 45 grams of ammonium sulfate. 3. Calculate the mass of oxygen in 250 grams of iron (II) oxide. B [] All work is shown using dimensional analysis. Not Yet []
5 Objective 10 Derive the empirical formula of a compound from experimental data. 1. Determine the empirical formula for a compound that contains 59.66% Chlorine and 40.34% Oxygen. 2. What is the empirical formula of a compound that is 25.26% Carbon, 14.74% Nitrogen, and 60.0% Fluorine? 3. Determine the empirical formula for a compound that contains 57.14% Sulfur and 42.86% Oxygen. B [] All work is shown using dimensional analysis. Not Yet []
6 Objective 11 Derive the molecular formula of a compound from experimental data. 1. Calculate the molecular formula of the compound whose molar mass is 410 grams and empirical formula is C 2 H 3 N. 2. Determine the molecular formula for a compound that is 63.16% C, 8.77% H, and 28.07% O; molar mass = 171 grams. 3. Caffeine, a stimulant found in coffee, contains 49.5% C, 5.15% H, 28.9% N, and 16.5% O by mass and has molar mass about 195 g/mol. Calculate its molecular formula. B [] All work is shown using dimensional analysis. Not Yet []
7 Objective 12 Distributed Practice Directions: Answer the following questions: 1. Identify the following as a physical property or a chemical property. a. density b. hardness c. corrosive d. tarnishes 2. Indicate what type of representative particles for the following: (atom, ion, formula unit, or molecule) a. Cesium b. Cesium oxide c. cobalt (II) d. carbon monoxide 3. Name the following compounds: a. Pb(NO 2 ) 4 b. S 2 O c. H 2 SO 3 d. Cu(C 2 H 3 O 2 ) 2 e. Na 2 S 4. Write formulas for the following compounds: a. Ammonium oxalate b. Diphosphorus pentafluoride c. Hypochlorous acid d. Chromium III chloride e. Chromium II Chlorate A [] 4 out of 4 answered correctly. B [] 3 out of 4 answered correctly. Not Yet []
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