Chemistry Distributed Practice Assessment

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1 Name Hour Chemistry Distributed Practice Assessment Practice 2011 Practice Exam A **This END OF COURSE Practice Exam is a qualifier for all Exam Takers 1

2 Objective 1 Answer questions relating to atomic structure 1. Determine the number of protons, neutrons, and electrons for a sodium-23 atom. 2. How many electrons are in the outermost energy level of a chlorine atom? 3. How many energy levels are in a sulfur atom? 4. What period is the element barium found in? 5. What group is the element lithium found in? Objective 2 Correctly classify a sample of matter as an element, compound, homogeneous solution or heterogeneous solution. 1. Sample A = Table Salt Sample B = Air Sample C = Neon Sample D = Soil Sample E = Concrete 5. Score: Objective 3 Apply the rules for naming and writing formulas for binary ionic compounds. Directions: Hook together the following ions to write the correct formula AND place the name of the resulting compound within the box. Arsenide Ion Calcium Ion Manganese (II) ion Bromide Ion 2

3 Objective 4 - Apply the rules for naming and writing formulas for ternary ionic compounds. Directions: Hook together the following ions to write the correct formula AND place the name of the resulting compound within the box. CN -1 Ni +2 NH 4 +1 CrO 4-2 PO 4-3 Objective 5 Apply the rules for naming binary molecular compounds. Directions: Name the following binary molecular compounds: 1. Cl 2 O 7 2. N 6 O 5 3. BCl 3 Objective 6 Apply the rules for writing formulas for binary molecular compounds. Directions: Write formulas for the following binary molecular compounds. 1. carbon disulfide 2. dinitrogen tetrahydride 3. pentaphosphorus trioxide 3

4 Objective 7 Apply the rules for naming and writing formulas for acids. Directions: Hook together the Hydrogen Ion to the following negative ions and write the correct formulas AND name the resulting acid. H +1 I -1 PO 3-3 CO 3-2 Objective 8 Use the mole to convert among measurements of mass, volume, and number of particles. Directions: Solve the following problems. Show work using *dimensional analysis. *(show how the units cancel throughout the entire problem.) Place your final answer on the line provided. Be sure to include the correct unit with your final answer. 1. Calculate the number of molecules in 30.3 grams of HCl. 2. Calculate the volume, in Liters, of 3.40 x molecules of Bromine (Br 2 ) gas at STP. 3. Calculate the mass of 53 Liters of Neon at STP. 4

5 Objective 9 Calculate the percent composition of a substance from its chemical formula or experimental data. Directions: Solve the following problems. Show work. Place your final answer on the line provided. Be sure to include the correct unit with your final answer. 1. When a 16.4 gram sample of Zirconium (II) oxide is decomposed into its elements by heating, grams of Zirconium is obtained. What is the percent composition of this compound? 2. Calculate the percent composition of Silicon Dioxide, a major component of sand. Objective 10 Derive the empirical formula of a compound from experimental data. Directions: Solve the following problems. Show work using *dimensional analysis. Place your final answer on the line provided. Be sure to include the correct unit with your final answer. 1. Determine the empirical formula for a compound that contains 93.3 % nitrogen and 6.7 % hydrogen. 2. Determine the empirical formula for a compound containing 40.4 % C, 7.8 % H, 35.9 % O, 15.7 % N. 5

6 Objective 11: Identify a reaction as combination, decomposition, single-replacement, double-replacement, complete combustion, or incomplete combustion. Directions: Identify the following reactions as a combination, decomposition, single-replacement, doublereplacement, complete combustion, or an incomplete combustion. 1. 4KMnO 4 2K 2 O + 4MnO + 5O 2 2. Cu + 2AgNO 3 Cu(NO 3 ) 2 + 2Ag 3. C 12 H 22 O O 2 12CO H 2 O 4. Na 2 O + CO 2 Na 2 CO CH 3 COCH 3 + 5O 2 6CO + 6H 2 O Objective 12: 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. sulfur dioxide reacts with water 2. chromium metal reacts with phosphorus producing a chromium (II) product 3. aluminum oxide reacts with water Objective 13: 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. Barium carbonate will decompose when heated 2. Ammonium chlorate decomposes when heated 3. Carbonic acid decomposes 6

7 Objective 14: Using the activity series, predict the products of a single-replacement 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. calcium metal is placed into a solution of mercury (II) bromide 2. fluorine gas is bubbled through a solution of aluminum bromide 3. lead metal is placed into a solution of iron (III) acetate Objective 15: 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. 1. Aqueous aluminum sulfate reacts with aqueous strontium nitrate Driving Force 2. Solutions of lithium carbonate reacts with silver nitrate Driving Force 3. Sulfuric acid is placed into a solution of cesium hydrogen carbonate, creating carbon dioxide gas, as well as two other products. Driving Force 7

8 Objective 16: 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. The term complete or incomplete will be provided in the sentence to guide you in your predictions. 1. C 7 H 6 O incompletely combusts. 2. Butane (C 4 H 10 ) completely combusts. Objective 17: 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. Show work using dimensional analysis. Place your final answer on the line provided. Be sure to include the correct unit with your final answer. 1. Write the equation for the formation of magnesium chloride from its constituent elements. 2. How many moles of magnesium are needed to form 3.5 moles of magnesium chloride? 3. How many grams of chlorine are necessary to produce 68.3 grams of magnesium chloride? 4. How many liters of chlorine are necessary to react completely with 238 grams of magnesium, assuming STP conditions? 8

9 Objective 18: 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: Answer the following questions. Show work using *dimensional analysis, when appropriate. Place your final answer on the line provided. Be sure to include the correct unit with your final answer. 1. Iron (III) oxide is produced from its constituent elements. a. Write the balanced equation for this reaction. b. How many grams of iron (III) oxide can be produced from the reaction of 50 grams of iron with 50 liters of oxygen gas, as STP? c. How many grams, or liters, of excess reagent are left over, unused? Objective 19: Calculate the theoretical yield, actual yield, or percent yield given appropriate information. Directions: Solve the following problems. Show work using *dimensional analysis. Place your final answer on the line provided. Be sure to include the correct unit with your final answer. 1. FeS 2 reacts with O 2 to produce Fe 2 O 3 and SO 3. a. Write the balanced equation for this reaction. b. If the reaction proceeds with a 91.3% yield, how many grams of Fe 2 O 3 are formed when 15.8 grams of FeS 2 reacts with excess O 2? c. How many liters of SO 3 are produced when the reaction from part b proceeds? 9

10 Objective 20: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical or physical process. 1. The specific heat of iron metal is J/g-K. How many J of heat are necessary to raise the temperature of a 1.05 kg block of iron from 25 o C to 88.5 o C? 2. When a certain substance with a mass of 100 grams is heated from 25 o C to 75 o C, it absorbed 4500 Joules of heat energy. Calculate the specific heat of the substance, and identify it using the following table: Water: Ice: Aluminum: Silver: Mercury: J/g-K 2.1 J/g-K 0.90 J/g-K 0.24 J/g-K 0.14 J/g-K Objective 21: Calculate enthalpy changes in chemical and physical processes from a thermochemical equation. Indicate if the change is endothermic or exothermic. Directions: Show all work, including units, to solve the following problems. 1. Gasohol contains ethanol, C 2 H 5 OH, which completely combusts to produce 1235 kj of heat energy. a. Write the balanced thermochemical equation: b. How much heat is released when 50 grams of ethanol completely combusts? 2. When magnesium metal combines with oxygen from the air, 1204 kj of heat energy is released. a. Write the balanced thermochemical equation: b. Calculate the amount of heat transferred when 2.4 g of magnesium reacts: c. How many grams of magnesium oxide are produced during an enthalpy change of -96 kj? Score: 10

11 Objective 22: Calculate enthalpy changes that occur using a warming or cooling curve; including phase changes such as melting, freezing, boiling, or condensing. Directions: Show all work, including units, to solve the following problems. DRAW A PHASE DIAGRAM! 1. How much heat (in kj) is absorbed when 50 grams of liquid water at 75 o C is converted to steam at 120 o C? The molar heat of vaporization for water is 40.7 kj/mole. The specific heat of water is J/g-K. The specific heat of steam, gaseous water, is 1.84 J/g-K. 2. What is the enthalpy change during the process in which of 50 grams of water at 50 o C is cooled to ice at -30 o C. The specific heat of liquid water is J/g-K. The specific heat of ice is 2.09 J/g-K. The molar heat of fusion for water is 6.01 kj/mol. Score: Objective 23: Apply Hess s law of heat summation to find enthalpy changes for chemical and physical processes. Directions: Show all work, including units, to solve the following problems. 1. Calculate the heat change, H, for the formation of nitrogen monoxide from its elements Write the target balanced equation here: Use these thermochemical equations: 4NH 3 (g) + 3O 2 (g) 2N 2 (g) + 6 H 2 O(g) 4NH 3 (g) + 5O 2 (g) 4NO (g) + 6H 2 O(g) H = kj H = kj Answer: 2. Calculate the enthalpy change for the reaction P 4 O 6 (s) + 2O 2 (g) P 4 O 10 (s) Given the following enthalpies of reaction: P 4 (s) + 3O 2 (g) P 4 O 6 (s) P 4 (s) + 5O 2 (g) P 4 O 10 (s) H = kj H = kj Score: Answer: 11

12 Objective 24: Apply Boyle s Law to problems involving pressure and volume at a constant temperature. Directions: Solve the following problems. Show all your work, including units within the problem. Place your final answer on the line. 1. A high-altitude balloon contains 50 Liters of helium gas at 109 kpa. What is the volume when the balloon rises to an altitude where the pressure is only 15 kpa? (Assume that the temperature remains constant.) 2. The pressure on a 4.25 Liter of anesthetic gas changes from 105 kpa to 28 kpa. What will be the new volume if the temperature remains constant? Objective 25: Use Charles s Law to solve problems involving temperature and volume at a constant pressure. Directions: Solve the following problems. Show all your work, including units within the problem. Place your final answer on the line. 1. If a sample of gas occupies 9.2 Liters at 325 Celsius, what will be its volume at 25 Celsius if the pressure does not change? 2. Exactly 10 Liters of air at 50 Celsius is warmed to 100 Celsius. What is the new volume if the pressure remains constant? Objective 26: Use Gay-Lussac s Law to solve problems involving pressure and temperature at a constant volume. Directions: Solve the following problems. Show all your work, including units within the problem. Place your final answer on the line. 1. A gas has a pressure of 6.58 kpa at 125 Celsius. What will be the pressure at 300 Celsius if the volume does not change? 2. The pressure in an automobile tire is 198 kpa at 27 Celsius. At the end of a trip on a hot sunny day, the pressure has risen to 225 kpa. What is the temperature of the air in the tire? (Assume the volume has not changed.) 12

13 Objective 27: Apply the combined gas law to problems involving pressure, temperature and volume. Directions: Solve the following problems. Show all your work, including units within the problem. Place your final answer on the line. 1. A gas at 155 kpa and 20 Celsius occupies a container with an initial volume of 2 Liters. By changing the volume, the pressure of the gas increases to 790 kpa as the temperature is raised to 120 Celsius. What is the new volume? 2. A 10 Liter air sample at a temperature of 78 Celsius has a pressure of 2.75 atmospheres. What will be the new pressure if the temperature is raised to 100 Celsius and the volume expands to 25 Liters? Objective 28: Apply the ideal gas law to problems involving pressure, volume, temperature and the number of moles. Directions: Solve the following problems. Show all your work, including units within the problem. Place your final answer on the line. 1. You fill a rigid steel cylinder that has a volume of 350 milliliters with nitrogen gas to a final pressure of 25 atmospheres at 30 Celsius. How many GRAMS of nitrogen gas does the cylinder contain? 2. What pressure, in kpa, will be exerted by 0.97 grams of a xenon gas at 25 Celsius if it is contained in a 0.73 Liter vessel? 13

14 Objective 29: Given the hydrogen-ion or hydroxide-ion concentration, calculate a ph. Indicate if a solution is acid, basic, or neutral. Calculate the ph of the following solutions. Indicate if it is acidic, basic or neutral. a. [H + ] = 2.3 x 10 5 b. [OH - ] = 3.2 x c. [OH - ] = 9.1 x 10-2 d. [H + ] = 3.8 x 10 7 e. [OH - ] = 1 x 10-7 _ Objective 30: Given the ph or poh of a solution, calculate the hydrogen-ion or hydroxide ion concentration. 1. Calculate the [H + ] from the following values: a. ph = 3.8 b. poh = 9.2 c. poh = 1.9 d. ph = 10.6 Objective 31: Identify the conjugate base associated with a given Bronsted-Lowry acid and the conjugate acid with a given Bronsted-Lowry base. 1. Give the conjugate acid of each of the following bases: a. Oxide ion b. Hydrogen sulfate ion c. Water d. Fluoride ion 2. Give the conjugate base of each of the following acids: a. Hydrosulfuric acid b. Water c. Hydrocyanic acid d. Hydrogen carbonate ion 14

15 Objective 32: Perform calculations involving Ka or Kb for weak acids and weak base equilibrium. 1. Calculate the ph of each of the following solution: 0.25 M propionic acid (HC 3 H 5 O 2 ), Ka = 1.3 x Calculate the Ka or Kb of the following solution: a. A student prepared a 0.75 M solution of formic acid (HCHO 2 ) and measured its ph using a ph meter. The ph at 25 C was found to be Calculate the Ka for formic acid at this temperature. Objective 33: Calculate the concentration of an acid or a base by using solution stoichiometry.(titration problems) 1. Calculate the volume of a 0.5 M Hydrochloric acid needed to completely neutralize 50 ml of a 1.5 M Calcium Hydroxide solution. 2. How many grams of sulfuric acid are necessary to completely neutralize 20 grams of barium hydroxide? 15

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