Mr. Murdoch Unit 1, 2 & 3 Exam Practice Reg Chem '14 to '15

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1 Mr. Murdoch Unit 1, 2 & 3 Exam Practice Reg Chem '14 to '15 These 49 questions came from NYS Chemistry Regents Exams. These 49 questions are similar to the TYPES of questions you will have on your Unit 1, 2, & 3 Chemistry Exam on Wednesday, October 29th The answer key for these 49 questions will be posted on Mr. Murdoch's Chemistry website. 1. A student intended to make a salt solution with a concentration of 10.0 grams of solute per liter of solution. When the student s solution was analyzed, it was found to contain 8.90 grams of solute per liter of solution. What was the percent error in the concentration of the solution? 1) 1.10% 2) 8.90% 3) 11.0% 4) 18.9% 2. A student calculated the percent by mass of water in a hydrate as 14.2%. A hydrate is a compound that contains water as part of its crystal structure. If the accepted value is 14.7%, the student's percent error was 1) 2) 3) 4) 5. The diagram below represents a Celsius thermometer recording a certain temperature. 3. Which mass measurement contains four significant figures? 1) g 2) g 3) 1003 g 4) 3870 g 4. Expressed to the correct number of significant figures, the sum of two masses is grams. Which two masses produce this answer? 1) g g 2) g g 3) g g 4) g g Unit 1-3 Exam Practice Page 1 What is the correct reading of the thermometer? 1) 5 C 2) 4.3 C 3) 0.3 C 4) 4 C 6. During a laboratory activity, a student combined two solutions. In the laboratory report, the student wrote A yellow color appeared. The statement represents the student s recorded 1) conclusion 2) observation 3) hypothesis 4) inference 7. When a mixture of water, sand, and salt is filtered, what passes through the filter paper? 1) water, only 2) water and sand, only 3) water and salt, only 4) water, sand, and salt

2 8. Which mixture can be separated by using the equipment shown below? 10. Given the diagrams X, Y, and Z below: 1) NaCl(aq) and SiO2(s) 2) NaCl(aq) and C6H12O6(aq) 3) CO2(aq) and NaCl(aq) 4) CO2(aq) and C6H12O6(aq) 9. A dry mixture of KNO3 and sand could be separated by 1) adding water to the mixture and filtering 2) adding water to the mixture and evaporating 3) heating the mixture to a high temperature 4) cooling the mixture to a low temperature Which diagram or diagrams represent a mixture of elements A and B? 1) X, only 2) Z, only 3) X and Y 4) X and Z 11. Which of these contains only one substance? 1) distilled water 2) sugar water 3) saltwater 4) rainwater 12. Which of these terms refers to matter that could be heterogeneous? 1) element 2) mixture 3) compound 4) solution 13. One similarity between all mixtures and compounds is that both 1) are heterogeneous 2) are homogeneous 3) combine in a definite ratio 4) consist of two or more substances 14. Which sample of matter is classified as a solution? 1) H2O(s) 2) H2O( ) 3) CO2(g) 4) CO2(aq) 15. According to Reference Table H, what is the vapor pressure of propanone at 45 C? 1) 22 kpa 2) 33 kpa 3) 70 kpa 4) 98 kpa Unit 1-3 Exam Practice Page 2

3 16. As the temperature of a liquid increases, its vapor pressure 1) decreases 2) increases 3) remains the same 17. Based on Reference Table H, which sample has the highest vapor pressure? 1) water at 20ºC 2) water at 80ºC 3) ethanol at 50ºC 4) ethanol at 65ºC 18. Which sample of water has the lowest vapor pressure? 1) 100 ml at 50ºC 2) 200 ml at 30ºC 3) 300 ml at 40ºC 4) 400 ml at 20ºC 19. The freezing point of bromine is 1) 539 C 2) 539 C 3) 7 C 4) 7 C 20. In which equation does the term "heat" represent heat of fusion? 1) NaCl(s) + heat NaCl( ) 2) NaOH(aq) + HCl(aq) NaCl(aq) + H2O( ) + heat 3) H2O( ) + heat H2O(g) 4) H2O( ) + HCl(g) H3O + (aq) + Cl (aq) + heat 21. The graph below represents the heating curve of a substance that starts as a solid below its freezing point. 22. A gas occupies a volume of 40.0 milliliters at 20 C. If the volume is increased to 80.0 milliliters at constant pressure, the resulting temperature will be equal to 1) 2) 3) 4) 23. Which graph shows the pressure-temperature relationship expected for an ideal gas? 1) 2) 3) 4) What is the melting point of this substance? 1) 30 C 2) 55 C 3) 90 C 4) 120 C 24. A 3.00-liter sample of gas is at 288 K and 1.00 atm. If the pressure of the gas is increased to 2.00 atm and its volume is decreased to 1.50 liters, the Kelvin temperature of the sample will be 1) 144 K 2) 288 K 3) 432 K 4) 576 K Unit 1-3 Exam Practice Page 3

4 25. Which temperature change would cause the volume of a sample of an ideal gas to double when the pressure of the sample remains the same? 1) from 200ºC to 400ºC 2) from 400ºC to 200ºC 3) from 200 K to 400 K 4) from 400 K to 200 K 26. As the temperature of a gas increases at constant pressure, the volume of the gas 1) decreases 2) increases 3) remains the same 27. At the same temperature and pressure, 1.0 liter of CO(g) and 1.0 liter of CO2(g) have 1) equal masses and the same number of molecules 2) different masses and a different number of molecules 3) equal volumes and the same number of molecules 4) different volumes and a different number of molecules 28. A closed container holds 3.0 moles of CO2 gas at STP. What is the total number of moles of Ne(g) that can be placed in a container of the same size at STP? 1) 1.0 mole 2) 1.5 moles 3) 3.0 moles 4) 0.0 moles 29. A real gas behaves more like an ideal gas when the gas molecules are 1) close and have strong attractive forces between them 2) close and have weak attractive forces between them 3) far apart and have strong attractive forces between them 4) far apart and have weak attractive forces between them 30. A real gas differs from an ideal gas because the molecules of real gas have 1) some volume and no attraction for each other 2) some volume and some attraction for each other 3) no volume and no attraction for each other 4) no volume and some attraction for each other 31. Two basic properties of the gas phase are 1) a definite shape and a definite volume 2) a definite shape but no definite volume 3) no definite shape but a definite volume 4) no definite shape and no definite volume 32. An increase in the average kinetic energy of a sample of copper atoms occurs with an increase in 1) concentration 2) temperature 3) pressure 4) volume 33. Which change in the temperature of a 1-gram sample of water would cause the greatest increase in the average kinetic energy of its molecules? 1) 1 C to 10 C 2) 10 C to 1 C 3) 50 C to 60 C 4) 60 C to 50 C 34. A sealed flask containing 1.0 mole of H2(g) and a sealed flask containing 2.0 moles of He(g) are at the same temperature. The two gases must have equal 1) masses 2) volumes 3) average kinetic energies 4) numbers of molecules Unit 1-3 Exam Practice Page 4

5 35. A student determines the density of zinc to be 7.56 grams per milliliter. If the accepted density is 7.14 grams per milliliter, what is the student s percent error? Show a correct numerical setup. Record your answer. 36. A student used a balance and a graduated cylinder to collect the following data: a Calculate the density of the element. Show your work. Include the appropriate number of significant figures and proper units. b If the accepted value is 6.93 grams per milliliter, calculate the percent error. c What error is introduced if the volume of the sample is determined first? 37. Base your answers to the following questions on the information below. A hot pack contains chemicals that can be activated to produce heat. A cold pack contains chemicals that feel cold when activated. a Based on energy flow, state the type of chemical change that occurs in a hot pack. b A cold pack is placed on an injured leg. Indicate the direction of the flow of energy between the leg and the cold pack. c What is the Law of Conservation of Energy? Describe how the Law of Conservation of Energy applies to the chemical reaction that occurs in the hot pack. 38. Base your answer to the following question on the information below. Given the equation for the dissolving of sodium chloride in water: When NaCl(s) is added to water in a 250-milliliter beaker, the temperature of the mixture is lower than the original temperature of the water. Describe this observation in terms of heat flow. Unit 1-3 Exam Practice Page 5

6 Base your answers to questions 39 through 42 on the information below. Given the heating curve where substance X starts as a solid below its melting point and is heated uniformly: 39. Describe, in terms of particle behavior or energy, what is happening to substance X during line segment. 40. Using ( ) to represent particles of substance X, draw at least five particles as they would appear in the substance at point F. Use the box provided above. 41. Identify a line segment in which the average kinetic energy is increasing. 42. Identify the process that takes place during line segment DE of the heating curve. Unit 1-3 Exam Practice Page 6

7 Base your answers to questions 43 and 44 on the diagram below, which shows a piston confining a gas in a cylinder. 43. The gas volume in the cylinder is 6.2 milliliters and its pressure is 1.4 atmospheres. The piston is then pushed in until the gas volume is 3.1 milliliters while the temperature remains constant. a Calculate the pressure, in atmospheres, after the change in volume. Show all work. b Record your answer. 44. Sketch the general relationship between the pressure and the volume of an ideal gas at constant temperature. 45. a Calculate the heat released when 25.0 grams of water freezes at 0 C. Show all work. b Record your answer with an appropriate unit. Unit 1-3 Exam Practice Page 7

8 Base your answers to questions 46 through 48 on the graph below, which shows the vapor pressure curves for liquids A and B. 46. Which liquid will evaporate more rapidly? Explain your answer in terms of intermolecular forces. 47. At what temperature does liquid B have the same vapor pressure as liquid A at 70 C? Your answer must include correct units. 48. What is the vapor pressure of liquid A at 70 C? Your answer must include correct units. Unit 1-3 Exam Practice Page 8

9 49. A sample of water is heated from a liquid at 40 C to a gas at 110 C. The graph of the heating curve is shown below. a. On the heating curve diagram provided below, label each of the following regions: Liquid, only Gas, only Phase change b. For section QR of the graph, state what is happening to the water molecules as heat is added. c. For section RS of the graph, state what is happening to the water molecules as heat is added. Unit 1-3 Exam Practice Page 9

10 Unit 1-3 Exam Practice Page 10

11 Chemistry[Chem Un 1 to 3 practice[10/26/2014]]- Eduware Classification Total Questions: LABS AND MEASUREMENTS (8) 11.A.Labs and Measurements (6) 11.A.ii.Measurement and Equipment (5) 11.A.ii.c.Percent Error (2) 11.A.ii.b.Significant Figures / Metric Units (3) 11.A.i.Scientific Methods (1) 11.B.Constructed Response XI (2) 5.PHYSICAL BEHAVIOR OF MATTER (40) 5.F.Mixtures (8) 5.F.ii.Separation of Mixtures (3) 5.F.ii.a.Filtration (3) 5.F.i.Homogeneous / Heterogeneous (5) 5.E.Intermolecular Forces (4) 5.E.ii.Vapor Pressure and Evaporation (4) 5.D.Phase Changes (3) 5.D.v.Boiling, Evaporating, Heat of Vaporization (1) 5.D.iv.Melting, Heat of Fusion / Solid (1) 5.D.i.Heating / Cooling Curves (1) 5.C.Properties of Gases (10) 5.C.ii.Gas Laws (7) 5.C.ii.b.Combined Gas Law Problems (5) 5.C.ii.a.Avogadro's Hypothesis (2) 5.C.i.Ideal Gas Model (KMT) (3) 5.C.i.b.Real Gas Deviations (2) 5.C.i.a.Ideal Gas Theory (1) 5.B.Energy, Temperature & Entropy (3) 5.B.ii.Temperature (3) 5.B.ii.a.Average Kinetic Energy (3) 5.H.Constructed Response V (12) 6.KINETICS/EQUILIBRIUM (1) 6.E.Constructed Response VI (1)

12 Exam Question Summary Chem Un 1 to 3 practice 10/26/2014 # QID# Ans Thinking Skills Standards A.ii.c A.ii.c A.ii.b A.ii.b A.ii.b A.i F.ii.a F.ii.a F.ii.a F.i F.i F.i F.i F.i E.ii E.ii E.ii E.ii D.v D.iv D.i C.ii.b C.ii.b C.ii.b C.ii.b C.ii.b. Unit 1-3 Exam Practice Page 12

13 Exam Question Summary Chem Un 1 to 3 practice 10/26/2014 # QID# Ans Thinking Skills Standards C.ii.a C.ii.a C.i.b C.i.b C.i.a B.ii.a B.ii.a B.ii.a n/a 11.B n/a 11.B n/a 6.E n/a 5.H n/a 5.H n/a 5.H n/a 5.H n/a 5.H n/a 5.H n/a 5.H n/a 5.H n/a 5.H n/a 5.H n/a 5.H n/a 5.H. Unit 1-3 Exam Practice Page 13

14 Answer Key Chem Un 1 to 3 practice Examples: 5.88 or 5.9 or a) Examples: or, or, and accept only to the nearest tenth with a range from Proper Units: g/ml or grams per milliliter b) Range of % c) The density would increase because the sample was wet when weighed 37. (essay) 38. Examples: An endothermic process absorbs heat energy. Heat flows from the surroundings to the mixture. heat is absorbed by system 39. Examples: The potential energy of the particles increases. PE increases. KE remains the same. particles more disordered Particles are spreading farther apart. Intermolecular forces of attraction decrease Examples: or or 42. Examples: boiling vaporization liquid vapor equilibrium 43. a Example: (6.2 ml)(1.4 atm) = (3.1 ml)(p2) b a Examples: q = mhf = (25.0 g)(334 J/g) or 25.0(334) b 8350 J Unit 1-3 Exam Practice Page 14

15 Answer Key Chem Un 1 to 3 practice 46. liquid A Example: The higher vapor pressure of liquid A indicates that the intermolecular forces between its molecules are weaker, allowing the molecules to escape more readily to the vapor phase (±2) C (±10) mm Hg 49. (essay) Unit 1-3 Exam Practice Page 15

16 Question ID's in Numerical Order

17 Answer Key Chem Un 1 to 3 practice 37. a exothermic b Examples: Energy flows from the injured leg to the cold pack. Heat flows from the higher temperature (the leg) to the lower temperature (the cold pack). The cold pack absorbs heat energy from the injured leg. c The energy released from the hot pack is equal to the energy absorbed by the surroundings. The total energy of the system (the hot pack) is equal to the total energy of the surroundings. Everything else is constant. 49. b. Examples: The water molecules acquire more kinetic energy. Heat is converted to kinetic energy of the water molecules. The water molecules speed up or increase their relative motion. c. Examples: The potential energy of the water molecules increases. The water molecules change from the liquid phase to the gas phase. There is less attraction between the H2O molecules.

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