the types of questions you will have on your unit 1, …...unit 1, 2 & 3 exam practice unit 1-3...

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

Unit 1-3 Exam Practice

These 49 questions came from NYS Chemistry Regents Exams. These 49 questions are similar tothe TYPES of questions you will have on your Unit 1, 2, & 3 Chemistry Exam on Wednesday,October 29th 2014. The answer key for these 49 questions will be posted on Mr. Murdoch'sChemistry website.

1) 1.10% 2) 8.90%3) 11.0% 4) 18.9%

1. A student intended to make a salt solution with aconcentration of 10.0 grams of solute per liter ofsolution. When the student’s solution wasanalyzed, it was found to contain 8.90 grams ofsolute per liter of solution. What was the percenterror in the concentration of the solution?

1) 2)3) 4)

2. A student calculated the percent by mass of waterin a hydrate as 14.2%. A hydrate is a compoundthat contains water as part of its crystal structure.If the accepted value is 14.7%, the student'spercent error was

1) 0.086 g 2) 0.431 g3) 1003 g 4) 3870 g

3. Which mass measurement contains foursignificant figures?

1) 210.10 g + 235.100 g2) 210.100 g + 235.10 g3) 210.1 g + 235.1 g4) 210.10 g + 235.10 g

4. Expressed to the correct number of significantfigures, the sum of two masses is 445.2 grams.Which two masses produce this answer?

1) 5°C 2) 4.3°C3) 0.3°C 4) 4°C

5. The diagram below represents a Celsiusthermometer recording a certain temperature.

What is the correct reading of the thermometer?

1) conclusion 2) observation3) hypothesis 4) inference

6. During a laboratory activity, a student combinedtwo solutions. In the laboratory report, thestudent wrote “A yellow color appeared.” Thestatement represents the student’s recorded

1) water, only2) water and sand, only3) water and salt, only4) water, sand, and salt

7. When a mixture of water, sand, and salt isfiltered, what passes through the filter paper?

Unit 1, 2 & 3 Exam Practice


1) NaCl(aq) and SiO2(s)2) NaCl(aq) and C6H12O6(aq)3) CO2(aq) and NaCl(aq)4) CO2(aq) and

C6H12O6(aq)

8. Which mixture can be separated by using theequipment shown below?

1) adding water to the mixture and filtering2) adding water to the mixture and evaporating3) heating the mixture to a high temperature4) cooling the mixture to a low temperature

9. A dry mixture of KNO3 and sand could beseparated by

1) X, only 2) Z, only3) X and Y 4) X and Z

10. Given the diagrams X, Y, and Z below:

Which diagram or diagrams represent a mixtureof elements A and B?

1) distilled water 2) sugar water3) saltwater 4) rainwater

11. Which of these contains only one substance?

1) element 2) mixture3) compound 4) solution

12. Which of these terms refers to matter that couldbe heterogeneous?

1) are heterogeneous2) are homogeneous3) combine in a definite ratio4) consist of two or more substances

13. One similarity between all mixtures andcompounds is that both

1) H2O(s) 2) H2O( )3) CO2(g) 4) CO2(aq)

14. Which sample of matter is classified as asolution?

1) 22 kPa 2) 33 kPa3) 70 kPa 4) 98 kPa

15. According to Reference Table H, what is thevapor pressure of propanone at 45°C?



1) decreases2) increases3) remains the same

16. As the temperature of a liquid increases, itsvapor pressure

1) water at 20ºC 2) water at 80ºC3) ethanol at 50ºC 4) ethanol at 65ºC

17. Based on Reference Table H, which sample hasthe highest vapor pressure?

1) 100 mL at 50ºC 2) 200 mL at 30ºC3) 300 mL at 40ºC 4) 400 mL at 20ºC

18. Which sample of water has the lowest vaporpressure?

1) 539°C 2) –539°C3) 7°C 4) –7°C

19. The freezing point of bromine is

1) NaCl(s) + heat NaCl( )2) NaOH(aq) + HCl(aq) NaCl(aq) + H2O(

) + heat3) H2O( ) + heat H2O(g)4) H2O( ) + HCl(g) H3O+(aq) + Cl–(aq) +

heat

20. In which equation does the term "heat"represent heat of fusion?

1) 30°C 2) 55°C3) 90°C 4) 120°C

21. The graph below represents the heating curve ofa substance that starts as a solid below itsfreezing point.

What is the melting point of this substance?

1) 2)

3) 4)

22. A gas occupies a volume of 40.0 milliliters at20°C. If the volume is increased to 80.0milliliters at constant pressure, the resultingtemperature will be equal to

1)

2)

3)

4)

23. Which graph shows the pressure-temperaturerelationship expected for an ideal gas?

1) 144 K 2) 288 K3) 432 K 4) 576 K

24. A 3.00-liter sample of gas is at 288 K and 1.00atm. If the pressure of the gas is increased to2.00 atm and its volume is decreased to 1.50liters, the Kelvin temperature of the sample willbe



1) from 200ºC to 400ºC2) from 400ºC to 200ºC3) from 200 K to 400 K4) from 400 K to 200 K

25. Which temperature change would cause thevolume of a sample of an ideal gas to doublewhen the pressure of the sample remains thesame?

1) decreases2) increases3) remains the same

26. As the temperature of a gas increases at constantpressure, the volume of the gas

1) equal masses and the same number ofmolecules

2) different masses and a different number ofmolecules

3) equal volumes and the same number ofmolecules

4) different volumes and a different number ofmolecules

27. At the same temperature and pressure, 1.0 literof CO(g) and 1.0 liter of CO2(g) have

1) 1.0 mole 2) 1.5 moles3) 3.0 moles 4) 0.0 moles

28. A closed container holds 3.0 moles of CO2 gasat STP. What is the total number of moles ofNe(g) that can be placed in a container of thesame size at STP?

1) close and have strong attractive forcesbetween them

2) close and have weak attractive forcesbetween them

3) far apart and have strong attractive forcesbetween them

4) far apart and have weak attractive forcesbetween them

29. A real gas behaves more like an ideal gas whenthe gas molecules are

1) some volume and no attraction for eachother

2) some volume and some attraction foreach other

3) no volume and no attraction for each other4) no volume and some attraction for each

other

30. A real gas differs from an ideal gas because themolecules of real gas have

1) a definite shape and a definite volume2) a definite shape but no definite volume3) no definite shape but a definite volume4) no definite shape and no definite volume

31. Two basic properties of the gas phase are

1) concentration 2) temperature3) pressure 4) volume

32. An increase in the average kinetic energy of asample of copper atoms occurs with an increasein

1) 1°C to 10°C 2) 10°C to 1°C3) 50°C to 60°C 4) 60°C to 50°C

33. Which change in the temperature of a 1-gramsample of water would cause the greatestincrease in the average kinetic energy of itsmolecules?

1) masses2) volumes3) average kinetic energies4) numbers of molecules

34. A sealed flask containing 1.0 mole of H2(g) anda sealed flask containing 2.0 moles of He(g) areat the same temperature. The two gases musthave equal



35. A student determines the density of zinc to be7.56 grams per milliliter. If the accepted densityis 7.14 grams per milliliter, what is the student’spercent 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 ofsignificant 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 containschemicals 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 energybetween the leg and the cold pack.

c What is the Law of Conservation of Energy? Describe how the Law of Conservation ofEnergy applies to the chemical reaction that occurs in the hot pack.

38. Base your answer to the following question onthe information below.

Given the equation for the dissolving of sodiumchloride in water:

When NaCl(s) is added to water in a250-milliliter beaker, the temperature of themixture is lower than the original temperature ofthe water. Describe this observation in terms of heat flow.



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 isheated uniformly:

39. Describe, in terms of particle behavior or energy, what is happening to substance X duringline segment .

40. Using (•) to represent particles of substance X, draw at least five particles as they wouldappear 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.



Base your answers to questions 43 and 44 on thediagram below, which shows a piston confininga gas in a cylinder.

43. The gas volume in the cylinder is 6.2 millilitersand its pressure is 1.4 atmospheres. The pistonis then pushed in until the gas volume is 3.1milliliters while the temperature remainsconstant.

a Calculate the pressure, in atmospheres, afterthe change in volume. Show all work.

b Record your answer.

44. Sketch the general relationship between thepressure and the volume of an ideal gas atconstant temperature.

45. a Calculate the heat released when 25.0 gramsof water freezes at 0°C. Show all work.

b Record your answer with an appropriate unit.



Base your answers to questions 46 through 48 on the graph below, which shows the vaporpressure curves for liquids A and B.

46. Which liquid will evaporate more rapidly? Explain your answer in terms of intermolecularforces.

47. At what temperature does liquid B have the same vapor pressure as liquid A at 70°C? Youranswer must include correct units.

48. What is the vapor pressure of liquid A at 70°C? Your answer must include correct units.



49. A sample of water is heated from a liquid at 40°C to a gas at 110°C. The graph of the heatingcurve is shown below.

a. On the heating curve diagram provided below, label each of the following regions:

Liquid, onlyGas, onlyPhase change

b. For section QR of the graph, state what is happening to the water molecules as heat isadded.

c. For section RS of the graph, state what is happening to the water molecules as heat isadded.

Chemistry[Chem Un 1 to 3 practice[10/26/2014]]- Eduware Classification Total Questions: 49

11.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)

Exam Question Summary Chem Un 1 to 3 practice 10/26/2014


# QID# Ans Thinking Skills Standards1 5044 3 11.A.ii.c.2 4896 3 11.A.ii.c.3 4905 3 11.A.ii.b.4 4856 3 11.A.ii.b.5 4855 2 11.A.ii.b.6 4968 2 11.A.i.7 5022 3 5.F.ii.a.8 4940 1 5.F.ii.a.9 4858 1 5.F.ii.a.10 5197 2 5.F.i.11 5172 1 5.F.i.12 5090 2 5.F.i.13 5017 4 5.F.i.14 4819 4 5.F.i.15 5115 3 5.E.ii.16 4963 2 5.E.ii.17 4800 4 5.E.ii.18 4743 4 5.E.ii.19 5116 4 5.D.v.20 4957 1 5.D.iv.21 5048 2 5.D.i.22 5046 3 5.C.ii.b.23 4872 1 5.C.ii.b.24 4820 2 5.C.ii.b.25 4803 3 5.C.ii.b.26 4798 2 5.C.ii.b.

Exam Question Summary Chem Un 1 to 3 practice 10/26/2014


# QID# Ans Thinking Skills Standards27 5174 3 5.C.ii.a.28 4772 3 5.C.ii.a.29 5170 4 5.C.i.b.30 4802 2 5.C.i.b.31 4746 4 5.C.i.a.32 5013 2 5.B.ii.a.33 4874 3 5.B.ii.a.34 4745 3 5.B.ii.a.35 5218 n/a 11.B.36 4995 n/a 11.B.37 4922 n/a 6.E.38 5221 n/a 5.H.39 5214 n/a 5.H.40 5213 n/a 5.H.41 5212 n/a 5.H.42 5211 n/a 5.H.43 5140 n/a 5.H.44 5139 n/a 5.H.45 5137 n/a 5.H.46 5071 n/a 5.H.47 5070 n/a 5.H.48 5069 n/a 5.H.49 4987 n/a 5.H.

Answer Key

Chem Un 1 to 3 practice


1.1 2 3 4

2.1 2 3 4

3.1 2 3 4

4.1 2 3 4

5.1 2 3 4

6.1 2 3 4

7.1 2 3 4

8.1 2 3 4

9.1 2 3 4

10.1 2 3 4

11.1 2 3 4

12.1 2 3 4

13.1 2 3 4

14.1 2 3 4

15.1 2 3 4

16. 1 2 3

17.1 2 3 4

18.1 2 3 4

19.1 2 3 4

20.1 2 3 4

21.1 2 3 4

22.1 2 3 4

23.1 2 3 4

24.1 2 3 4

25.1 2 3 4

26. 1 2 3

27.1 2 3 4

28.1 2 3 4

29.1 2 3 4

30.1 2 3 4

31.1 2 3 4

32.1 2 3 4

33.1 2 3 4

34.1 2 3 4

35.Examples: 5.88or 5.9 or 6

36. a) Examples:

or,

or,

and accept only tothe nearest tenthwith a range from6.7 - 6.9

Proper Units: g/mlor grams permilliliter

b) Range of 1.8 -2.0%c) The densitywould increasebecause thesample was wetwhen weighed

37. (essay)38. Examples: –An

endothermicprocess absorbsheat energy.–Heat flows fromthe surroundingsto the mixture.–heat is absorbedby system

39. Examples: –Thepotential energy ofthe particlesincreases. –PEincreases.–KE remains thesame. –particlesmore disordered–Particles arespreading fartherapart.–Intermolecularforces of attractiondecrease.

40.

41. Examples: or or

42. Examples:–boiling–vaporization–liquid – vaporequilibrium

43. a Example: (6.2mL)(1.4 atm) =(3.1 mL)(P2)b 2.8

44.

45. a Examples: q =mHf = (25.0g)(334 J/g) or25.0(334)b 8350 J

Answer Key



46. liquid AExample:The higher vaporpressure of liquid A indicates that theintermolecularforces between itsmolecules areweaker, allowingthe molecules toescape morereadily to thevapor phase.

47. 114 (±2) °C48. 710 (±10) mm Hg49. (essay)

Question ID's inNumerical Order9. 485810. 519718. 474334. 474531. 474628. 477226. 479817. 480030. 480225. 480314. 481924. 48205. 48554. 485623. 487233. 48742. 48963. 490537. 49228. 494020. 495716. 49636. 496849. 498736. 499532. 501313. 50177. 50221. 504422. 504621. 504848. 506947. 507046. 507112. 509015. 511519. 511645. 513744. 513943. 514029. 517011. 517227. 517442. 521141. 521240. 521339. 521435. 521838. 5221

Answer Key


37. a exothermicb Examples: – Energy flows from the injured leg to the cold pack. – Heat flows from the highertemperature (the leg) to the lower temperature (the cold pack). – The cold pack absorbs heatenergy 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 kineticenergy 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 moleculeschange from the liquid phase to the gas phase. –There is less attraction between the H2Omolecules.

the types of questions you will have on your unit 1, …...unit 1, 2 & 3 exam practice unit 1-3...

Documents