Ch4 – Properties of Matter | Full Review Test Bank 15e

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Course Title: Hein 15e

Package Title: Hein 15e Test Bank

Chapter Number: 4

Question type: Multiple Choice

1) Which is not a physical property of water?

a) Water is colorless.

b) The freezing point of water is 0 ^ºC.

c) Water reacts with sodium metal to produce sodium hydroxide and hydrogen.

d) The density of water at 4 ^ºC is 1.00 g/mL.

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

2) Physical properties include all the following except:

a) boiling point

b) reactivity with other substances

c) odor

d) specific gravity

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

3) Which of the following is not a physical change?

a) melting of zinc

b) dissolving sugar in water

c) crushing of stone

d) a burning candle

Difficulty: medium

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

4) Which of the following is a chemical change?

a) iron rusting

b) water freezing

c) alcohol evaporating

d) ice melting

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

5) Which of the following is not a chemical change?

a) decomposition of water into hydrogen and oxygen gas

b) compression of oxygen gas

c) tarnishing of silver

d) charging of a cellular phone

Difficulty: medium

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

6) Which of the following is a physical change?

a) kerosene burning

b) decomposition of water by electrolysis

c) salt dissolving in water

d) converting alcohol to vinegar

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

7) Which phase change absorbs energy?

a) H₂O (l) → H₂O (g)

b) H₂O (l) → H₂O (s)

c) H₂O (g) → H₂O (l)

d) H₂O (g) → H₂O (s)

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

8) Which of the following physical changes take place by absorbing energy?

a) Melting

b) Condensation

c) Deposition

d) Freezing

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

9) Which of the following processes release energy?

a) condensation of water on a wind shield of a car

b) formation of copper (II) oxide from copper and oxygen

c) ball rolling down a hill

d) formation of ice from liquid water

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

10) A 400.0 g sample of water is at 30.0 ^ºC. How many joules of energy are required to raise the temperature of the water to 45.0 ^ºC?

a) 628 J

b) 1880 J

c) 25100 J

d) 450 J

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

11) How many joules of energy are required to raise the temperature of 150.0 g of water from 15.0 ^ºC to 45.0 ^ºC?

a) 4500 J

b) 18800 J

c) 25400 J

d) 6590 J

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

12) How many joules of energy are required to cook an omelet in a 5.0 kg iron skillet that was heated from 25.0 ^ºC to 150.0 ^ºC? (The specific heat of iron is 0.452 J/g ^ºC)

a) 280 J

b) 5100 J

c) 280000 J

d) 1400 J

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

13) A 100. g iron rod is heated to an unknown initial temperature. While cooling down to a temperature of 25.0 ^ºC, the rod releases 600.2 J of energy. What was its initial temperature? (The specific heat of iron is 0.452 J/g ^ºC)

a) 38.3 J

b) 11.7 J

c) 27.7 J

d) 22.3 J

Difficulty: Medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

14) How many joules of energy are released when 45.0 g of water cools from 18.0 ^ºC to 7.0 ^ºC?

a) 495 J

b) 791 J

c) 2860 J

d) 2070 J

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

15) How many joules of energy are released when 100.0 g of water cools from 98.0 ^ºC to 20.0 ^ºC?

a) 32600 J

b) 33800 J

c) 167 J

d) 7800 J

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

16) How many kilojoules of energy are required to bring 800.0 g water from 20.0⁰C to the boiling point?

a) 268 kJ

b) 2.68 × 10⁸ kJ

c) 3.35 × 10⁵kJ

d) 3.35 × 10⁸kJ

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

17) How many kilojoules of energy are released when .1.60 kg of water cools from 80.0 ^ºC to 60.0 ^ºC?

a) 32.0 kJ

b) 382 kJ

c) 515 kJ

s) 134 kJ

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

18) 15.6 g of a metal absorbs 836.8 J of heat energy that raises its temperature by 21 ^ºC. What is the specific heat of the metal?

a) 620 J

b) 1100 J

c) 0.39 J

d) 2.6 J

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

19) 400.0 g of a metal absorbs 10000. J of heat energy and its temperature rises from 20.0 ^ºC to 103.0 ^ºC. What is the specific heat of the metal?

a) 0.301 J/g^ºC

b) 0.255 J/g^ºC

c) 3.32 J/g ^ºC

d) 0.243 J/g^ºC

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

20) 250.0 g of a metal releases 5000. J of energy and its temperature drops from 90.0 ^ºC to 15.7 ^ºC. What is the specific heat of the metal?

a) 3.72 J/g^ºC

b) 0.269 J/g^ºC

c) 0.222 J/g^ºC

d) 1.27 J/g ^ºC

Difficulty: medium

Learning Objective 1: Define a hydrocarbon compound and explain their role in the world’s energy supply.

Section Reference 1: Section 4.6

21) 300.0 g of water is at 12.0 ^ºC. The water absorbs 4016 J of heat energy. What is the new temperature of the water?

a) 3.2 ^ºC

b) 15.2 ^ºC

c) 8.8 ^ºC

D) 13.1 ^ºC

Difficulty: hard

Learning Objective 1: Define a hydrocarbon compound and explain their role in the world’s energy supply.

Section Reference 1: Section 4.6

22) 45.0 g of water is at 20.0 ^ºC. The water releases 2000. J of energy as heat. What is the new temperature of the water in Kelvin?

a) 19.9K

b) 30.6 K

c) -168K

d) 282K

Difficulty: hard

Learning Objective 1: Define a hydrocarbon compound and explain their role in the world’s energy supply.

Section Reference 1: Section 4.6

23) A sample of water absorbs 3.00 × 10³ J of heat energy and its temperature rises from 20.0 ^ºC to 31.2 ^ºC. What is the mass of the water?

a) 3.21 g

b) 64.0 g

c) 3.58 g

d) 1120 g

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

24) A sample of water releases 4.50 × 10³ J of heat energy and its temperature drops from 80.0^ºC to 68.0^ºC. What is the mass of the water?

a) 89.6 g

b) 13.4 g

c) 15.8 g

d) 1570 g

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

25) Hydrogen combines with oxygen to form water. If 1.67 g of hydrogen completely combines with 13.33 g of oxygen what mass of water will be produced?

a) 1.67 g

b) 11.66 g

c) 13.33 g

d) 15.00 g

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

26) A 20. g sample of solid carbon and 127 g of oxygen gas burn to form 73 g of pure carbon dioxide. If no other products are formed and all of the carbon is reacted, what is the mass of the unreacted oxygen?

a) 54 g

b) 49 g

c) 74 g

d) 99 g

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

27) 12.0 g of solid carbon reacts with 4.0 g of elemental hydrogen to produce natural gas. How much carbon and hydrogen are needed to make 100. g of natural gas?

a) 75 g of carbon and 25 g of hydrogen

b) 25 g of carbon and 75 g of hydrogen

c) 60 g of carbon and 40 g of hydrogen

d) 80 g of carbon and 20 g of hydrogen

Difficulty: medium

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

28) 3.17 g of sodium combines completely with chlorine to form 8.00 g of sodium chloride. What is the mass of chlorine in this sample of sodium chloride?

a) 3.17 g

b) 4.83 g

c) 8.00 g

d) 11.17 g

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

29) A sample of carbon monoxide has a mass of 4.00 g. What is the mass of oxygen in this compound if the mass of carbon is 1.71 g?

a) 1.71 g

b) 2.29 g

c) 0.59 g

d) 5.71 g

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

30) A compound is decomposed into its constituent elements carbon, hydrogen and oxygen. If on decomposition, 6.0 g of carbon, 3.0 g of hydrogen and 8.0 g of oxygen were formed, what was the mass of the compound before it was decomposed?

a) 17 g

b) 9.0 g

c) 14 g

d) 140 g

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

31) Which is not a physical property?

a) boiling point

b) physical state

c) color

d) bleaching action

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

32) Which is not a physical property?

a) Grinding

b) Crushing

c) Fizzing

d) boiling

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

33) Which of the following is a physical change?

a) a piece of wood is burned

b) a nail rusts

c) a rubber band is stretched

d) a firecracker explodes

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

34) Which of the following is a chemical change?

a) water evaporates

b) a penny tarnishes

c) ice melts

d) rock is ground into sand

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

35) Which is not a chemical property?

a) burning

b) rusting

c) Freezing

d) reactivity with water

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

36) Combining hydrogen gas and oxygen gas to form water is a

a) chemical change.

b) physical change.

c) conservation reaction.

d) none of these choices

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

37) To heat 60.0 g of water from 30.0 ^ºC to 50.0 ^ºC requires

a) 5.02 kJ.

b) 7.53 kJ.

c) 12.6 kJ.

d) 6.28 kJ.

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

38) Quantity of heat needed to raise the temperature of 65 mL of water in a water heater from 20.0 ^oC to 65.0 ^oC is ___. Assume density of water equals 1.00 g/mL

a) 2.9 kJ

b) 12 kJ

c) 18 kJ

d) 23 kJ

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

39) The specific heat of aluminum is 0.900 J/g ^ºC. How much energy is required to heat 45.0 g of aluminum from 20.0 ^ºC to 50.0 ^ºC?

a) 2840 J

b) 1220 J

c) 810. J

d) 2030 J

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

40) The specific heat of iron is 0.473 J/g^ºC. How much energy is required to heat a 40.0 g sample of iron from 35.0 ^ºC to 75.0 ^ºC?

a) 757 J

b) 2080 J

c) 6690 J

d) 1320 J

Difficulty: easy

Learning Objective 1: Define a hydrocarbon compound and explain their role in the world’s energy supply.

Section Reference 1: Section 4.6

41) An unknown piece of a metal weighing 123 g is placed in boiling water and after a few minutes is plunged into 75 mL of water at 25.0 ^oC. If the final temperature of the metal and water is 29.0 ^oC, what is the specific heat capacity of the metal? (Assume that the density of water is 1.0 g/mL and specific heat capacity of water is 4.184 J/g^oC.)

a) 0.14 J/g^oC

b) 0.23 J/g^oC

c) 1.6 J/g^oC

d) 3.6 J/g^oC

Difficulty: hard

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

42) The specific heat of iron is 0.473 J/g^ºC. A 400.0g sample of iron at 20.0^ºC releases 2270.4 J of heat energy. What is the new temperature of the iron?

a) 8.0 ^ºC

b) 12.0^ºC

c) 20.0 ^ºC

d) 32.0 ^ºC

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

43) The quantity of heat required to raise the temperature of 1.0 gram of a substance by 1 °C is called

a) heat capacity.

b) specific heat.

c) heat activity.

d) energy activity.

Difficulty: easy

Learning Objective 1: List the basic steps involved in solving chemistry problems.

Section Reference 1: Section 4.3

44) Energy that matter possesses due to its position is called

a) potential energy.

b) potential motion.

c) kinetic motion.

d) kinetic energy.

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

45) Which of the following is a chemical change?

a) ice melts

b) alcohol evaporates

c) a rock is ground into sand

d) silver tarnishes

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

46) Which of the following is a chemical property of chlorine?

a) It has a sharp suffocating odor.

b) It is a yellowish-green gas.

c) It boils at –34.6^ºC.

d) It combines with sodium to form sodium chloride.

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

47) An example of a physical property is:

a) TNT is explosive

b) gasoline is flammable

c) zinc reacts with hydrochloric acid to produce hydrogen gas

d) none of these choices

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

48) According to the law of conservation of energy, energy can be ___.

a) created

b) destroyed

c) created and destroyed

d) converted from one form to another

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

49) The specific heat of iron is 0.473 J/g^ºC and the specific heat of lead is 0.128 J/g^ºC. In order to raise the temperature of one gram of those metals by one degree Celsius,

a) both metals require the same amount of energy.

b) the iron requires more energy than the lead.

c) the lead requires more energy than the iron.

d) no correct answer is given

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

50) What is the specific heat of a solid that requires 124 J of heat to raise the temperature of 95.5 g of the substance from 20.0 ^ºC to 25.0 ^ºC?

a) 2.6 J/g^ºC

b) 0.26 J/g^ºC

c) 1.4 J/g^ºC

d) 5.9 × 10⁴ J/g^ºC

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

51) How many joules of energy are absorbed when 250.g of lead, specific heat is 0.128 J/g^ºC, are heated from 25 ^ºC to 245 ^ºC?

a) 800. J

b) 7040 J

c) 7840 J

d) 8640 J

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

52) Which of the following illustrates an increase in potential energy?

a) a firecracker explodes

b) a person climbs a set of stairs

c) a wind-up toy winding down

d) an apple dropping from a tree

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

53) The change of vapors into ice is a

a) chemical change.

b) physical change.

c) heterogeneous change.

d) homogeneous change.

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

54) When 20.0 g of mercury is heated from 10.0 ^ºC to 20.0 ^º, 27.6 J of energy are absorbed. What is the specific heat of mercury?

a) 0.725 J/g^ºC

b) 0.138 J/g^ºC

c) 2.76 J/g^ºC

d) None of these answer choices are correct.

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

55) A 400.0 g metal bar requires 6.446 kJ of energy to change its temperature from 18.0 ^ºC to 95.0 ^ºC. What is the specific heat of the metal?

a) 0.895 J/g^ºC

b) 161 J/g^ºC

c) 2.09 × 10^–4 J/g^ºC

d) 0.209 J/g^ºC

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

56) A shiny silver colored strip of metal is heated in a hot flame. It turns powdery and white. When the flame is removed and the strip cools it remains powdery white. What can you conclude from these observations?

a) All metals oxidize with heat.

b) The metal strip has undergone a physical change.

c) All physical changes require heat.

d) The strip has undergone a chemical change.

Difficulty: medium

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

57) One joule is equal to ___.

a) 4.814 cal

b) 1.000 cal

c) 0.239 cal

d) 0.513 cal

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

58) A sample of an unknown substance was tested in a laboratory. The sample could not be decomposed by chemical or physical means. Based on these results, the laboratory reported that the sample was most likely a(n) ___.

a) compound

b) element

c) solution

d) mixture

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

59) Which of the following terms represents a form of energy?

a) degree

b) joule

c) temperature

d) heat

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

60) What is the SI unit for energy?

a) calorie

b) joule

c) kilojoule

d) kilocalorie

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

61) How many kilojoules of heat energy are required to raise the temperature of 400.0g of water from 18.0^ºC to 25.0 ^ºC?

a) 12000 kJ

b) 12 kJ

c) 30. KJ

d) 42 kJ

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

62) As Kelvin temperature decreases, the average kinetic energy of the particles in a sample ___.

a) increases

b) decreases

c) remains the same

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

63) The specific heat of copper is 0.386 J/g^ºC. A 20.0 g sample of copper is heated from 25.0 ^ºC to 35.0 ^ºC. How much heat did the copper absorb?

a) 837 J

b) 77.2 J

c) 194 J

d) 270 J

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

64) The specific heat of zinc is 0.388 J/g^ºC. A 700.0 g sample of zinc at 35.0 ^ºC absorbs 2.336 kJ of heat. What is the final temperature of the zinc?

a) 8.6 ^ºC

b) 26.4 ^ºC

c) 43.6 ^ºC

d) 301 ^ºC

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

65) A 25.0 g sample of magnesium at 22.0 ^ºC absorbs 356.3 J of heat. The temperature of the magnesium rises to 36.5 ^ºC. What is the specific heat of the magnesium?

a) 0.648 J/g^ºC

b) 0.390 J/g^ºC

c) 0.444 J/g^ºC

d) 0.983 J/g^ºC

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

66) Given the following list for a metal:
Melting point= 1600 ºC

Density= 9.8 g/mL

Volume= 35 mL

Mass= 89.g

How many of the above can be used to characterize this metal?

a) 4

b) 3

c) 2

d) 1

Difficulty: medium

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

67) The following list represents properties of iron metal:
atomic mass = 55.85 amu

density = 7.87 g/cm³

melting point = 1538 ºC

undergoes oxidation in moist air

How many of these are physical properties?

a) four

b) three

c) two

d) one

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

68) Which of the following represents a physical change?

a) CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(l)

b) AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq)

c) N₂(g) + 3 H₂(g) → 2 NH₃(g)

d) H₂O(s) → H₂O(l)

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

69) In the reaction
16 H⁺(aq) + 10 (aq) + 2 (aq) → 5 Br₂(l) + 2 Mn²⁺(aq) + 8 H₂O(l)

The reactants are:

a) H⁺(aq), Br^–(aq), MnO₄^–(aq)

b) Br₂(l) , Mn²⁺(aq), H²O(l)

c) H⁺(aq), H₂O(l)

d) Br^–(aq), MnO₄^–(aq)

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

70) In the reaction
Ag(s) + 2 HNO₃(aq) → AgNO₃(aq) + NO(g) + H₂O(l)

The products are:

a) Ag(s), HNO₃(aq)

b) AgNO₃(aq), NO(g), H₂O(l)

c) AgNO₃(aq), NO(g)

d) HNO₃(aq), H₂O(l)

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

71) Select the alternative that represents a physical change.
a)

b)

c)

d)

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

72) Select the alternative that represents a chemical change.
a)

b)

c)

d)

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

73) An iron pin (specific heat = 0.473 ) at 110°C is dropped into 50.0 mL of H₂O at 15.0°C. After a couple of minutes, the temperature of the water reaches 17.4°C. What was the mass of the iron pin?

a) 44 g

b) 15 g

c) 1.3 g

d) 11 g

Difficulty: hard

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

74) Which of the following processes would have a change in potential energy as shown below?

a) melting chocolate

b) boiling water

c) burning gasoline

s) frying bacon

Difficulty: hard

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

75) What mass of water at 10.0°C is needed to cool 500.0 mL of tea from 25.0°C to 18.3°C? Assume that density and specific heat of the tea are the same as water.

a) 4.0 × 10² g

b) 2.2 × 10² g

c) 1.1 × 10³ g

d) 6.2 × 10² g

Difficulty: hard

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

76) What will be the final temperature of a system in which 150.0 g of water at 5.0 °C are added to 1.00 L of water at 90.5 °C?

a) 106 °C

b) 5.57 °C

c) 79.3 °C

d) 82.8 °C

Difficulty: hard

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

77) Assume equal masses of the following substances, all of them at 20.0°C and exposed to the same source of heat simultaneously. Which substance will reach a temperature of 35.0°C faster?

a) aluminum

b) lead

c) titanium

d) tin

Difficulty: hard

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

78) Assume equal masses of the following substances, all of them at 20.0°C and exposed to the same source of heat simultaneously. Which substance will take the longest time to heat up to 35.5°C?

a) aluminum

b) lead

c) titanium

d) tin

Difficulty: hard

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

79) A microwave oven supplies 1.000 kJ per second. How many minutes should be set on the microwave in order to heat 250. g of water from 24.3 °C to its boiling point?

a) 2.54 minutes

b) 1.32 minutes

c) 79.2 minutes

s) 0.424 minutes

Difficulty: hard

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

Question type: True/False

80) In a physical change new substances are formed.

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

81) One calorie equals 0.234 joule.

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

82) Melting and boiling are examples of physical changes.

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

83) Rusting and combustion are examples of chemical changes.

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

84) Temperature and heat are two forms of kinetic energy.

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

85) When chemical reactions occur, energy is always absorbed.

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

86) The correct SI unit for energy is the calorie.

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

87) Color, taste, odor, density, and boiling point are all physical properties.

Difficulty: easy

Learning Objective 1: Compare the physical and chemical properties of a substance.

Section Reference 1: Section 4.1

88) When water boils it is converted into hydrogen and oxygen.

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

89) Steam condenses into water is a chemical change.

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

90) Kinetic energy is the energy matter possesses due to its motion.

Difficulty: easy

Learning Objective 1: List the various forms of energy, explain the role of energy in chemical changes and state the law of conservation of energy.

Section Reference 1: Section 4.4

91) When 0.5 grams of sugar are dissolved in water, a chemical change takes place.

Difficulty: medium

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

92) Dry ice undergoing sublimation is an example of a physical change.

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

93) Milk turn sour is an example of a physical change.

Difficulty: easy

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

94) If the temperature of a system increases as a result of a chemical or physical change, then the system has absorbed energy.

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Question type: Essay

95) A sample of metal with a mass of 54.3 g at 100.0 ^ºC is dropped into 175.0 g of water at 25.3 ^ºC. The temperature of the water rises to 27.1 ^ºC. Assume there is no heat lost to the environment.
a) What is the amount of heat gained by the water?
b) What is the specific heat of the metal?

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Solution: a) 1300J; b) 0.33 J/g^ºC

96) A sample of metal with a mass of 350.0 g is heated to 100.0 ^ºC and dropped into 400.0 g of water at 21.4 ^ºC. The temperature of the water rises to 28.0 ^ºC. Assume there is no heat lost to the environment.
a) What is the amount of heat gained by the water?
b) What is the specific heat of the metal?

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Solution: a) 11000J; b) 0.438 J/g^ºC

97) A sample of metal with a mass of 650.0 g is heated to 98.0 ^ºC and dropped into 500.0 g of water at 28.4 ^ºC. The water temperature rises to 39.0 ^ºC. Assume there is no heat lost to the environment.
a) What is the amount of heat gained by the water?
b) What is the specific heat of the metal?

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Solution: a) 22.2 kJ; b) 0.578 J/g^ºC

98) A sample of metal with a mass of 28.5 g is heated to 151.7 ^ºC and dropped into 150.0 g of water at 22.0 ^ºC. The water temperature rises to 24.2 ^ºC. Assume there is no heat lost to the environment.
a) What is the amount of heat gained by the water?
b) What is the specific heat of the metal?

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Solution: a) 1400 J; b) 0.39 J/g^ºC

99) The specific heat of gold is 0.131 J/g^ºC. A 400.0 g sample of gold at 350.0 ^ºC is dropped into 180.0 g of water at 22.0 ^ºC. Assume no heat is lost to the environment.
a) What will be the final temperature of the water?
b) What will be the final temperature of the gold?

Difficulty: hard

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Solution: a) 43.3^ºC; b) 43.3^ºC

100) The specific heat of aluminum is 0.900 J/g^ºC. A 300.0 g sample of aluminum at 300.0 ^ºC is dropped into 200.0 g of water at 20.0 ^ºC. Assume no heat is lost to the environment.
a) What will be the final temperature of the water?

b) What will be the final temperature of the aluminum?

Difficulty: hard

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Solution: a) 88.3^ºC; b) 88.3^ºC

101) A 50.0 ml solution of sodium hydroxide is at 22.0 ^ºC. The solution has a density of 1.10 g/mL and a specific heat of 4.10 J/g^ºC. The solution absorbs 1.876 kJ of heat energy.
a) How many degrees Celsius will the temperature of the solution rise?

b) What will be the final temperature of the solution?

Difficulty: hard

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Solution: a) 8.32 ^ºC; b) 30.3 ^ºC

102) If 100.0 g of a fuel can raise the temperature of 8.00 L of water from 22.0 ^ºC to 98.0 ^ºC, how much heat is given off by 1.00 g of the fuel?

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Solution: 25400 J or 25.4 kJ

103) A 25.0 g sample of lead, specific heat = 0.128 J/g^ºC, was warmed from 35.0 ^ºC to 200.0 ^ºC. The same amount of heat energy was absorbed by a 60.0 g sample of copper, specific heat = 0.385 J/g^ºC, at 35.0 ^ºC. What is the final temperature of the copper?

Difficulty: medium

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Solution: 57.9^ºC

104) Compare a substance with a high specific heat to a substance with low specific heat with respect to ability to absorb or release heat.

Difficulty: easy

Learning Objective 1: Calculate the amount of heat lost or gained in a given system.

Section Reference 1: Section 4.5

Solution: The substance with the higher specific heat will have less of a temperature increase when absorbing the same amount of energy as the substance with the lower specific heat. This is because the substance with the higher specific heat requires more energy to change the temperature of one gram of substance one degree Celsius. The substance with the higher specific heat will have less of a temperature decrease when releasing the same amount of energy as the substance with the lower specific heat. This is because the substance with the higher specific heat must lose more energy to change the temperature of one gram of substance one degree Celsius.

105) Explain what happens at the molecular level when water freezes.

Difficulty: hard

Learning Objective 1: Compare physical and chemical changes in a substance.

Section Reference 1: Section 4.2

Solution: Freezing occurs because energy is removed (i.e. lowering of the temperature) from the system, in this case water. As a result of the removal of energy from the individual water molecules, their motion is slowed down enough to allow for them to experience stronger interactions, which are experienced in the solid phase.