A Very Brief History Of Chemistry Test Bank Answers Ch0

Chemistry: Molecular Nature of Matter, 8e (Jespersen)

Chapter 0 A Very Brief History of Chemistry

1) Which of the following is the logical progression of elements formed in a star?

A) Hydrogen → Helium → Argon → Carbon

B) Hydrogen → Helium → Carbon → Argon

C) Helium → Hydrogen → Argon → Carbon

D) Helium → Hydrogen → Carbon → Argon

E) Argon → Carbon → Helium → Hydrogen

Diff: 2

Section: 0.2

2) Why is iron the heaviest element formed in a star prior to the formation of a supernova?

A) The formation of iron in a star starts a cooling process of the star, ending nucleosynthesis.

B) Iron reacts with the hydrogen in stars to cause a violet explosion that leads to a super nova.

C) Iron is the heaviest element that is stable at high temperatures; all others are radioactive.

D) The formation of iron in a star causes a reaction with helium that causes nucleosynthesis to end.

E) When iron is formed in the outer layers of a star, the iron has enough kinetic energy to leave the gravity of the star.

Diff: 1

Section: 0.2

3) One would expect a fairly even distribution of elements on the earth; instead, the distribution is uneven. Which of the following best describes why we observe this?

A) The nebula that formed the earth had elements that were not evenly distributed.

B) Winds on the surface of the earth have moved the heavy and light elements into bands.

C) The early earth liquefied, resulting in heavier elements migrating toward the core and lighter elements moving toward the surface. This migration to the surface was largely by lava flows, which were inconsistent.

D) Some water-soluble elements were washed by water into pockets on the surface.

E) The magnetic properties of the core caused the metals to pool into certain areas between the poles on the earth.

Diff: 2

Section: 0.2

4) The relative number of atoms of each element in a particular compound

A) is always l:l.

B) is the same as the density ratio.

C) is the same as the weight ratio.

D) is definite and constant.

E) cannot be determined experimentally.

Diff: 2

Section: 0.3 (was 0.2)

5) Which of the following postulates from Dalton's atomic theory are now considered incorrect?

I. All atoms of a given element are identical.

II. Matter consists of very small particles known as atoms.

III. Atoms are indestructible and indivisible.

A) III only

B) II only

C) I only

D) I and II

E) I and III

Diff: 1

Section: 0.4

6) Which of the following statements is/are consistent with Dalton's atomic theory?

I. The atoms in a given sample of an element do not share any common properties.

II. Matter consists of particles called atoms.

III. In chemical reactions, atoms merely rearrange and do not disintegrate.

A) III only

B) II only

C) I only

D) II and III

E) I and III

Diff: 2

Section: 0.5 (was 0.4)

7) Which of the following statements is/are NOT consistent with Dalton's atomic theory?

I. The atoms in a given sample of an element do not share any common properties.

II. Matter consists of tiny particles called molecular substances.

III. In chemical reactions, atoms merely rearrange and do not disintegrate.

A) III only

B) II only

C) I only

D) II and III

E) I and II

Diff: 2

Section: 0.4

8) Which of the following postulates from Dalton's atomic theory is incorrectly stated?

A) The atoms in a given sample of an element are identical.

B) Matter consists of tiny particles called atoms.

C) In chemical reactions, atoms merely rearrange and do not disintegrate.

D) In a given chemical compound, the atoms can be present in various numerical ratios.

E) The atoms of different elements differ in mass and other properties.

Diff: 2

Section: 0.4

9) Which of the following is consistent with the postulates from Dalton's atomic theory?

A) The atoms in a given sample of an element are not necessarily identical.

B) Matter consists of tiny particles called ions.

C) In chemical reactions, atoms both rearrange and disintegrate in smaller subatomic particles.

D) The atoms of different elements can be identical in mass and other properties.

E) In a given chemical compound, the atoms are always present in the same fixed numerical ratio.

Diff: 2

Section: 0.4

10) Which one of the statements below is true?

A) When two atoms combine to form a chemical compound, they do so in many different proportions by mass.

B) When two different compounds combine to form an element, they do so in definite proportions by mass.

C) When two different elements combine to form a chemical compound, they do so in definite proportions by mass.

D) When two molecules combine in a chemical reaction, a number of different elements can be generated depending on the masses used.

E) When two different elements combine to form a mixture, they do so in definite proportions by atomic number.

Diff: 2

Section: 0.4

11) Which one of the statements below is false?

A) In chemical reactions, atoms are rearranged.

B) In a given compound, the atoms are always present in the same fixed numerical ratio.

C) Matter is made up of tiny particles called atoms.

D) In a sealed reaction flask, the total mass after the reaction is over, is the same as before the reaction started.

E) When hydrogen and oxygen react to form water, the mass of oxygen atoms is equal to the mass of hydrogen atoms.

Diff: 1

Section: 0.4

12) Which of the following examples is consistent with the postulates from Dalton's atomic theory?

Hint: Be sure to keep the definitions of atoms and molecules straight!

A) The atoms in a sample of chlorine are similar to the atoms in a sample of elemental sulfur.

B) Matter consists of extremely tiny particles that are always either positively or negatively charged.

C) When water is formed from oxygen and hydrogen molecules, the atoms in water are grouped differently compared to the atoms in molecules of hydrogen and oxygen.

D) A sample of water contains hydrogen and oxygen atoms combined in two different ratios by mass.

E) There are eight different types of sulfur atoms in any naturally occurring sample of elemental sulfur.

Diff: 2

Section: 0.4

13) To form hydrogen sulfide, H2S, 4.03 g of molecular hydrogen (H2) are reacted with 62.13 g of sulfur (S). If all of the hydrogen and sulfur completely react to form hydrogen sulfide, how many grams of hydrogen sulfide should be formed?

A) 66.16 g

B) 58.10 g

C) 4.03 g

D) 70.19 g

E) 33.03 g

Diff: 3

Section: 0.4

14) Which of these scientists developed the atomic theory?

A) John Dalton

B) J. J. Thomson

C) Robert Millikan

D) Henry Moseley

E) Ernest Rutherford

Diff: 1

Section: 0.4

15) When J. J. Thomson discovered the electron, what physical property of the electron did he measure?

A) charge

B) charge-to-mass ratio

C) temperature

D) mass

E) atomic number

Diff: 1

Section: 0.4

16) Which one of the following contributes to the charge of an atom, but does NOT contribute significantly to the mass of an atom?

A) electrons

B) nuclei

C) photons

D) neutrons

E) protons

Diff: 2

Section: 0.5 (was 0.4)

17) Which of the following have roughly the same mass?

A) a proton and an electron

B) a neutron and an electron

C) a neutron and a proton

D) an electron and an alpha particle

E) none of these options

Diff: 1

Section: 0.5

18) Which of the following have opposite electric charges?

A) a proton and an electron

B) a neutron and an electron

C) a neutron and a proton

D) an electron and an alpha particle

E) none of these options

Diff: 1

Section: 0.5

19) Consider the atoms of 65Cu and 65Zn. Both of these atoms have the same

A) number of electrons.

B) atomic mass.

C) number of neutrons.

D) mass number.

E) number of protons.

Diff: 1

Section: 0.5

20) Which of the following particles will not be deflected by charged plates?

A) hydrogen atoms

B) cathode rays

C) alpha particles

D) protons

E) These are all deflected by charged plates.

Diff: 2

Section: 0.5

21) Uranium exists in nature in the form of several isotopes and the different isotopes have different

A) atomic numbers.

B) charges.

C) numbers of electrons.

D) numbers of neutrons.

E) numbers of protons.

Diff: 2

Section: 0.5

22) Two isotopes of an element differ only in their

A) symbol.

B) atomic number.

C) mass number.

D) number of protons.

E) number of electrons.

Diff: 1

Section: 0.5

23) Which answer below best describes all atoms of a given isotope of a particular element?

A) They possess the same mass but their other properties differ.

B) They possess similar chemical properties and the same mass but have nothing else in common.

C) They possess the same atomic number but have nothing else in common.

D) They possess the same number of electrons, the same atomic number, and similar chemical properties but differ in their masses.

E) They possess the same number of electrons, the same atomic number, the same mass, and the same chemical properties.

Diff: 1

Section: 0.5

24) Which answer below best describes all atoms of a particular element?

A) They possess the same number of electrons, the same atomic number, and the same mass, but have nothing else in common.

B) They possess the same mass and the same chemical properties but have nothing else in common.

C) They possess the same number of electrons and the same atomic number but may differ in mass.

D) They possess the same number of electrons, chemical properties, and mass but have nothing else in common.

E) They possess the same atomic number and the same mass but have nothing else in common.

Diff: 2

Section: 0.5

25) The species shown below that has 24 neutrons is

A) Cr

B) Mn

C) Mg

D) Sc

E) V

Diff: 2

Section: 0.5

26) The species shown below that has 24 electrons is

A) Cr

B) Mn

C) Mg

D) Sc

E) V

Diff: 2

Section: 0.5

27) The species V has the same number of neutrons as

A) V

B) Sc

C) Mn

D) Cr

E) Co

Diff: 2

Section: 0.5

28) Consider the atoms of Mg and Al. Both of these species have the same

A) number of neutrons and electrons.

B) number of ions.

C) number of neutrons.

D) number of neutrons and mass number.

E) number of protons and electrons.

Diff: 2

Section: 0.5

29) Consider the atoms of 59Co and 60Co. Both of these atoms have the same

A) number of neutrons and electrons.

B) number of neutrons and ions.

C) mass number.

D) number of photons.

E) number of protons and electrons.

Diff: 2

Section: 0.5

30) An atom of the isotope sulfur-33 consists of how many protons, neutrons, and electrons? (p = proton, n = neutron, e = electron)

A) 15 p, 18 n, 15 e

B) 16 p, 17 n, 16 e

C) 33 p, 16 n, 33 e

D) 16 p, 16 n, 33 e

E) 16 p, 33 n, 16 e

Diff: 2

Section: 0.5

31) An ion of the isotope chlorine-35 has an ionic charge of 1-. How many protons, neutrons, and electrons does it contain? (p = proton, n = neutron, e = electron)

Hint: Consider how changes in the number of electrons versus the number of protons affects the ionic charge of an ion.

A) 17 p, 35 n, 17 e

B) 17 p, 17 n, 35 e

C) 18 p, 17 n, 18 e

D) 17 p, 18 n, 18 e

E) 35 p, 17 n, 18 e

Diff: 2

Section: 0.5

32) Compare Mg and Al. In what respect do these species differ?

I. number of neutrons and number of electrons

II. number of protons, and number of neutrons

III. mass number and number of protons

A) I only

B) II only

C) III only

D) I and III

E) I, II, and III

Diff: 3

Section: 0.5

33) A neutral iodine atom has an atomic mass number = 131. Which description below fits this atom?

A) 39 protons, 78 neutrons, 39 electrons

B) 53 protons, 78 neutrons, 53 electrons

C) 52 protons, 79 neutrons, 54 electrons

D) 53 protons, 131 neutrons, 53 electrons

E) 54 protons, 131 neutrons, 54 electrons

Diff: 2

Section: 0.5

34) Which description below fits the atom?

Hint: Remember how charge alters the number of electrons.

A) 29 protons, 65 neutrons, 29 electrons

B) 29 protons, 36 neutrons, 65 electrons

C) 29 protons, 36 neutrons, 31 electrons

D) 29 protons, 36 neutrons, 27 electrons

E) 31 protons, 34 neutrons, 29 electrons

Diff: 2

Section: 0.5

35) Which description below fits the 112Cd atom?

A) 48 protons, 64 neutrons, 48 electrons

B) 48 protons, 62 neutrons, 48 electrons

C) 48 protons, 64 neutrons, 46 electrons

D) 48 protons, 62 neutrons, 46 electrons

E) 50 protons, 64 neutrons, 48 electrons

Diff: 2

Section: 0.5

36) The atomic mass of naturally occurring iron, which is a mixture of isotopes, is listed as . This means that the average mass of iron is

A) 55.847 times as great as that of a 12C atom.

B) 55.847 times as great as that of a 1H atom.

C) 55.847/1.0079 times as great as that of a 1H atom.

D) 55.847/12.000 times as great as that of a 12C atom.

E) 55.847/12.011 times as great as that of a 12C atom.

Diff: 2

Section: 0.5

37) The atomic mass of naturally occurring nickel, which is a mixture of isotopes, is listed as 58.6934 u. This means that the average mass of nickel is

A) 58.6934 times as great as that of a 12C atom.

B) 58.6934 times as great as that of a 1H atom.

C) 58.6934/1.0079 times as great as that of a 1H atom.

D) 58.6934/12.000 times as great as that of a 12C atom.

E) 58.6934/12.011 times as great as that of a 12C atom.

Diff: 2

Section: 0.5

38) The atomic mass of naturally occurring silver, which is a mixture of two isotopes, is listed as 107.868 u. This means that

Hint: Individual atoms have a mass number that is the sum of the protons and neutrons.

A) all silver atoms found in nature have a mass that is 107.868/12.000 times as great as that of a 12C atom.

B) all silver atoms found in nature have a mass that is 107.868/1.0079 times as great as that of a 1H atom.

C) some silver atoms found in nature have a mass that is 107.868/12.000 times as great as that of a 12C atom.

D) some silver atoms found in nature have a mass that is 107.868/1.0079 times as great as that of a 1H atom.

E) no silver atoms found in nature has a mass that is 107.868/12.000 times as great as that of a 12C atom.

Diff: 2

Section: 0.5

39) The atomic mass of naturally occurring copper, which is a mixture of two isotopes, is listed as 63.546 u. This means that

Hint: Individual atoms have a mass number which is the sum of the protons and neutrons.

A) all copper atoms found in nature have a mass that is 63.546/12.000 times as great as that of a 12C atom.

B) all copper atoms found in nature have a mass that is 63.546/1.0079 times as great as that of a 1H atom.

C) some copper atoms found in nature have a mass that is 63.546/12.000 times as great as that of a 12C atom.

D) some copper atoms found in nature have a mass that is 63.546/1.0079 times as great as that of a 1H atom.

E) no copper atoms found in nature has a mass that is 63.546/12.000 times as great as that of a 12C atom.

Diff: 3

Section: 0.5

40) The atomic mass of naturally occurring gallium, which is a mixture of two isotopes, is listed as 69.723 u. This means that

Hint: Individual atoms have a mass number that is the sum of the protons and neutrons.

A) all gallium atoms found in nature have a mass that is 69.723/12.000 times as great as that of a 12C atom.

B) all gallium atoms found in nature have a mass that is 69.723/1.0079 times as great as that of a 1H atom.

C) some gallium atoms found in nature have a mass that is 69.723/12.000 times as great as that of a 12C atom.

D) some gallium atoms found in nature have a mass that is 69.723/1.0079 times as great as that of a 1H atom.

E) no gallium atoms found in nature has a mass that is 69.723/12.000 times as great as that of a 12C atom.

Diff: 3

Section: 0.5

41) The atomic mass of naturally occurring fluorine, which exists in nature as a single isotope, is listed as 18.9984 u. This means that

A) all fluorine atoms found in nature have a mass that is 18.9984/12.000 times as great as that of a 12C atom.

B) all fluorine atoms found in nature have a mass that is 18.9984/1.0079 times as great as that of a 1H atom.

C) some fluorine atoms found in nature have a mass that is 18.9984/12.000 times as great as that of a 12C atom.

D) some fluorine atoms found in nature have a mass that is 18.9984/1.0079 times as great as that of a 1H atom.

E) no fluorine atom found in nature has a mass that is 18.9984/12.000 times as great as that of a 12C atom.

Diff: 3

Section: 0.5

42) The atomic mass of naturally occurring cobalt, which exists in nature as a single isotope, is listed as 58.9332 u. This means that

A) all cobalt atoms found in nature have a mass that is 58.9332/12.000 times as great as that of a 12C atom.

B) all cobalt atoms found in nature have a mass that is 58.9332/1.0079 times as great as that of a 1H atom.

C) some cobalt atoms found in nature have a mass that is 58.9332/12.000 times as great as that of a 12C atom.

D) some cobalt atoms found in nature have a mass that is 58.9332/1.0079 times as great as that of a 1H atom.

E) no cobalt atom found in nature has a mass that is 58.9332/12.000 times as great as that of a 12C atom.

Diff: 2

Section: 0.5

43) A naturally occurring element consists of three isotopes. The data for the isotopes are:

isotope 1: 46.972 u, 69.472%

isotope 2: 48.961 u, 21.667%

isotope 3: 49.954 u, 8.8610%

What is the average atomic mass of this naturally occurring element?

A) 47.667 u

B) 47.699 u

C) 48.629 u

D) 48.667 u

E) 48.961 u

Diff: 2

Section: 0.5

44) A naturally occurring element consists of three isotopes. The data for the isotopes are:

isotope 1: 146.9672 u, 64.792%

isotope 2: 148.9638 u, 26.117%

isotope 3: 149.9592 u, 9.0910%

What is the average atomic mass of this naturally occurring element?

A) 49.254 u

B) 147.76 u

C) 148.63 u

D) 148.67 u

E) 147.88 u

Diff: 2

Section: 0.5

45) A naturally occurring element consists of three isotopes. The data for the isotopes are:

isotope 1: 187.9122 u., 10.861%

isotope 2: 190.9047 u, ?????%

isotope 3: 192.8938 u, 76.711%

What is the average atomic mass of this naturally occurring element?

Hint: Percentages should always add up to 100% then find the weighted average.

A) 64.035 u

B) 190.57 u

C) 190.67 u

D) 192.08 u

E) 192.11 u

Diff: 3

Section: 0.5

46) A naturally occurring element consists of three isotopes. The data for the isotopes are:

isotope 1: 147.9554 u, 10.563%

isotope 2: 150.9496 u, 70.811%

isotope 3: 152.9461 u, 18.626%

What is the average atomic mass of this naturally occurring element?

A) 50.335 u

B) 150.62 u

C) 150.67 u

D) 151.01 u

E) 151.08 u

Diff: 2

Section: 0.5

47) A naturally occurring element consists of two isotopes. The data for the isotopes are:

isotope 1 68.5257 u 60.226 %

isotope 2 70.9429 u ?????? %

Calculate the average atomic mass of this element.

Hint: Percentages should always add up to 100% then find the weighted average.

A) 69.728 u

B) 69.743 u

C) 69.934 u

D) 69.972 u

E) 70.141 u

Diff: 3

Section: 0.5

48) Chemistry has four main ideas that were given in chapter 0. List them.

Diff: 2

Section: 0.5

49) Planets are formed after supernovas from ________ left over from the formation of a new star.

Diff: 2

Section: 0.1

50) What two factors determine the final chemical makeup of a planet?

Diff: 1

Section: 0.3

51) Molecules are made of tiny particles called ________.

Diff: 1

Section: 0.3

52) According to the Law ________, there is no gain or loss of mass in chemical reactions.

Diff: 1

Section: 0.4

53) In a chemical compound, the elements are always combined in the same proportions by ________.

Diff: 1

Section: 0.4

54) A compound is made of nitrogen and hydrogen in a ratio of 5.65 grams nitrogen to 1.22 grams of hydrogen. There are ________ grams of nitrogen in a sample of this compound containing 4.00 grams of hydrogen.

Hint: Consider the ratio of the masses to determine the mass of nitrogen.

Diff: 1

Section: 0.4

55) A compound is made of nitrogen and hydrogen in a ratio of 22.6 grams nitrogen to 4.88 grams of hydrogen. There are ________ grams of hydrogen in a sample of the compound containing 12.6 grams of nitrogen.

Hint: Consider the ratio of the masses to determine the mass of hydrogen.

Diff: 3

Section: 0.4

56) A compound of phosphorus and chlorine contains 3.00 grams of phosphorus and 10.3 grams of chlorine. There are ________ grams of phosphorus in a sample of the compound containing 17.2 grams of chlorine.

Hint: Consider the ratio of the masses to determine the mass of phosphorous.

Diff: 3

Section: 0.4

57) A compound of phosphorus and chlorine contains 3.00 grams of phosphorus and 10.3 grams of chlorine. There are ________ total grams of the compound in a sample that contains 4.00 grams of chlorine.

Hint: Consider the ratio of the masses to determine the mass of compound.

Diff: 3

Section: 0.4

58) If 2.00 grams of molecular hydrogen react with 16.00 grams of oxygen to form water, how many grams of water must be formed if all of the hydrogen and oxygen react?

Hint: Consider the ratio of the masses to determine the mass of compound.

Diff: 3

Section: 0.4

59) The particles found in nuclei, the protons and neutrons, are collectively called ________.

Diff: 1

Section: 0.4

60) Which subatomic particle has a positive charge?

Diff: 1

Section: 0.5

61) How many electrons are in an atom of 35Cl?

Diff: 1

Section: 0.5

62) How many nucleons are in an atom of 40K?

Diff: 1

Section: 0.5

63) The element chlorine has two main isotopes that result in almost all chlorine on Earth. The two are listed below with their atomic masses. The average atomic mass of chlorine is listed as 35.453 u. Using this information what is the relative abundances of the two chlorine isotopes?

Chlorine-35: 34.969 u

Chlorine-37: 36.966 u

Hint: Set up a weighted average calculation where one percentage is x and the other percentage is (100 - x).

Diff: 2

Section: 0.5

64) The element bromine has two main isotopes that result in almost all bromine on Earth. The two are listed below with their atomic masses. The average atomic mass of bromine is listed as 79.904 u. Using this information what is the relative abundances of the two chlorine isotopes?

Bromine-79: 78.918 u

Bromine-81: 80.916 u

Hint: Set up a weighted average calculation where one percentage is x and the other percentage is (100 - x).

Diff: 3

Section: 0.5

65) Microwave radiation observed by Penzias and Wilson in 1964 helps to support the big-bang theory because it observed microwave radiation that was characteristic of a temperature that matched the predicted temperature of the universe after heating up for 14 billion years.

Diff: 3

Section: 0.5

66) Stars that are classified as red giants are formed after the outer layer of hydrogen in a star cools and is no longer white hot.

Diff: 2

Section: 0.2

67) In stars the heaviest elements migrate to the outer layers of the star due to centrifugal forces.

Diff: 2

Section: 0.2

68) Atoms are made of tiny particles called molecules.

Diff: 1

Section: 0.2

69) In any given chemical compound, elements are be combined in various non-fixed amounts by mass.

Diff: 1

Section: 0.4

70) When a piece of paper burns in a closed container, the combined masses of the products is less than the mass of the original piece of paper.

Diff: 1

Section: 0.4

71) Atoms must be broken apart into their subatomic particles and then rearranged in order for chemical reactions to occur.

Hint: What happens in a chemical reaction between reactants and products?

Diff: 2

Section: 0.4

72) The hydrogen atom minus an electron is known as the proton.

Diff: 3

Section: 0.4

73) Almost the entire mass of an atom is concentrated in a very large volume outside the center of the atom.

Diff: 1

Section: 0.5

74) In a neutral atom, the number of protons must equal the number of neutrons.

Diff: 1

Section: 0.5

75) At the nanoscale level, the structures under investigation usually have dimensions of tens to hundreds of atoms.

Diff: 1

Section: 0.5

76) Molecular self-assembly occurs when two atoms can spontaneously arrange themselves into creating a diatomic molecular structure.

Diff: 2

Section: On the Cutting Edge 0.1

77) The atomic force microscope that is used with electrically nonconducting samples makes it possible to obtain an image of individual atoms.

Diff: 2

Section: On the Cutting Edge 0.1

78) When an electrical spark is passed through hydrogen gas molecules, positive ions can be generated through the interaction.

Diff: 2

Section: On the Cutting Edge 0.1

79) When positive ions are formed in a mass spectrometer, they are attracted to a positively charged metal plate that has a small hole in its center.

Diff: 2

Section: On the Cutting Edge 0.2

80) In a mass spectrometer, a beam of ions is sorted by the magnet into a number of beams based on the same charges that they have.

Diff: 2

Section: On the Cutting Edge 0.2

81) In a mass spectrometer, a beam of ions emerge from between the poles of the magnet after being sorted into an array of beams based on their masses.

Diff: 2

Section: On the Cutting Edge 0.2

82) According to recent IUPAC recommendations, a range of atomic masses should be used instead a single value.

Diff: 2

Section: On the Cutting Edge 0.2

83) Average atomic masses are used in the periodic table. These values give the true representation of mixtures of isotopes for different elements that are consistent around the world and universe.

Diff: 2

Section: On the Cutting Edge 0.3

84) What is the most logical reason for only light elements being formed during the nucleosynthesis stage of the big-bang?

Hint: Consider the kinetic energy of the particles and how kinetic energy can affect them coming together.

A) There were not enough neutrons and protons to produce large elements.

B) The density of protons and neutrons was not large enough.

C) The electrons were not present yet to form protons and neutrons to a large scale.

D) Temperatures were still too great for a large number of protons and neutrons to stabilize into one atom.

E) There were not enough neutrons to produce large elements.

Diff: 3

Section: On the Cutting Edge 0.3, 0.4

85) Assuming that most of the mass of the universe is found in stars, why is hydrogen still the most common element in the universe?

Hint: Consider the kinetic energy of the particles and how kinetic energy can affect them coming together.

A) There were not enough neutrons and protons to produce large elements.

B) The density of protons and neutrons was not large enough.

C) The electrons were not present yet to form protons and neutrons to a large scale.

D) Temperatures in stars are still too great for a large number of protons and neutrons to stabilize into one atom.

E) Hydrogen is found in the outer layer of stars, which has the largest volume.

Diff: 3

Section: 0.2

86) A compound of hydrogen and sulfur contains 2.69 grams of hydrogen and 47.31 grams of sulfur. Another sample of the same compound that contains 75.63 grams of sulfur would contain how many grams of hydrogen?

Hint: Consider the ratio of the masses to determine the mass of hydrogen

A) 2.69 g

B) 1.68 g

C) 0.59 g

D) 4.30 g

E) 203.4 g

Diff: 3

Section: 0.2

87) Based on the law of Conservation of Mass, 1.2 g of elemental carbon (C) reacts with

molecular oxygen (O2) to produce 4.4 g of carbon dioxide gas (CO2) as the only product. What mass of oxygen reacts?

A) 16 g

B) 1.0 g

C) 4.4 g

D) 22 g

E) 3.2 g

Diff: 3

Section: 0.4

88) Based on the law of Conservation of Mass, 1.8 g of elemental carbon (C) reacts with 4.8 g of

molecular oxygen (O2) to produce carbon dioxide gas (CO2) as the only product. What mass of carbon dioxide is formed?

A) 18 g

B) 1.9 g

C) 6.6 g

D) 12 g

E) 1.2 g

Diff: 2

Section: 0.4

89) Based on the law of Conservation of Mass, 65.4 g of zinc metal reacts with exactly 32.1 g of sulfur to produce zinc sulfide (ZnS) as the only product. What mass of zinc sulfide can be formed from 10.0 g zinc metal?

Hint: Consider the ratio of the masses to determine the mass of zinc sulfide.

A) 28 g

B) 19 g

C) 5.6 g

D) 14.9 g

E) 8.4 g

Diff: 2

Section: 0.4

90) The major isotopes of tungsten (with abundances shown) are 182W (26.32%), 183W (14.31%), 184W (30.67%), and 186W (28.62%). What is the atomic mass of tungsten?

A) 184

B) 183

C) 190

D) 186

E) 185

Diff: 3

Section: 0.4

91) A naturally occurring element consists of two isotopes. Calculate the average atomic mass and identify the element, based on the data below.

isotope 1: 10.013 u 19.78 %

isotope 2: 11.009 u ??????%

Hint: Percentages should always add up to 100% then find the weighted average.

A) 10.991 u, neon

B) 10.81 u, lithium

C) 10.81 u, boron

D) 11.01 u, carbon

E) 10.81 u, nitrogen

Diff: 3

Section: 0.5

92) A naturally occurring element consists of two isotopes. Calculate the fractional abundances for the two isotopes, if its average atomic mass is 107.87 u.

isotope 1: 106.91 u ?? %

isotope 2: 108.90 u ?? %

Hint: Set up a weighted average calculation where one percentage is x and the other percentage is (100-x).

A) 106.91 u, 39.264 %; 108.90 u, 60.736 %

B) 106.91 u, 44.150 %; 108.90 u, 55.850 %

C) 106.91 u, 55.850 %; 108.90 u, 44.150 %

D) 106.91 u, 51.759 %; 108.90 u, 48.241 %

E) 106.91 u, 41.759 %; 108.90 u, 58.241 %

Diff: 3

Section: 0.5

© 2022 John Wiley & Sons, Inc. All rights reserved. Instructors who are authorized users of this course are permitted to download these materials and use them in connection with the course. Except as permitted herein or by law, no part of these materials should be reproduced, stored in a retrieval system, or transmitted, in any form or by any means, electronic, mechanical, photocopying, recording or otherwise.