Chemistry 13Th Edition By Raymond Chang – Test Bank

 

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Sample Test

Chapter 03

Mass Relationships in Chemical Reactions

 

 

 

Multiple Choice Questions

 

1.   An atom of helium has a mass about four times greater than that of an atom of hydrogen. Which choice makes the correct comparison of the redative numbers of helium and hydrogen atoms in equal masses of the two elements?

2.   There are about four times as many helium atoms as hydrogen atoms.

3.   There are about two times as many helium atoms as hydrogen atoms.

4.   The number of helium and hydrogen atoms is the same.

5.   There are about half as many helium atoms as hydrogen atoms.

6.   There are about one-fourth as many helium atoms as hydrogen atoms.

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.01

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

2.   There are two stable isotopes of chlorine: chlorine-35, with a mass of 34.968853 amu; and chlorine-37, with a mass of 36.965903. Given that the average atomic mass of a chlorine atom is 35.45 amu, which of the following statements is true?

3.    

Chlorine contains almost exclusively  CI with very little  Cl.

 

1.    

Chlorine contains more  Cl than  Cl.

 

1.    

Chlorine contains roughly equal amounts of  Cl and  Cl.

 

1.    

Chlorine contains more  Cl than  Cl.

 

1.    

Chlorine contains almost exclusively of  Cl, with very little  Cl.

 

 

 

Bloom’s Level: 5. Evaluate

Difficulty: Easy

Gradable: automatic

Section: 03.01

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

3.   An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative numbers of bromine and neon atoms in 1,000 g of each element?

4.   The number of bromine and neon atoms is the same.

5.   There are one thousand times as many bromine atoms as neon atoms.

6.   There are one thousand times as many neon atoms as bromine atoms.

7.   There are four times as many neon atoms as bromine atoms.

8.   There are four times as many bromine atoms as neon atoms.

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.01

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

4.   An atom of bromine has a mass about four times greater than that of an atom of neon. How many grams of neon will contain the same number of atoms as 1,000 g of bromine?

5.   4 g Ne

6.   250 g Ne

7.   400 g Ne

8.   1,000 g Ne

9.   4,000 g Ne

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.01

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

5.   An average atom of uranium (U) is approximately how many times heavier than an atom of potassium?

6.   6.1 times

7.   4.8 times

8.   2.4 times

9.   12.5 times

10.                7.7 times

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.01

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

6.   Boron obtained from borax deposits in Death Valley consists of two isotopes. They are boron-10 and boron-11 with atomic masses of 10.013 amu and 11.009 amu, respectively. The atomic mass of boron is 10.81 amu (see periodic table). Which isotope of boron is more abundant, boron-10 or boron-11?

7.   Cannot be determined from data given

8.   Neither, their abundances are the same.

9.   Boron-10

10.                Boron-11

 

 

Bloom’s Level: 5. Evaluate

Difficulty: Medium

Gradable: automatic

Section: 03.01

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

7.   The element oxygen consists of three naturally occurring isotopes: 16O, 17O, and 18O. The atomic mass of oxygen is 16.0 amu. What can be implied about the relative abundances of these isotopes?

8.   More than 50% of all O atoms are 17O.

9.   Almost all O atoms are 18O.

10.                Almost all O atoms are 17O.

11.                The isotopes all have the same abundance, i.e. 33.3%.

12.                The abundances of 17O and 18O are very small.

 

 

Bloom’s Level: 5. Evaluate

Difficulty: Medium

Gradable: automatic

Section: 03.01

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

8.    

Calculate the average atomic mass of lithium using the following data:

 

 

6.   6.51 amu

7.   6.02 amu

8.   6.94 amu

9.   7.02 amu

10.                6.50 amu

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.01

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

9.    

Calculate the average atomic mass of silver using the following data:

 

 

106.             106.91 amu

107.             108.00 amu

108.             107.90 amu

109.             107.87 amu

110.             108.90 amu

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.01

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

10.                What is the average mass of one S atom?

11.                32.07 g

12.                32.07 amu

13.                32.07 g/mol

14.                5.32 x 10-23 amu

15.                1.93 x 1025 g

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

11.                What is the molecular mass of Br2?

12.                79.90 amu

13.                79.90 g

14.                159.8 amu

15.                159.8 g

16.                2.65 x 10-22 amu

 

 

Bloom’s Level: 3. Apply

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

 

12.                What is the average mass of one Ca atom?

13.                40.08 amu

14.                40.08 g

15.                40.08 g/mol

16.                2.41 x 10-21 amu

17.                2.41×1025 g

 

 

Bloom’s Level: 3. Apply

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

13.                What is the average mass, in grams, of one Zn atom?

14.                65.39 amu

15.                65.39 g

16.                3.94 x 1025g

17.                1.09 x 10-22 g

18.                1.661 x 10-24g

 

 

Bloom’s Level: 3. Apply

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

14.                What is the average mass, in grams, of one Rb atom?

15.                6.02 x 1023 g

16.                1.42 x 10-22g

17.                5.15 x 1025 g

18.                85.47 g

19.                85.47 amu

 

 

Bloom’s Level: 3. Apply

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

15.                What is the mass of 3.50 x 1024 Ti atoms?

16.                47.9 amu

17.                47.9 g

18.                5.81 g

19.                278 g

20.                5.81 amu

 

 

Bloom’s Level: 3. Apply

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

16.                What is the mass of 4.50 x 1022 Cu atoms?

17.                7.47 x 10-2 g

18.                7.47 x 10-2 amu

19.                4.75 g

20.                63.55 amu

21.                63.55 g

 

 

Bloom’s Level: 3. Apply

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

17.                If 0.274 moles of a substance weighs 62.5 g, what is the molar mass of the substance, in units of g/mol?

18.                2.28 ´ 102 g/mol

19.                1.71 ´ 101 g/mol

20.                4.38 ´ 10–3 g/mol

21.                2.17 ´ 102 g/mol

22.                6.02 x 1023 g/mol

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

18.                One mole of iron

19.                is heavier than one mole of lead (Pb).

20.                is 77.0 g of iron.

21.                is 26.0 g of iron.

22.                weighs the same as one mole of lead.

23.                None of the above.

 

 

Bloom’s Level: 5. Evaluate

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

19.                Which one of the following does not represent 1.000 mol of the indicated substance?

20.                6.022 ´ 1023 C atoms

21.                26.00 g Fe

22.                12.01 g C

23.                65.39 g Zn

24.                6.022 ´ 1023 Fe atoms

 

 

Bloom’s Level: 5. Evaluate

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

20.                How many Br atoms are in 2.50 g of Br?

21.                 

1.88 x 1022 Br atoms

 

1.   1.51 x 1024 Br atoms

2.   7.54 x 1021 Br atoms

3.   6.02 x 1023 Br atoms

4.   9.42 x 1021 Br atoms

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

21.                How many C atoms are in 5.50 g of C?

22.                5.01 x 1022 C atoms

23.                3.31 x 1024 C atoms

24.                6.02 x 1023 C atoms

25.                2.76 x 1023 C atoms

26.                5.50 x 1023 C atoms

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

 

22.                Determine the number of moles of aluminum in 96.7 g of Al.

23.                0.279 mol

24.                3.58 mol

25.                7.43 mol

26.                4.21 mol

27.                6.02 ´ 1023 mol

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

23.                Calculate the number of moles of xenon in 12.0 g of xenon.

24.                1.00 mol

25.                0.0457 mol

26.                0.183 mol

27.                7.62 ´ 10–3 mol

28.                0.0914 mol

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

24.                A gold wire has a diameter of 1.00 mm. What length of this wire contains exactly 1.00 mol of gold? (density of Au = 17.0 g/cm3)

25.                2630 m

26.                3.69 m

27.                251 m

28.                14.8 m

29.                62.7 m

 

 

Bloom’s Level: 4. Analyze

Difficulty: Difficult

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

25.                A silver wire has a diameter of 0.500 mm. What length of this wire contains exactly 1.00 mol of silver? (density of Ag = 10.5 g/cm3)

26.                52.3 m

27.                222 m

28.                13.1 m

29.                2.01 m

30.                890 m

 

 

Bloom’s Level: 4. Analyze

Difficulty: Difficult

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

26.                A copper wire has a diameter of 2.00 mm. What length of this wire contains exactly 1.00 mol of copper? (density of Cu = 8.92 g/cm3)

27.                0.178 m

28.                0.567 m

29.                180 m

30.                45.1 m

31.                2.27 m

 

 

Bloom’s Level: 4. Analyze

Difficulty: Difficult

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

27.                How many F atoms are in 5.54 g of F2?

28.                6.02 ´ 1023 atoms

29.                0.146 atoms

30.                0.292 atoms

31.                8.78 ´ 1022 atoms

32.                1.76 ´ 1023 atoms

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

28.                How many O atoms are in 4.39 g of CO2?

29.                5.29 x 1024 O atoms

30.                1.03 x 1022 O atoms

31.                1.65 x 1023 O atoms

32.                6.01 x 1022 O atoms

33.                1.20 x 1023 O atoms

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

29.                How many Cl atoms are in 0.0728 g of PCl3?

30.                4.38 x 1022 Cl atoms

31.                1.32 x 1023 Cl atoms

32.                3.19 x 1020 Cl atoms

33.                9.58 x 1020 Cl atoms

34.                1.81 x 1024 Cl atoms

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

30.                How many moles of CF4 are there in 171 g of CF4?

31.                0.51 mol

32.                1.94 mol

33.                4.07 mol

34.                88.0 mol

35.                171 mol

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

31.                How many moles of NH3 are there in 77.5 g of NH3?

32.                0.220 mol

33.                4.55 mol

34.                14.0 mol

35.                1.31 ´ 103 mol

36.                None of the above.

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

32.                Calculate the number of moles of cesium in 50.0 g of cesium.

33.                0.376 mol

34.                0.357 mol

35.                2.66 mol

36.                2.80 mol

37.                0.0200 mol

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

33.                Which of the following samples contains the greatest number of atoms?

34.                100 g of Pb

35.                2.0 mole of Ar

36.                0.1 mole of Fe

37.                5 g of He

38.                20 million O2 molecules

 

 

Bloom’s Level: 5. Evaluate

Difficulty: Medium

Gradable: automatic

Section: 03.02

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

34.                Which of the following CO2 samples contains the greatest number of moles of CO2?

35.                3.5 moles CO2

36.                3.21 x 1023 CO2 molecules

37.                4.50 x 1022 CO2 molecules

38.                5.60 g CO2

39.                3.19 x 101 g CO2

 

 

Bloom’s Level: 5. Evaluate

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

 

35.                Which of the following NH3 samples contains the greatest number of moles of NH3?

36.                0.356 moles NH3

37.                4.65 x 1023 NH3 molecules

38.                6.78 x 1022 NH3 molecules

39.                8.90g NH3

40.                6.78 x 101g NH3

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: The Mole (Definition and Avogadro’s number)

Topic: Stoichiometry and Chemical Reactions

 

 

36.                Calculate the molar mass of Ba(NO3)2.

37.                199.3 g/mol

38.                323.3 g/mol

39.                247.3 g/mol

40.                261.3 g/mol

41.                398.6 g/mol

 

 

Bloom’s Level: 3. Apply

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

 

37.                Calculate the molar mass of (NH4)2SO4.

38.                114.11 g/mol

39.                228.22 g/mol

40.                118.14 g/mol

41.                63.09 g/mol

42.                132.15 g/mol

 

 

Bloom’s Level: 3. Apply

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

 

 

 

38.                Calculate the molecular mass of menthol, C10H20O.

39.                156.26 amu

40.                140.26 amu

41.                29.02 amu

42.                48.17 amu

43.                137.11 amu

 

 

Bloom’s Level: 3. Apply

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

 

 

39.                What is the molar mass of acetaminophen, C8H9NO2?

40.                151.16 g/mol

41.                43.03 g/mol

42.                67.09 g/mol

43.                143.10 g/mol

44.                135.16 g/mol

 

 

Bloom’s Level: 3. Apply

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

 

40.                What is the molecular mass of nicotine, C10H14N2?

41.                27.03 amu

42.                148.22 amu

43.                149.13 amu

44.                81.12 amu

45.                162.23 amu

 

 

Bloom’s Level: 3. Apply

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Molar Mass

Topic: Stoichiometry and Chemical Reactions

 

 

 

41.                What is the mass of 0.0250 mol of P2O5?

42.                35.5 g

43.                5676 g

44.                0.0250 g

45.                1.51 ´ 1022 g

46.                3.55 g

 

 

Bloom’s Level: 3. Apply

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

42.                Calculate the mass of 3.00 moles of CF2Cl2.

43.                3.00 g

44.                174 g

45.                363 g

46.                1.81 ´ 1024 g

47.                40.3 g

 

 

Bloom’s Level: 3. Apply

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

43.                Calculate the mass of 4.50 moles of Ca3PO4.

44.                215 g

45.                968 g

46.                0.0209 g

47.                87.1 g

48.                392 g

 

 

Bloom’s Level: 3. Apply

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

44.                Calculate the mass of 0.00456 moles of (NH4)2SO4.

45.                132 g

46.                3.45 x 10-5 g

47.                114 g

48.                0.603 g

49.                0.520 g

 

 

Bloom’s Level: 3. Apply

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

45.                The molecular formula of aspirin is C9H8O4. How many aspirin molecules are present in one 500-milligram tablet?

46.                2.77 molecules

47.                2.77 ´ 10–3 molecules

48.                1.67 ´ 1024 molecules

49.                1.67 ´ 1021 molecules

50.                None of these is correct.

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

46.                Formaldehyde has the formula CH2O. How many molecules are there in 0.11 g of formaldehyde?

47.                6.1 ´ 10–27

48.                3.7 ´ 10–3

49.                4.0

50.                2.2 ´ 1021

51.                6.6 ´ 1022

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

47.                How many molecules are there in 8.0 g of ozone, O3?

48.                3.0 molecules

49.                3.6 ´ 1024 molecules

50.                1.0 ´ 1023 molecules

51.                3.0 ´ 1023 molecules

52.                6.0 ´ 1023 molecules

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

48.                How many moles of HCl are represented by 1.0 ´ 1019 HCl molecules?

49.                1.7 ´ 10–5 mol

50.                1.5 ´ 10–3 mol

51.                1.0 ´ 1019 mol

52.                37 mol

53.                6.0 ´ 104 mol

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.02

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

49.                How many sodium atoms are there in 6.0 g of Na3N?

50.                3.6 ´ 1024 atoms

51.                4.6 ´ 1022 atoms

52.                1.3 ´ 1023 atoms

53.                0.22 atoms

54.                0.072 atoms

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

50.                How many moles of O are in 2.45 moles of H2CO3?

51.                2.45 moles O

52.                39.2 moles O

53.                118 moles O

54.                7.35 moles O

55.                0.459 moles O

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

51.                How many moles of H are in 4.56 moles of NH2NH2?

52.                4.52 moles H

53.                4.56 moles H

54.                9.12 moles H

55.                18.39 moles H

56.                18.24 moles H

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

52.                How many moles of C are in 1.22 moles of C6H12O6?

53.                7.32 moles C

54.                87.9 moles C

55.                1.22 moles C

56.                14.7 moles C

57.                2.44 moles C

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

53.                How many sulfur atoms are there in 21.0 g of Al2S3?

54.                8.42 ´ 1022 atoms

55.                2.53 ´ 1023 atoms

56.                2.14 ´ 1023 atoms

57.                6.02 ´ 1023 atoms

58.                6.30 ´ 1026 atoms

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

54.                How many sulfur atoms are present in 25.6 g of Al2(S2O3)3?

55.                0.393

56.                6.00

57.                3.95 ´ 1022

58.                7.90 ´ 1022

59.                2.37 ´ 1023

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

55.                How many fluorine atoms are there in 65 g of CF4?

56.                0.74 atoms

57.                3.0 atoms

58.                4.5 ´ 1023 atoms

59.                1.8 ´ 1024 atoms

60.                2.4 ´ 1023 atoms

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

56.                How many moles of O atoms are in 25.7 g of CaSO4?

57.                0.189 mol

58.                0.755 mol

59.                4.00 mol

60.                1.14 ´ 1023 mol

61.                4.55 ´ 1023 mol

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

57.                How many O atoms are there in 51.4 g CaSO4?

58.                4.00

59.                2.40 ´ 1024

60.                1.13

61.                9.09 ´ 1023

62.                2.28 ´ 1023

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

58.                How many moles of Cl atoms are there in 65.2 g CHCl3?

59.                0.548 mol

60.                1.09 mol

61.                3.30 ´ 1023 mol

62.                1.64 mol

63.                3.00 mol

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

59.                How many carbon atoms are there in 15 lbs of sugar, C12H22O11?

60.                4.1 x 1028 C atoms

61.                1.2 x 1026 C atoms

62.                1.4 x 1026 C atoms

63.                2.6 x 1022 C atoms

64.                3.2 x 1023 C atoms

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

60.                Calculate the mass of O in 4.36 g of Cl2O7?

61.                30.5 g O

62.                48.8 g O

63.                11.2 g O

64.                69.8 g O

65.                2.67 g O

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

61.                Calculate the mass of C in 5.46 g of C2H4?

62.                0.455 g C

63.                4.68 g C

64.                65.6 g C

65.                13.1 g C

66.                24.0 g C

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

62.                Calculate the mass of N in 2.34 g of N2H4?

63.                4.68 g N

64.                65.6 g N

65.                28.02 g N

66.                2.05 g N

67.                2.34 g N

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

63.                How many grams of nitrogen are there in 7.5 g of Ca(NO3)2?

64.                0.64 g

65.                1.3 g

66.                0.15 g

67.                1.2 g

68.                2.3 g

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

64.                Calculate the mass of 4.50 moles of chlorine gas, Cl2.

65.                6.34 ´ 10–2 g

66.                4.50 g

67.                15.7 g

68.                160. g

69.                319 g

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

65.                What is the mass of 3.00 moles of ethanol, C2H6O?

66.                4.99 ´ 10–24 g

67.                138 g

68.                6.52 ´ 10–2 g

69.                50.0 g

70.                1.81 ´ 1024 g

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

66.                What is the mass of 0.55 mole of C6H6?

67.                78.11 g

68.                78.11 amu

69.                42.96 g

70.                42.96 amu

71.                7.04 x 10-3 g

 

 

Bloom’s Level: 4. Analyze

Difficulty: Easy

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

67.                What is the mass of 8.25 ´ 1019 UF6 molecules?

68.                352 g

69.                0.0482 g

70.                1.37 ´ 10–4 g

71.                2.90 ´ 1022 g

72.                8.25 ´ 1019 g

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.03

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

 

 

68.                A mass spectrometer works by ionizing atoms or molecules, and then accelerating them through oppositely charged plates. The mass is obtained by

69.                measuring the force of impact on a detecting screen, and then calculating the mass using force = mass ´ acceleration.

70.                suspending the ions in an applied electric field, and then calculating mass by the setting the downward gravitational force equal to the upward electrostatic force.

71.                measuring the magnitude of deflection as the ions pass through a magnetic field to obtain the charge-to-mass ratio, and then calculating the mass from that ratio.

72.                measuring the time it takes for the ions to hit the detector at a known distance to calculate the acceleration, and then calculating mass from force = mass ´ acceleration.

 

 

Bloom’s Level: 5. Evaluate

Difficulty: Medium

Gradable: automatic

Section: 03.04

Subtopic: Molear Mass

Topic: Stoichiometry and Chemical Reactions

 

69.                The mineral pyrolusite is a compound of 55Mn and 16O. If 63% of the mass of pyrolusite is due to manganese, what is the empirical formula of pyrolusite?

70.                MnO

71.                Mn2O

72.                Mn2O2

73.                MnO2

74.                none of these

 

 

Bloom’s Level: 4. Analyze

Difficulty: Difficult

Gradable: automatic

Section: 03.06

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

 

 

 

70.                The mineral manganosite is a compound of 55Mn and 16O. If 77% of the mass of manganosite is due to manganese, what is the empirical formula of manganosite?

71.                MnO

72.                Mn2O

73.                Mn2O2

74.                MnO2

75.                none of these

 

 

Bloom’s Level: 4. Analyze

Difficulty: Difficult

Gradable: automatic

Section: 03.06

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

 

71.                The mineral hausmannite is a compound of 55Mn and 16O. If 72% of the mass of hausmannite is due to manganese, what is the empirical formula of hausmannite?

72.                MnO

73.                Mn3O

74.                Mn3O4

75.                Mn4O3

76.                MnO3

 

 

Bloom’s Level: 4. Analyze

Difficulty: Difficult

Gradable: automatic

Section: 03.06

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

 

 

 

72.                Zircon is a mineral with the empirical formula ZrSiO4. If all the zirconium is 90Zr, all the silicon is 28Si, and all the oxygen is 16O, what mass of oxygen is present in 10. g of zircon?

73.                0.88 g

74.                1.2 g

75.                1.8 g

76.                3.5 g

77.                5.4 g

 

 

Bloom’s Level: 4. Analyze

Difficulty: Difficult

Gradable: automatic

Section: 03.05

Subtopic: Mole Conversions

Topic: Stoichiometry and Chemical Reactions

 

73.                The mineral orpiment, having the empirical formula As2S3, was used in ancient times as a cosmetic. What mass of arsenic is present in 5.0 g of orpiment? [Given: naturally occurring arsenic is all arsenic-75; assume that all naturally occurring sulfur is sulfur-32 (only approximately true)]

74.                0.61 g

75.                3.0 g

76.                1.5 g

77.                2.0 g

78.                3.5 g

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.05

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

 

 

 

 

74.                A compound with an empirical formula of C2H4Br has a molar mass of 215.90 g/mol. What is the molecular formula?

75.                C4H8Br2

76.                C2H4Br

77.                CHBr

78.                C6H12Br3

79.                C4H8Br

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.06

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions

 

75.                A compound with an empirical formula of C2H3Br2 has a molar mass of 373.69 g/mol. What is the molecular formula?

76.                C2H3Br2

77.                CHBr

78.                C6H9Br6

79.                C4H6Br2

80.                C4H6Br4

 

 

Bloom’s Level: 4. Analyze

Difficulty: Medium

Gradable: automatic

Section: 03.06

Subtopic: Formula Determination of Unknown Compounds (Empirical and Molecular Formulas)

Topic: Stoichiometry and Chemical Reactions