Chemistry A Molecular Approach 3rd Edition Test Bank

Follow Below Link to Download File

https://homeworklance.com/downloads/chemistry-molecular-approach-3rd-edition-test-bank/

We also Do 100% Original and Plagiarism Free Assignment / Homework and Essay

Email us for original and Plagiarism Free Work At ( info.homeworklance@gmail.com ) or order us at

(https://homeworklance.com/custom-order/ )

View Sample Chapter Below:

Chemistry: A Molecular Approach, 3e (Tro)

Chapter 4   Chemical Quantities and Aqueous Reactions

Multiple Choice Questions

1) Global warming is thought to be caused by the increase of one particular gas.  Name the gas.

1.     A) oxygen

2.     B) carbon monoxide

3.     C) carbon dioxide

4.     D) nitrogen

5.     E) helium

Answer:  C

Diff: 1      Page Ref: 4.1

2) How many grams of Li3N can be formed from 1.75 moles of Li?  Assume an excess of nitrogen.

6 Li(s) +  N2(g)  →  2 Li3N(s)

18.   A) 18.3 g Li3N

19.   B) 20.3 g Li3N

20.   C) 58.3 g Li3N

21.   D) 61.0 g Li3N

22.   E) 15.1 g Li3N

Answer:  B

Diff: 3      Page Ref: 4.2

3) How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction?  The molar mass of KNO3 is 101.11 g/mol.

4 KNO3(s)  →  2 K2O(s) + 2 N2(g)  + 5 O2(g)

1.     A) 0.290 mol O2

2.     B) 0.580 mol O2

3.     C) 18.5 mol O2

4.     D) 0.724 mol O2

5.     E) 1.73 mol O2

Answer:  D

Diff: 3      Page Ref: 4.2

4) How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction?  The molar mass of KNO3 is 101.11 g/mol.

4 KNO3(s)  →  2 K2O(s) + 2 N2(g)  + 5 O2(g)

1.     A) 0.290 mol N2

2.     B) 0.580 mol N2

3.     C) 18.5 mol N2

4.     D) 0.724 mol N2

5.     E) 1.73 mol N2

Answer:  A

Diff: 3      Page Ref: 4.2

5) Two samples of calcium fluoride are decomposed into their constituent elements.  The first sample produced 0.154 g of calcium and 0.146 g of fluorine.  If the second sample produced 294 mg of fluorine, how many g of calcium were formed?

1.     A) 0.280 g

2.     B) 3.09 × 102g

3.     C) 3.13 g

4.     D) 0.309 g

5.     E) 2.80 × 102g

Answer:  D

Diff: 3      Page Ref: 4.2

6) Two samples of potassium iodide are decomposed into their constituent elements.  The first sample produced 13.0 g of potassium and 42.3 g of iodine.  If the second sample produced 24.4 kg of potassium, how many kg of iodine were produced?

13.   A) 13.3 kg

14.   B) 22.5 kg

15.   C) 79.4 kg

16.   D) 44.4 kg

17.   E) 92.4 kg

Answer:  C

Diff: 3      Page Ref: 4.2

7) A 14.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3).  If ammonia is the only product, what mass of ammonia is formed?

17.   A) 17.01 g

18.   B) 1.10 g

19.   C) 14.01 g

20.   D) 3.02 g

21.   E) 23.07 g

Answer:  A

Diff: 3      Page Ref: 4.2

8) Consider the following balanced reaction.  How many grams of water are required to form 75.9 g of HNO3?  Assume that there is excess NO2 present.  The molar masses are as follows:  H2O = 18.02 g/mol, HNO3 = 63.02 g/mol.

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

38.   A) 38.0 g H2O

39.   B) 21.7 g H2O

40.   C) 43.4 g H2O

41.   D) 10.9 g H2O

42.   E) 26.5 g H2O

Answer:  D

Diff: 4      Page Ref: 4.2

9) Consider the following reaction.  How many moles of oxygen are required to produce 2.33 moles of water?  Assume that there is excess C3H7SH present.

C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)

1.     A) 1.55 moles O2

2.     B) 3.50 moles O2

3.     C) 2.33 moles O2

4.     D) 4.14 moles O2

5.     E) 6.21 moles O2

Answer:  B

Diff: 2      Page Ref: 4.2

10) Consider the following balanced reaction.  What mass (in g) of CO2 can be formed from 288 mg of O2?  Assume that there is excess C3H7SH present.

C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g)

1.     A) 0.396 g CO2

2.     B) 0.209 g CO2

3.     C) 0.792 g CO2

4.     D) 0.126 g CO2

5.     E) 0.198 g CO2

Answer:  E

Diff: 4      Page Ref: 4.2

11) According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed?

2 H2S(g) +  SO2(g)  →  3 S(s)  + 2H2O(l)

99.   A) 99.8 g S

100.B) 66.6 g S

101.C) 56.1 g S

102.D) 44.4 g S

103.E) 14.0 g S

Answer:  A

Diff: 4      Page Ref: 4.2

12) How many molecules of H2S are required to form 79.0 g of sulfur according to the following reaction?  Assume excess SO2.

2 H2S(g) + SO2(g)  →  3 S(s) + 2H2O(l)

1.     A) 1.48 × 1024 molecules H2S

2.     B) 9.89 × 1023 molecules H2S

3.     C) 5.06 × 1025 molecules H2S

4.     D) 3.17 × 1025 molecules H2S

5.     E) 2.44 × 1023 molecules H2S

Answer:  B

Diff: 5      Page Ref: 4.2

13) Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2.

2 C8H18  +  25 O2  →  16 CO2  +  18 H2O

1.     A) 0.640 moles

2.     B) 64.0 moles

3.     C) 2.56 moles

4.     D) 16.0 moles

Answer:  C

Diff: 3      Page Ref: 4.3

14) A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl3).  If it is the only product, what mass of PCl3 is formed?

30.   A) 30.15 g

31.   B) 54.93 g

32.   C) 140.01 g

33.   D) 79.71 g

34.   E) 91.86 g

Answer:  B

Diff: 3      Page Ref: 4.3

15) Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N2O4 and 45.0 g N2H4.  Some possibly useful molar masses are as follows:  N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol.

N2O4(l) + 2 N2H4(l)  →  3 N2(g) + 4 H2O(g)

59.   A) LR = N2H4, 59.0 g N2 formed

60.   B) LR = N2O4, 105 g N2 formed

61.   C) LR = N2O4, 45.7 g N2 formed

62.   D) LR = N2H4, 13.3 g N2 formed

63.   E) No LR, 45.0 g N2 formed

Answer:  C

Diff: 5      Page Ref: 4.3

16) Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction.  A possibly useful molar mass is BCl3 = 117.16 g/mol.

BCl3(g) + 3 H2O(l)  →  H3BO3(s) + 3 HCl(g)

75.   A) 75.9 g HCl

76.   B) 132 g HCl

77.   C) 187 g HCl

78.   D) 56.0 g HCl

79.   E) 25.3 g HCl

Answer:  D

Diff: 5      Page Ref: 4.3

17) According to the following reaction, what amount of Al2S3 remains when 20.00 g of Al2S3 and 2.00 g of H2O are reacted?  A few of the molar masses are as follows:  Al2S3 = 150.17 g/mol, H2O = 18.02 g/mol.

Al2S3(s) + 6 H2O(l)  →  2 Al(OH)3(s) + 3 H2S(g)

28.   A) 28.33 g

29.   B) 14.00 g

30.   C) 8.33 g

31.   D) 19.78 g

32.   E) 17.22 g

Answer:  E

Diff: 5      Page Ref: 4.3

18) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2.

2 C8H18 + 25 O2  →  16 CO2 + 18 H2O

20.   A) 20.00%

21.   B) 25.00%

22.   C) 50.00%

23.   D) 12.50%

Answer:  B

Diff: 5      Page Ref: 4.3

19) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 8.000 moles of O2.

2 C8H18 + 25 O2  →  16 CO2 + 18 H2O

20.   A) 20.00%

21.   B) 25.00%

22.   C) 50.00%

23.   D) 12.50%

Answer:  D

Diff: 5      Page Ref: 4.3

20) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 8.000 moles of C8H18 with 4.000 moles of O2.

2 C8H18 + 25 O2  →  16 CO2 + 18 H2O

20.   A) 20.00%

21.   B) 25.00%

22.   C) 50.00%

23.   D) 12.50%

Answer:  B

Diff: 5      Page Ref: 4.3

21) Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react with excess Al according to the following reaction.

Fe2O3(s) + 2 Al(s)  →  Al2O3(s) + 2 Fe(s)

61.   A) 61.03 %

62.   B) 28.65 %

63.   C) 57.30 %

64.   D) 20.02 %

65.   E) 81.93 %

Answer:  E

Diff: 5      Page Ref: 4.3

22) Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

1.     A) 1.50 M

2.     B) 1.18 M

3.     C) 0.130 M

4.     D) 0.768 M

5.     E) 2.30 M

Answer:  A

Diff: 3      Page Ref: 4.4