Chemistry For Today General Organic and Biochemistry 8th International Edition by Spencer L. Seager - Test Bank

Chemistry For Today General Organic and Biochemistry 8th International Edition by Spencer L. Seager – Test Bank

 

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Sample Questions Are Posted Below

 

Chapter 5—Chemical Reactions

 

MULTIPLE CHOICE

 

1. Which of the following statements is not true about the reaction?

2 CH₄ + 3 O₂ ® 2 CO₂ + 4 H₂O

a.	Water is a reactant.
b.	Methane and carbon dioxide are products.
c.	Methane is a product.
d.	Water and carbon dioxide are products.

 

 

ANS:  D                    PTS:  1

 

2. Which of the following reactions is correctly balanced?

a.	N2 + H ® 2NH3	c.	Zn + 2HCl ® H2 + ZnCl2
b.	2H2O + C ® CO + 2H2	d.	CO + O2 ® CO2

 

 

ANS:  C                    PTS:  1

 

3. Which set of coefficients balances the equation?

____ CH₄ ®  ____C₃H₈ + ____ H₂

a.

3,1,1

b.

3,2,1

c.

3,1,2

d.

6,2,2

 

 

ANS:  C                    PTS:  1

 

4. When the equation below is properly balanced, what coefficient is in front of KCl?

KClO₃ ® KCl + O₂

a.

1

b.

2

c.

3

d.

4

 

 

ANS:  B                    PTS:  1

 

5. Propane, C₃H₈, burns to produce carbon dioxide and water by the equation below. What is the coefficient in front of the carbon dioxide in the balanced equation?

C₃H₈ + O₂ ® CO₂ + H₂O

a.

1

b.

2

c.

3

d.

6

 

 

ANS:  C                    PTS:  1

 

6. Consider the reactants and propose the right side of the equation.

Mg + H₂SO₄ ®  _______

a.

no reaction

b.

MgHSO4

c.

MgSO4 + H2

d.

MgH2 + SO4

 

 

ANS:  C                    PTS:  1

 

7. Consider the reactants in the partial equation given. Which choice is a product?

H₃PO₄ + Sr(OH)₂ ®  ____

a.

no reaction

b.

SrH3PO5

c.

SrH5PO6

d.

Sr3(PO4)2

 

 

ANS:  D                    PTS:  1

 

8. Which species would be considered a spectator ion based on the following equation?

Ba²⁺ + 2NO₃^– + 2Na⁺ + SO₄²⁺ ® BaSO_4(s) + 2NO₃^– + 2Na⁺

a.

Ba2+

b.

SO42+

c.

BaSO4

d.

2NO3–

 

 

ANS:  D                    PTS:  1

 

9. A REDOX reaction can also be a(n)

a.	combination reaction.	c.	decomposition reaction.
b.	single replacement reaction.	d.	More than one response is correct.

 

 

ANS:  D                    PTS:  1

 

10. Which of the following is an oxidizing agent?

a.

O2

b.

H2

c.

H2O

d.

HCl

 

 

ANS:  A                    PTS:  1

 

11. Single replacement reactions are always

a.	redox reactions.	c.	combination reactions.
b.	nonredox reactions.	d.	decomposition reactions.

 

 

ANS:  A                    PTS:  1

 

12. Which of the following equations (not balanced) represents an oxidation-reduction process?

a.	AgNO3 + NaCl ® AgCl + NaNO3	c.	C2H4 + O2 ® CO2 + H2O
b.	C + O2 ® CO2	d.	more than one response is correct

 

 

ANS:  D                    PTS:  1

 

13. What is the oxidation number of Cl in HClO₃?

a.

+2

b.

+3

c.

+4

d.

+5

 

 

ANS:  D                    PTS:  1

 

14. What is the oxidation number of Br in ?

a.

-1

b.

+1

c.

+2

d.

+3

 

 

ANS:  D                    PTS:  1

 

15. What is the oxidation number of Mn in KMnO₄?

a.

+9

b.

+5

c.

+7

d.

+4

 

 

ANS:  C                    PTS:  1

 

16. In which of the following does an element have an oxidation number of +4?

a.

TiO2

b.

HBr

c.

SO3

d.

 

 

ANS:  A                    PTS:  1

 

17. Which of the following contains the metal with the highest oxidation number?

a.

CaCl2

b.

NaCl

c.

FeCl3

d.

CuCl2

 

 

ANS:  C                    PTS:  1

 

18. What substance is oxidized in the following reaction?

4HCl + MnO₂ ® Cl₂ + 2H₂O + MnCl₂

a.

Cl in HCl

b.

Mn in MnO2

c.

H in HCl

d.

O in MnO2

 

 

ANS:  A                    PTS:  1

 

19. What substance is reduced in the following reaction?

4HCl + MnO₂ ® Cl₂ + 2H₂O + MnCl₂

a.

Cl in HCl

b.

Mn in MnO2

c.

H in HCl

d.

O in MnO2

 

 

ANS:  B                    PTS:  1

 

20. What is the oxidizing agent in the following reaction?

4HCl + MnO₂ ® Cl₂ + 2H₂O + MnCl₂

a.

HCl

b.

Cl2

c.

MnO2

d.

MnCl2

 

 

ANS:  C                    PTS:  1

 

21. What is the reducing agent in the following reaction?

4HCl + MnO₂ ® Cl₂ + 2H₂O + MnCl₂

a.

HCl

b.

Cl2

c.

MnO2

d.

MnCl2

 

 

ANS:  A                    PTS:  1

 

22. Which of the following is a decomposition reaction?

a.	SO2 + O2 ® 2SO3	c.	2H2O2 ® 2H2O + O2
b.	2C2H2 + 5O2 ® 4CO2 + 2H2O	d.	AgNO3 + NaCl ® AgCl + NaNO3

 

 

ANS:  C                    PTS:  1

 

23. Which of the following is a combination reaction?

a.	SO2 + O2 ® 2SO3	c.	2H2O2 ® 2H2O + O2
b.	2C2H2 + 5O2 ® 4CO2 + 2H2O	d.	AgNO3 + NaCl ® AgCl + NaNO3

 

 

ANS:  A                    PTS:  1

 

24. Which of the following is a single replacement reaction?

a.	CuO + H2 ® Cu + H2O	c.	SO2 + H2O ® H2SO3
b.	HBr + KOH ® H2O + KBr	d.	2HI ® I2 + H2

 

 

ANS:  A                    PTS:  1

 

25. Which of the following is a double replacement reaction?

a.	CuO + H2 ® Cu + H2O	c.	SO2 + H2O ® H2SO3
b.	HBr + KOH ® H2O + KBr	d.	2HI ® I2 + H2

 

 

ANS:  B                    PTS:  1

 

26. Barium sulfate is often ingested to aid in the diagnosis of GI tract disorders. The equation for its production is Ba²⁺ + SO ® BaSO₄(s). What type of equation is this?

a.	a total ionic equation	c.	an oxidation-reduction equation
b.	a full equation	d.	a net ionic equation

 

 

ANS:  D                    PTS:  1

 

27. Which ions in the following reaction would be classified as spectator ions?

Zn + 2H⁺ + 2Cl ® Zn²⁺ + 2Cl^– + H₂

a.	Zn2+	c.	Cl–
b.	H+	d.	More than one response is correct.

 

 

ANS:  C                    PTS:  1

 

28. Which ions will appear in the total ionic equation for the following reaction?

a.	and	c.	, , and H+
b.	and	d.	, , , and

 

 

ANS:  D                    PTS:  1

 

29. For the reaction of HCl and NaOH, which of the following type of chemicals will appear in the net equation?

a.

weak acid

b.

weak base

c.

salt

d.

water

 

 

ANS:  D                    PTS:  1

 

30. In the equation for an endothermic reaction, the word “heat” appears

a.	on the right side.	c.	on both sides.
b.	on the left side.	d.	on neither side.

 

 

ANS:  B                    PTS:  1

 

31. The energy involved in chemical reactions

a.	always appears as heat.	c.	always appears as electricity.
b.	always appears as light.	d.	can take many forms.

 

 

ANS:  D                    PTS:  1

 

32. Given the equation 2CO + O₂ ® 2CO₂, how many grams of CO₂ form if 34.0 grams of CO are combined with excess oxygen?

a.

53.4

b.

21.6

c.

145

d.

107

 

 

ANS:  A                    PTS:  1

 

33. Oxygen can be prepared in the lab by heating potassium chlorate in the presence of a catalyst. The reaction is 2KClO₃ ®  2KCl + 3O₂. How many moles of O₂ could be obtained from one mole of KClO₃?

a.

1.5

b.

3.0

c.

1.0

d.

2.0

 

 

ANS:  A                    PTS:  1

 

34. The Haber Process is a method for the production of ammonia, an important chemical intermediate. The reaction for this process is: N₂ + 3H₂ ® 2NH₃. When the equation is correctly interpreted in terms of moles, how many moles of H₂ will react with one mole of N₂?

a.

1

b.

2

c.

3

d.

6

 

 

ANS:  C                    PTS:  1

 

35. How many grams of N₂ are required to completely react with 3.03 grams of H₂ for the following balanced chemical equation?      N₂ + 3H₂ ® 2NH₃

a.

1.00

b.

6.00

c.

14.0

d.

28.0

 

 

ANS:  C                    PTS:  1

 

36. The Haber Process is a method for the production of ammonia, an important chemical intermediate. The reaction for this process is

 N₂ + 3H₂ ® 2NH₃

According to the mole interpretation, how many grams of NH₃ could be produced by the complete reaction of 2.80 grams of N₂ and excess H₂?

a.

34.0

b.

17.0

c.

3.10

d.

3.40

 

 

ANS:  D                    PTS:  1

 

37. In the reaction 2H₂O ® 2H₂ + O₂, 2.0 mol water will produce how many grams of O₂?

a.

16

b.

32

c.

36

d.

64

 

 

ANS:  B                    PTS:  1

 

38. In the reaction 2CH₄ + O₂ ® 2CO + 4H₂, how many molecules of CO will be produced by the complete reaction of 1.60 grams of CH₄?

a.

12.0 ´ 1023

b.

3.01 ´ 1022

c.

6.02 ´ 1022

d.

2.00

 

 

ANS:  C                    PTS:  1

 

39. If 5 grams of CO and 5 grams of O₂ are combined according to the reaction, which is the limiting reagent?  2CO + O₂ ® 2CO₂

a.

CO2

b.

O2

c.

CO

d.

CO and O2

 

 

ANS:  C                    PTS:  1

 

40. Acetylene, C₂H₂, burns according to the following reaction: C₂H₂+5O₂ ® 4CO₂+2H₂O. Suppose 1.20 g of C₂H₂ is mixed with 3.50 g of O₂ in a closed, steel container, and the mixture is ignited. What substances will be found in the mixture left when the burning is complete?

a.	CO2 and H2	c.	C2H2, CO2, and H2O
b.	O2, CO2, and H2O	d.	O2, C2H2, CO2, and H2O

 

 

ANS:  C                    PTS:  1

 

41. Suppose 2.43 g of magnesium is reacted with 3.20 g of oxygen: 2Mg + O₂ ® 2MgO. How many grams of MgO will be produced?

a.

5.63

b.

1.27

c.

8.06

d.

4.03

 

 

ANS:  D                    PTS:  1

 

42. Tincture of iodine is an antiseptic. Which of the following is another antiseptic?

a.	5% sodium hypochlorite	c.	ozone
b.	3% hydrogen peroxide	d.	All are antiseptics

 

 

ANS:  B                    PTS:  1

 

43. What are coefficients needed to balance the following reaction?

2 CH₄ + ____ O₂ ® ____ CO₂ + ____ H₂O

a.

8,2,4

b.

4,1,2

c.

4,2,4

d.

none of these

 

 

ANS:  C                    PTS:  1

 

44. According to the law of conservation of matter, which of the following may NEVER occur as a result of a chemical reaction?

a.	creation of new chemical species.	c.	rearranged to form new substances.
b.	reaction of starting materials.	d.	reduction in total mass.

 

 

ANS:  D                    PTS:  1

 

45. Which is not a meaning of oxidation?

a.	to gain electrons	c.	to combine with oxygen
b.	to lose hydrogen	d.	to lose electrons

 

 

ANS:  A                    PTS:  1

 

46. The modern definition of oxidation is a process

a.	involving a reaction with oxygen.	c.	in which electrons are gained.
b.	in which hydrogen is gained.	d.	none of the choices.

 

 

ANS:  D                    PTS:  1

 

47. Tests are to be conducted on new anti-cancer drug and you are to prepare a fresh supply for the human subject studies. You discover that you were able to produce 1.345 g of this substance although it was theoretically possible to make 1.433 g. What was the percent yield for this synthesis?

a.

93.859 %

b.

93.86 %

c.

94 %

d.

0.9386 %

 

 

ANS:  B                    PTS:  1

 

48. A percentage yield less than 100% is often obtained in a reaction. What is(are) the reason for obtaining less than theoretically predicted?

a.	Side reactions occurred	c.	reaction did not go to completion
b.	poor laboratory technique	d.	all of the choices

 

 

ANS:  D                    PTS:  1

 

49. A percentage yield greater than 100% has been reported in a scientific paper you are assigned to read. What would be a reasonable explanation for this?

a.	A lack of training of the professor who published the study.
b.	The product was measured more than once.
c.	Small measurement errors could have caused this to occur.
d.	It must be a typographical error since yields can’t exceed 100%.

 

 

ANS:  C                    PTS:  1

 

50. Which of the following types of chemical reaction classes always involve oxidation?

a.	single replacement	c.	combination
b.	double replacement	d.	decomposition

 

 

ANS:  A                    PTS:  1

 

51. When the following equation is balanced, how many oxygen atoms are present on the reactant side of the equation?        C₂H₆ + O₂  ®  CO₂ + H₂O

a.

14

b.

7

c.

3

d.

20

 

 

ANS:  A                    PTS:  1

 

52. When nitrogen (N₂) reacts with sodium (Na), sodium nitride (Na₃N) is formed.  The balanced equation for the reaction would be:

a.		c.
b.		d.

 

 

ANS:  D                    PTS:  1

 

53. The reaction below would be considered  _____ .

CaCO₃ + heat  ®  CaO + CO₂

a.	an endothermic combination.	c.	an endothermic decomposition.
b.	an exothermic combination.	d.	an exothermic decomposition.

 

 

ANS:  C                    PTS:  1

 

54. Which of the following conversion factors would allow one to calculate the amount of PbI₂ produced from a given amount of NaI in the following unbalanced reaction?

Pb(NO₃)₂ + Nal  ®  Pbl₂ + NaNO₃

a.

b.

c.

d.

 

 

ANS:  B                    PTS:  1

 

55. The following would represent what type of chemical reaction?

a.	decomposition.	c.	single replacement.
b.	combination.	d.	double replacement.

 

 

ANS:  C                    PTS:  1

 

56. Automotive car batteries rely on the reaction shown below.  Identify the spectator ion(s).

PbO₂(s) + 4 H⁺(aq) + 2 SO₄^2-(aq) + Pb(s) ® 2 PbSO₄(s) + 2 H₂O(l)

a.	SO42-	c.	H+ and SO42-
b.	H+	d.	There are no spectator ions.

 

 

ANS:  D                    PTS:  1

 

57. What is the assigned oxidation number for molybdenum in aluminum molybdate, Al₂(MoO₄)₃?

a.

+2

b.

+3

c.

+6

d.

+7

 

 

ANS:  C                    PTS:  1

 

58. A container is filled with 4.0 g H₂ and 5.0 g O₂.  The mixture is ignited to produce water according to the following equation.  How much water is produced?

2H₂ + O₂ ® 2H₂O

a.

4.0 g

b.

5.0 g

c.

5.6 g

d.

9.0 g

 

 

ANS:  C                    PTS:  1

 

59. Consider the following chemical equation.  Which substance is oxidized?

BaCl₂ (aq) + H₂SO₄ (aq) ® BaSO₄ (s) + 2HCl (aq)

a.

Ba2+

b.

Cl– and H+

c.

SO42-

d.

none of them

 

 

ANS:  D                    PTS:  1

 

60. The reaction 2KBr + F₂ ® 2KF + Br₂ is an example of a _____  reaction.

a.	spectator	c.	single replacement
b.	metaphysical	d.	double replacement

 

 

ANS:  C                    PTS:  1

 

61. Which of the following phrases can be used to describe the process of reduction?

a.	to gain oxygen	c.	to gain electrons
b.	to combine with hydrogen	d.	to decrease in oxidation number

 

 

ANS:  A                    PTS:  1

 

62. Lycopene, a phytonutrient, has several potential health benefits, including protection against prostate, cervical and pancreatic cancer.  Which of the following is a good source of this substance?

a.

spinach

b.

broccoli

c.

strawberries

d.

tomatoes

 

 

ANS:  D                    PTS:  1

 

63. Air bags serve an important role in providing driver and front-seat passenger protection in the event of an automobile accident.  They rely on several chemical reactions.  Which of the following chemicals is responsible for N₂ production?

a.	sodium azide	c.	silicon dioxide
b.	potassium nitrate	d.	more than one answer is correct.

 

 

ANS:  D                    PTS:  1

 

TRUE/FALSE

 

1. The reaction Mg + 3N₂ ® Mg₃N₂ is correctly balanced as written.

 

ANS:  F                    PTS:  1

 

2. The reaction Ca + Cl₂ ® CaCl₂ is a redox reaction.

 

ANS:  T                    PTS:  1

 

3. Redox reactions may also be a decomposition reaction.

 

ANS:  T                    PTS:  1

 

4. The oxidation number of iodine in HIO₄ is +6.

 

ANS:  F                    PTS:  1

 

5. In the reaction Zn + Cu(NO₃)₂ ® Cu + Zn(NO₃), the Zn is reduced.

 

ANS:  F                    PTS:  1

 

6. In the reaction CuCl₂ + Fe ® Cu + FeCl₂ the CuCl₂ is the oxidizing agent.

 

ANS:  T                    PTS:  1

 

7. The reaction AgNO₃ + HCl ® AgCl + HNO₃ is a redox reaction.

 

ANS:  F                    PTS:  1

 

8. In an exothermic reaction, heat is liberated to the surroundings.

 

ANS:  T                    PTS:  1

 

9. All redox reactions are exothermic reactions.

 

ANS:  F                    PTS:  1

 

10. The net ionic equation for the reaction H₂SO₄ + NaOH ® Na₂SO₄ + H₂O is

H⁺ + OH ® H₂O.

 

ANS:  T                    PTS:  1

 

11. 2CO + O₂ ® 2CO₂

 

ANS:  F                    PTS:  1

 

12. Products are always on the right side of a chemical equation.

 

ANS:  T                    PTS:  1

 

13. In ionic compounds, metals have a positive oxidation number.

 

ANS:  T                    PTS:  1

 

14. The reducing agent is the substance that is reduced in the reaction.

 

ANS:  F                    PTS:  1

 

15. Some redox reactions involve only oxidation without any reduction.

 

ANS:  F                    PTS:  1

 

16. A net ionic equation may include one or more spectator ions.

 

ANS:  F                    PTS:  1

 

17. The reactions NaOH + HCl ® H₂O + NaCl and Ca(OH)₂ + 2HBr ® 2H₂O + CaBr₂ have the same net ionic equation.

 

ANS:  T                    PTS:  1

 

18. Most reactions give a percent yield of almost 100%.

 

ANS:  F                    PTS:  1

 

19. Water is a product when any inorganic acid reacts with any inorganic base.

 

ANS:  T                    PTS:  1

 

20. The batteries in an automobile contain lead plates, water, PbSO₄ and H₂SO₄. The instructions with a battery charger state that when a car battery is being charged, there must be no flames or sparks. Hydrogen is liberated during the process and might explode on ignition. Therefore, the hydrogen released is an indication that a redox reaction occurs during the charging process.

 

ANS:  T                    PTS:  1

 

21. All redox reactions involve oxygen.

 

ANS:  F                    PTS:  1

 

22. The oxidation number of cesium (Cs) is always +1.

 

ANS:  F                    PTS:  1

 

23. The oxidation number of Cr in K₂CrO₄ is +6.

 

ANS:  T                    PTS:  1

 

24. Integers are used in properly balanced chemical equations because whole moles of substances are needed for a reaction.

 

ANS:  F                    PTS:  1

 

25. In the real world, one should not expect to obtain as much product as can be predicted from the stoichiometric calculation.

 

ANS:  T                    PTS:  1

 

26. While antiseptics and disinfectants are both antibacterials, only an antiseptic should be used on living tissue.

 

ANS:  T                    PTS:  1

 

27. The ultimate source of all energy used by animals is the carbohydrates found in plants.

 

ANS:  F                    PTS:  1