1

Unit 4 Practice QuestionsI. Reactions: balancing, typesQuestions 1-3 refer to the following:(A) 1(B) 2(C) 3 Cu + HNO3 Cu(NO3)2 + H2O + NO(D) 4(E) 5

1. When the above equation is balanced, what will be the coefficient of Cu?

2. If 6 moles of Cu reacted according to the above equation, what will be the number of moles of NO formed?

3. If Cu(NO3)2 goes into solution as ions, what will be the number of ions into which it will dissociate?

2

Questions 1-3 refer to the following:

(A) H2

(B) NH3

(C) CO2

(D) HCl(E) O2

1. A gas produced by the reaction of zinc with hydrochloric acid

2. A gas combustion product that is heavier than air3. A gas produced by the heating of potassium

chlorate

3

I

One mole of NaCl contains 2 moles of ions

II

NaCl is a stable salt at room temperature

The reaction in which HgO is heated to release O2 is called decomposition

In a decomposition reaction, the original compound is broken apart into equal numbers of atoms

BECAUSE

BECAUSE

4

I

When a hydrocarbon is combusted in air, carbon monoxide is the major product

II

Air contains much more nitrogen than oxygen

A piece of zinc placed in a blue copper solution will displace the copper from the solution, producing copper metal and a colorless Zn2+ solution

Copper is a much more active metal than zinc

BECAUSE

BECAUSE

5

I

A wooden splint is set on fire and blown out, leaving a hot glowing end. When the glowing splint is inserted into a sample of purified CO2 gas, it will reignite into a flame

II

CO2 gas contains oxygenBECAUSE

6

I

AgCl is insoluble in water

II

All chlorides are soluble in water except for those of silver, mercury and lead

Calcium phosphate is a water-soluble compound

All group I ions form water-soluble salts

BECAUSE

BECAUSE

7

The reaction of aluminum with dilute H2SO4 can be classified as

(A) Synthesis(B) Decomposition(C) Single replacement(D) Double replacement

8

What are the simplest whole-number coefficients that balance this equation?

___C4H10 + ___O2 ___CO2 + ___H2O

(A) 1,6,4,2(B) 2,13,8,10(C) 1,6,1,5(D) 3,10,16,20(E) 4,26,16,20

9

If the equation for the reaction below is balanced using the smallest possible whole-number coefficients, then the coefficient for oxygen gas is

___C2H4 + ___O2 ___CO2 + ___H2O

(A) 1(B) 2(C) 3(D) 4(E) 5

10

When the equation below is balanced using the lowest whole-number terms, the coefficient of CO2 is

___C4H10 + ___O2 ___CO2 + ___H2O

(A) 2(B) 4(C) 8(D) 10(E) 13

11

When the equation for the reaction below is balanced, how many moles of NF3 wold be required to react completely with 6 moles of H2O?

___NF3 + ___H2O ___HF + ___NO + ___NO2

(A) 0.5 mole(B) 1 mole(C) 2 moles(D) 3 moles(E) 4 moles

12

Which coefficient balances the reaction given below?

2Ca3(PO4)2 + 6SiO2 + 10C 10CO + P4 + ___CaSiO3

(A) 2(B) 4(C) 5(D) 6(E) 8

13

Which of the following reactions produces a yellow precipitate?

(A) NaOH (s) + HCl (aq) NaCl(aq) + H2O(B) 2NaOH(aq) + BaCl2 (aq) Ba(OH)2 (s) + 2NaCl (aq)(C) Pb(NO3)2 (aq) + 2KI (aq) 2KNO3 (aq) + PbI2 (s)(D) CuO(s) + Mg(s) Cu(s) + MgO (s)(E) 4Fe + 3O2 2Fe2O3

14

When the equation for the reaction shown below is completed and balanced and all coefficients are reduced to lowest whole-number terms, the coefficient of O2 is

___Al + ___O2 ___Al2O3

(A) 1(B) 2(C) 3(D) 4(E) 6

15

What is the sum of the coefficients of the following equation when it is balanced?

___C6H12O6 + ___O2 ___CO2 + ___H2O

(A) 20(B) 38(C) 21(D) 19(E) 18

16

What is the precipitate produced from the double displacement reaction of an aqueous solution of lead(II) nitrate and an aqueous solution of potassium sulfate?

(A) PbSO4

(B) KNO3

(C) K2Pb(D) NO2

(E) SO3

17

The reaction below is classified as a

CH3CO2Na + HClO4 CH3CO2H + NaClO4

(A) Double displacement reaction(B) Synthesis reaction(C) Decomposition reaction(D) Single displacement and decomposition reaction(E) Synthesis and decomposition reaction

18

H2 + Cl2 2HCl

The above reaction is classified as a

(A) Decomposition(B) Double displacement(C) Neutralization(D) Oxidation-reduction(E) Single displacement

19

What is the sum of the coefficients of the products for the following reaction, after balancing?

__K2Cr2O7 + __HCl __KCl + __CrCl3 + __H2O + __Cl2

(A) 10(B) 12(C) 13(D) 14(E) 15

20

Which equation is correctly balanced?

(A) Na + Cl2 2NaCl(B) CH4 + 3O2 CO2 + H2O(C) 2KI + Pb(NO3)2 2KNO3 + PbI2

(D) H2SO4 + KOH K2SO4 + H2O(E) C6H12O6 + 6O2 6CO2 + H2O

21

Which of the following can be classified as a precipitation reaction?

(A) HCl (aq) + NaOH (aq)(B) KBr (aq) + NaCl (aq)(C) AgNO3(aq) + MgCl2(aq)(D) CaCl2 (aq) + KI (aq)(E) NaNO3 (aq) + HC2H3O2 (aq)

22

What would be the stoichiometric coefficient of hydrochloric acid in the following equation?

___Cl2 + ___H2O ___HCl +___HClO3

(A) 1(B) 3(C) 5(D) 10(E) 12

23

When the equation___C2H6 + ___O2 ___CO2 +___H2O

Is competely balanced using the lowest whole number coefficients, the sum of the coefficients will be

(A) 4(B) 9.5(C) 19(D) 15.5(E) 11

24

Which reaction between ions does not form a precipitate?

(A) Ag1+ + Cl1-

(B) Pb2+ + 2I1-

(C) Ca2+ + CO32-

(D) Hg2+ + 2Br1-

(E) Na1+ + OH1-

25

The product formed when oxygen and hydrogen are mixed in a test tube at room temperature is

(A) Hydrogen peroxide(B) Water(C) A base(D) A zwitterion(E) No reaction takes place

26

If the equation for the reaction below is balanced with whole-number coefficients, what is the coefficient for oxygen gas?

___C2H4 + ___O2 ___CO2 + ___H2O

(A) 1(B) 2(C) 3(D) 4(E) 5

27

For a metal atom to replace another kind of metallic ion in a solution, the metal atom must be

(A) A good oxidizing agent(B) Higher in the activity series than the metal in

solution(C) Lower in the electromotive chart than the metal

in solution(D) Equal in activity to the metal in solution

28

How many atoms are represented in the formula Ca3(PO4)2?

(A) 5(B) 8(C) 9(D) 12(E) 13

29

What is the total number of atoms represented in one molecule of (CH3)2NH?

(A) 5(B) 8(C) 9(D) 10(E) 12

30

The chemical symbol Ar could stand for

(A) One mole of argon(B) One atom of argon(C) Both a mole or an atom of argon(D) Neither a mole or an atom of argon(E) One molecule of argon

31

Which salt has a solubility that is different from the other four?

(A) AgCl(B) PbBr2

(C) Ca3(PO4)2

(D) Na2CO3

(E) Al(OH)3

32

The net ionic equation for the reaction between CaCl2 and Na2CO3 to form calcium carbonate and sodium chloride would include all of the following except:

(A) Ca2+

(B) CO32-

(C) 2Na1+

(D) CaCO3

(E) All of the substances above would be in the net ionic equation

33

When most fuels burn, the products include carbon dioxide and

(A) Hydrocarbons(B) Hydrogen(C) Water(D) Hydroxide(E) Hydrogen peroxide

34

Which of the following elements normally exist as monoatomic molecules?

(A) Cl(B) H(C) O(D) N(E) He

35

In this equation:Al(OH)3 + H2SO4 Al2(SO4)3 + H2O

The whole number coefficients of the balanced equation are

(A) 1,3,1,2(B) 2,3,2,6(C) 2,3,1,6(D) 1,3,1,6

36

For the reaction of sodium with water, the balanced equation using the smallest whole numbers has which of the following coefficients?

I. 1II. 2III. 3

(A) I only(B) III only(C) I and II only(D) II and III only(E) I, II, and III

37

The reaction of zinc metal, Zn, and hydrochloric acid, HCl, produces which of the following?

I. H2 (g)II. Cl2 (g)III. Zn2+ (aq)

(A) II only(B) III only(C) I and II only(D) I and III only(E) I, II, and III

38

Which reactions would form at least one solid precipitate as a product? Assume aqueous reactants.

I. AgNO3 + NaCl NaNO3 + AgClII. Pb(NO3)2 + 2KI PbI2 + 2KNO3

III. 2NaOH + H2SO4 Na2SO4 + 2H2O

(A) I only(B) II only(C) III only(D) I and II only(E) II and III only

39

Which of these equations is/are properly balanced?

I. Cl2 + NaBr Br2 + 2NaClII. 2Na + O2 Na2OIII. 2K + 2H2O H2 + 2KOH

(A) I only(B) II only(C) III only(D) I and III only(E) I, II and III

40

One reason for a double displacement reaction to go to completion is that

(A) A product is soluble(B) A product is given off as a gas(C) The products can react with each other(D) The products are miscible

41

I

The percent composition of oxygen in water is 33%

II

One atom of oxygen makes up one-third of the mass of a water molecule

BECAUSE

II. % Composition, Empirical and Molecular Formulas

42

Laboratory results showed the composition of a compound to be 58.81% barium, 13.73% sulfur and 27.46% oxygen. What is the empirical formula?

(A) BaSO4

(B) BaS2O(C) Ba2SO3

(D) BaS2O4

(E) Ba2SO4

43

What is the percent composition of oxygen in C6H12O6 (molar mass = 180)?

(A) 25%(B) 33%(C) 40%(D) 53%(E) 75%

44

A compound was analyzed and found to be composed of 75% carbon and 25% hydrogen. What is the empirical formula of this compound?

(A) C2H4

(B) CH4

(C) CH3

(D) CH2

(E) CH

45

The percent composition by mass of oxygen in BaSO4 is

(A) 233.4%(B) 66.7%(C) 27.4%(D) 58.7%(E) 13.7%

46

Which statement is true about the percent composition by mass in C6H12O6?

(A) Carbon is 6.7% by mass(B) Oxygen is 53.3 % by mass(C) Hydrogen is 12% by mass(D) Carbon is 72% by mass(E) Carbon is 20% by mass

47

What is the approximate percentage composition by mass of the element oxygen in the compound HClO4?

(A) 16%(B) 32%(C) 50%(D) 64%(E) 75%

48

The percent composition of an unknown element X in CH3X is 32%. Which of the following is element X?

(A) H(B) F(C) Cl(D) Na(E) Li

49

A compound’s composition by mass is 50% S and 50% O. What is the empirical formula of this compound?

(A) SO(B) SO2

(C) S2O(D) S2O3

(E) S3O4

50

What percentage of the total mass of KHCO3 is made up by nonmetallic elements?

(A) 17%(B) 83%(C) 61%(D) 20%(E) 50%

51

A compound has a composition of 40% sulfur and 60% oxygen by mass. What is the empirical formula of this compound?

(A) SO(B) S2O3

(C) S2O7

(D) SO3

(E) SO2

52

A hydrocarbon has the empirical formula CH3. A probable molecular formula for this compound could be

(A) C3H3

(B) C2H6

(C) C3H8

(D) C4H8

(E) C5H10

53

What is the percentage by mass of sulfur in H2SO4?

(A) 16%(B) 33%(C) 36%(D) 42%(E) Cannot be determined

54

What is the percent composition by weight of Al in Al2(SO4)3?

(A) 7.9%(B) 31.6%(C) 15.8%(D) 12.7%(E) 22.3%

55

What is the molecular formula of a compound with the empirical formula C3H6O2 and a mass of 148 amu?

(A) C6H12O4

(B) C2H6O2

(C) C9H18O6

(D) C2H3O(E) None of the above

56

What is the percent by mass of silicon in a sample of silicon dioxide?

(A) 21%(B) 33%(C) 47%(D) 54%(E) 78%

57

Which of the following could be the molecular formula for a molecule with an empirical formula of CH2?

(A) CH(B) CH4

(C) C2H2

(D) C2H6

(E) C3H6

58

Which of the following statements about molecular and empirical formulas is/are false?

I. a given compound can have the same

molecular and empirical formulaII. The molecular formula is a whole-number

multiple of the empirical formulaIII. H2O2 represents the empirical formula of

hydrogen peroxide

(A) III only(B) I and II only(C) II and III only(D) I, II, and III(E) I only

59

What is the percentage composition of calcium in calcium hydroxide, Ca(OH)2?

(A) 40%(B) 43%(C) 54%(D) 69%(E) 74%

60

Which of the following compounds contains the greatest percentage of oxygen by weight?

(A) C3H6O5Cl(B) C3H6O2

(C) C5H10O5

(D) C4H8O3

(E) They are all equal

61

What is the mass of nitrogen in a 50.0 g sample of sodium nitrite (NaNO2)?

(A) 20.2 g(B) 16.4 g(C) 10.1 g(D) 8.23 g(E) 23.4 g

62

In the laboratory, a sample of hydrated salt was heated at 110oC for 30 minutes until all the water was driven off. The data were as follows:

Mass of hydrate before heating = 250 gMass of hydrate after heating = 160 g

From these data, what was the percent of water by mass in the original sample?

(A) 26.5(B) 36(C) 47(D) 56(E) 90

63

What is the approximate percentage of oxygen in the formula mass of Ca(NO3)2?

(A) 28(B) 42(C) 58(D) 68(E) 84

64

What formulas could represent the empirical formula and the molecular formula of a given compound?

(A) CH2O and C4H6O4

(B) CHO and C6H12O6

(C) CH4 and C5H12

(D) CH2 and C3H6

(E) CO and CO2

65

Analysis of a gas gave: C = 85.7% and H = 14.3%. If the formula mass of this gas is 42, what are the empirical formula and the true formula?

(A) CH and C4H4

(B) CH2 and C3H6

(C) CH3 and C3H9

(D) C2H2 and C3H6

(E) C2H4 and C3H6

66

In synthesizing MgO from a Mg strip burned in a crucible, which of the following is NOT true?

(A) The initial strip of Mg should be cleaned(B) The lid of the crucible should fit tightly to

exclude oxygen(C) The heating of the covered crucible should

continue until the Mg is fully reacted(D) The crucible, lid and contents should be cooled

to room temperature before measuring their mass

(E) When the Mg appears to be fully reacted, the crucible lid should be partially removed and heating continued

67

A compound whose molecular mass is 90.0 grams contains 40.0% carbon, 6.67% hydrogen, and 53.33% oxygen. What is the true formula of the compound?

(A) C2H2O4

(B) CH2O4

(C) C3H6O(D) C3HO3

(E) C3H6O3

68

If the simplest formula of a substance is CH2 and its molecular mass is 56, what is its true formula?

(A) CH2

(B) C2H4

(C) C3H4

(D) C4H8

(E) C5H10

69

III. Moles, Conversions and Stoichiometry

Questions 1-4 refer to the following:

(A) 9.03 x 1023 molecules(B) 44.8 liters(C) 3.5 moles(D) 6.0 grams(E) 3.01 x 1023 atoms

1. 0.25 moles of O2 at STP2. 3.0 moles of H2 at STP3. 56 grams of N2 at STP4. 96.0 grams of SO2 at STP

70

I

Two liters of CO2 can be produced by 1 gram of carbon burning completely

II

The amount of gas evolved in a chemical reaction can be determined by using the mole relationship of the coefficients in the balanced equation

One mole of CO2 has a greater mass than 1 mole of H2O

The molecular mass of CO2 is greater than the molecular mass of H2O

BECAUSE

BECAUSE

71

I

There are 3 moles of atoms in 18 grams of water

II

There are 6 x 1023 atoms in 1 mole

The complete electrolysis of 45 grams of water will yield 40 grams of H2 and 5 grams of O2

Water is composed of hydrogen and oxygen in a ratio of 8:1 by mass

BECAUSE

BECAUSE

72

I

When 2 liters of oxygen gas react with 2 liters of hydrogen completely, the limiting factor is the volume of the oxygen

II

The coefficients in balanced equations of gaseous reactions give the volume relationships of the gases

If equal masses of sodium metal and chlorine gas are allowed to react, some sodium will be leftover after all the chlorine is used up

The reaction requires twice as many atoms of chlorine as sodium

BECAUSE

BECAUSE

73

In the following reaction, how many liters of SO2 at STP will result from the complete burning of pure sulfur in 8 liters of oxygen?

S + O2 SO2

(A) 1(B) 4(C) 8(D) 16(E) 32

74

If 80 grams of Al and 80 grams of Fe2O3 are combined, what is the maximum number of moles of Fe that can be produced?

2Al + Fe2O3 Al2O3 + 2Fe

(A) 1(B) 4(C) 8(D) 16(E) 32

75

Acetylene, used as a fuel in welding torches, is produced in a reaction between calcium carbide and water:

CaC2 + 2H2O Ca(OH)2 + C2H2

How many grams of C2H2 are formed from 0.400 moles of CaC2?

(A) 0.400(B) 0.800(C) 4.00(D) 10.4(E) 26.0

76

Aspirin (C9H8O4) is prepared by reacting salicylic acid (C7H6O3) and acetic anhydride (C4H6O3)

C7H6O3 + C4H6O3 C9H8O4 + C2H4O2

How many moles of salicylic acid should be used to prepare six 5-grain aspirin tablets? (1g = 15.5 grains)

(A) 0.01(B) 0.1(C) 1.0(D) 2.0(E) 31.0

77

Ag(NH3)2+ Ag+ + 2NH3

If 5.8 g of Ag(NH3)2+ yields 1.4 g of ammonia, how

many moles of silver are produced?

(A) 4.4(B) 5.8(C) 0.041(D) 0.054(E) 7.2

78

How many grams of O2 will it take to oxidize 88 grams of C3H8 to CO and H2O?

(A) 32(B) 64(C) 112(D) 166(E) 224

79

How many molecules are in a 36.5 g sample of SF6 gas?

(A) 1.51 x 1022

(B) 1.06 x 1022

(C) 1.51 x 1023

(D) 1.06 x 1024

(E) 1.51 x 10-24

80

What would be the approximate weight of 1.204 x 1024 bromine atoms?

(A) 80 grams(B) 120 grams(C) 160 grams(D) 180 grams(E) 200 grams

81

Chlorophyll, a green pigment involved in the light reactions of photosynthesis, consists of 2.4312 percent Mg. If you are given a 100 g sample of chlorophyll, how many atoms of Mg will it contain?

(A) 6.02 x 1022 atoms(B) 6.02 x 1023 atoms(C) 6.02 x 1024 atoms(D) 6.02 x 1025 atoms(E) None of the above

82

Water is formed by the addition of 4.0 g of H2 to an excess of O2. If 27 g of H2O is recovered, what is the percent yield for the reaction?

(A) 25%(B) 50%(C) 75%(D) 100%(E) Cannot be determined

83

In the reaction 2SO2 + O2 2SO3, 0.25 mole of sulfur dioxide is mixed with 0.25 mole of oxygen and allowed to react. What is the maximum number of moles of SO3 that can be produced?

(A) 0.0625 mole(B) 0.125 mole(C) 0.25 mole(D) 0.5 mole(E) 1.0 mole

84

The volume of water vapor required to produce 44.8 liters of oxygen by the below reaction is

2H2O 2H2 + O2

(A) 11.2 L(B) 22.4 L(C) 44.8 L(D) 89.6 L(E) 100.0 L

85

Given this reaction that occurs in plants:

6CO2 + 6H2O C6H12O6 + 6O2

If 54 grams of water are consumed by the plant, how many grams C6H12O6 can be made? Assume an unlimited supply of carbon dioxide for the plant to consume as well.

(A) 54 grams(B) 180 grams(C) 540 grams(D) 3 grams(E) 90 grams

86

According to the reaction:

Pb + S PbSWhen 20.7 grams of lead are reacted with 6.4 grams of sulfur

(A) There will be an excess of 20.7 grams of lead(B) The sulfur will be in excess by 3.2 grams(C) The lead and sulfur will react completely

without any excess reactants(D) The sulfur will be the limiting factor in the

reaction(E) There will be an excess of 10.3 grams of lead

87

Given a 4-gram sample of each H2(g) and He(g), each in separate containers, which of the following statements is true? (assume STP)

(A) The sample of hydrogen gas will occupy 44.8 liters and the sample of helium will contain 6.02 x 1023 molecules

(B) The sample of hydrogen gas will occupy 22.4 liters and sample of helium will contain 3.02 x 1023 molecules

(C) The sample of hydrogen gas will occupy 44.8 liters and the sample of helium will contain 1.202 x 1024 molecules

(D) The sample of helium will occupy 44.8 liters and the sample of hydrogen gas will contain 6.02 x 1023 molecules

(E) None of the above statements is correct.

88

If 48.6 grams of magnesium are placed in a container with 64 grams of oxygen gas and the reaction below proceeds to completion, what is the mass of MgO (s) produced?

2Mg + O2 2MgO

(A) 15.4 grams(B) 32.0 grams(C) 80.6 grams(D) 96.3 grams(E) 112 grams

89

Given the reaction at STP:

Mg + 2HCl MgCl2 + H2

How many liters of H2 can be produced from the reaction of 12.15 grams of Mg with excess HCl?

(A) 2.0 liters(B) 4.0 liters(C) 11.2 liters(D) 22.4 liters(E) 44.8 liters

90

A sample of a gas at STP contains 3.01 x 1023 molecules and has a mass of 20.0 grams. This gas would

(A) Have a molar mass of 20.0 grams/mole and occupy 11.2 liters

(B) Occupy 22.4 liters and have a molar mass of 30.0 grams/mole

(C) Occupy 22.4 liters and have a molar mass of 20.0 grams/mole

(D) Have a molar mass of 40.0 grams/mole and occupy 33.6 liters

(E) Have a molar mass of 40.0 grams/mole and occupy 11.2 liters

91

2NO + 2H2 N2 + 2H2O

Which of the following statements is true regarding the reaction given above?

(A) If 1 mole of H2 is consumed, 0.5 mole of N2 is produced

(B) If 1 mole of H2 is consumed, 0.5 mole of H2O is produced

(C) If 0.5 mole of H2 is consumed, 1 mole of N2 is produced

(D) If 0.5 mole of H2 is consumed, 1 mole of NO is consumed

(E) If 0.5 mole of H2 iscondsumed, 1 mole of H2O is produced

92

Propane and oxygen react according to the equation: C3H8 + 5O2 3CO2 + 4H2O

How many grams of water can be produced from the complete combustion of 2.0 moles of C3H8?

(A) 144.0(B) 82.0(C) 8.0(D) 44.8(E) 22.4

93

Carbon and oxygen react to form carbon dioxide according to the reaction: C + O2 CO2

How much carbon dioxide can be formed from the reaction of 36 grams of carbon with 64 grams of oxygen gas?

(A) 36 grams(B) 64 grams(C) 28 grams(D) 132 grams(E) 88 grams

94

How many grams of Fe2O3 can be formed form the rusting of 446 grams of Fe according to the reaction: 4Fe + 3O2 2Fe2O3

(A) 320 grams(B) 223 grams(C) 159 grams(D) 480 grams(E) 640 grams

95

Sodium and chlorine react according to the following reaction: 2Na + Cl2 2NaCl

If the reaction starts with 5.0 moles of Na and 3.0 moles of Cl2, then which statement below is true?

(A) Cl2 is the excess reagent and 5.0 moles of NaCl will be produced

(B) Na is the excess reagent and 2.5 moles of NaCl will be produced

(C) There will be an excess of 2.0 moles of Na(D) Na is the limiting reagent and 2.0 moles of NaCl

will be produced(E) Cl2 is the excess reagent and 2.0 moles of NaCl

will be produced

96

According to the reaction: 3H2 + N2 2NH3

How many grams of hydrogen gas and nitrogen gas are needed to make exactly 68 grams of ammonia?

(A) 2 grams of hydrogen gas and 28 grams of nitrogen gas

(B) 3 grams of hydrogen gas and 1 gram of nitrogen gas

(C) 12 grams of hydrogen gas and 56 grams of nitrogen gas

(D) 102 grams of hydrogen gas and 34 grams of nitrogen gas

(E) 6 grams of hydrogen gas and 2 grams of nitrogen gas

97

What is the mass of 3.0 x 1023 atoms of neon gas?

(A) 0.50 grams(B) 1.0 grams(C) 5.0 grams(D) 40.0 grams(E) 10.0 grams

98

Which of the following statements is the most accurate with regard to the significance of Avogadro’s number, 6.02 x 1023?

(A) It is the conversion factor between grams and atomic mass units

(B) It is a universal physical constant just as the speed of light

(C) It is the number of particles that is required to fill a 1-liter container

(D) It is the inverse diameter of an H atom(E) It is the number of electrons in the universe

99

In the laboratory a student was determining the formula for the hydrate of barium chloride, BaCl2. The student heated the sample in the crucible strongly for 10 minutes. The mass data is provided below:

mass of crucible and cover 31.623 gmass of crucible, cover and 33.632 g

sample prior to heatingmass of crucible, cover and 33.376 g

sample after heatingAfter the heating, how many moles of water were removed from the sample?

(A) 0.0142 moles(B) 0.0974 moles(C) 0.112 moles(D) 0.256 moles(E) 1.85 moles

100

How many grams of hydrogen gas can be produced from the following reaction if 65 grams of zinc and 65 grams of HCl are present in the reaction?

Zn + 2HCl ZnCl2 + H2

(A) 1.0(B) 1.8(C) 3.6(D) 7.0(E) 58

101

If 60. grams of NO is reacted with sufficient O2 to form NO2 that is removed during the reaction, how many grams of NO2 can be produced?

(A) 46(B) 60.(C) 92(D) 120(E) 180

102

What volume of gas, in liters, would 1.5 moles of hydrogen occupy at STP?

(A) 11.2(B) 22.4(C) 33.6(D) 44.8(E) 67.2

103

A gas at STP that contains 6.02 x 1023 atoms and forms diatomic molecules will occupy

(A) 11.2 L(B) 22.4 L(C) 33.6 L(D) 67.2 L(E) 1.06 qt

104

5.00 liters of gas at STP have a mass of 12.5 grams. What is the molar mass of the gas?

(A) 12.5 g/mol(B) 25.0 g/mol(C) 47.5 g/mol(D) 56.0 g/mol(E) 125 g/mol

105

How many moles of CaO are needed to react with an excess of water to form 370 grams of calcium hydroxide?

(A) 1.0(B) 2.0(C) 3.0(D) 4.0(E) 5.0

106

When 1 mole of chlorine gas reacts completely with excess KBr solution, as shown below, the products obtained are

Cl2 + 2Br-

(A) 1 mol of Cl- ions and 1 mol of Br-(B) 1 mol of Cl- ions and 2 mol of Br-(C) 1 mol of Cl- ions and 1 mol of Br2

(D) 2 mol of Cl- ions and 1 mol of Br2

(E) 2 mol of Cl- ions and 2 mol of Br2

107

What mass of CaCO3 is needed to produce 11.2 liters of CO2 at STP when the calcium carbonate is reacted with an excess amount of hydrochloric acid?

(A) 25.0 g(B) 44.0 g(C) 50.0 g(D) 100. g(E) None of the above

108

What is the approximate formula mass of Ca(NO3)2?

(A) 70(B) 82(C) 102(D) 150(E) 164

109

If 10 liters of CO gas react with sufficient oxygen for a complete reaction, how many liters of CO2 gas are formed?

(A) 5(B) 10(C) 15(D) 20(E) 40

110

If 49 grams of H2SO4 react with 80.0 grams of NaOH, how much reactant will be left over after the reaction is complete?

(A) 24.5 g H2SO4

(B) None of either compound(C) 20. g NaOH(D) 40. g NaOH(E) 60. g NaOH

111

Given one mole of CH4 (g) at STP. Which statements are true?

I. There are 6.02 x 1023 molecules presentII. The sample will occupy 22.4 LIII. The sample will weigh 16 g

(A) I only(B) II only(C) I and III only(D) II and III only(E) I, II, and III

112

What is the molar mass of Ca3(PO4)2?

(A) 310 grams/mole(B) 154 grams/mole(C) 67 grams/mole(D) 83 grams/mole(E) 115 grams/mole

113

If the density of a diatomic gas at STP is 1.43 g/L, what is the gram molecular mass of the gas?

(A) 14.3 g(B) 32.0 g(C) 48.0 g(D) 64.3 g(E) 224 g

114

From 2 moles of KClO3 how many liters of O2 can be produced at STP by decomposition of tall the KClO3?

(A) 11.2(B) 22.4(C) 33.6(D) 44.8(E) 67.2

115

How many atoms are in one mole of water?

(A) 3(B) 54(C) 6.02x1023

(D) 2(6.02x1023)(E) 3(6.02x1023)

116

Four grams of hydrogen gas at STP contain

(A) 6.02x1023 atoms(B) 12.04x1023 atoms(C) 12.04x1046 atoms(D) 1.2x1023 molecules(E) 12.04x1023 molecules

117

How many liters of O2 can be produced by completely decomposing 2.00 moles of KClO3?

(A) 11.2(B) 22.4(C) 33.6(D) 44.8(E) 67.2

118

If the molecular mass of NH3 is 17, what is the density of this compound at STP?

(A) 0.25 g/L(B) 0.76 g/L(C) 1.52 g/L(D) 3.04 g/L(E) 9.11 g/L

119

How many grams of sulfur are present in 1 mole of H2SO4?

(A) 2(B) 32(C) 49(D) 64(E) 98

120

What is the approximate mass, in grams, of 1 liter of nitrous oxide, N2O, at STP?

(A) 1(B) 2(C) 11.2(D) 22(E) 4

121

What is the molar mass of CaCO3?

(A) 68 g/mol(B) 75 g/mol(C) 82 g/mol(D) 100 g/mol(E) 116 g/mol

122

What volume, in liters, will be occupied at STP by 4 grams of H2?

(A) 11.2(B) 22.4(C) 33.6(D) 44.8(E) 56.0

123

What volume, in liters, of NH3 is produced when 22.4 liters of N2 are made to combine completely with a sufficient quantity of H2 under appropriate conditions?

(A) 11.2(B) 22.4(C) 44.8(D) 67.2(E) 89.6

124

What volume, in liters, of SO2 will result from the complete burning of 64 grams of sulfur?

(A) 2.0(B) 11.2(C) 44.8(D) 126(E) 158

125

How many grams of CO2 can be prepared from 150 grams of calcium carbonate reacting with an excess of hydrochloric acid solution?

(A) 11(B) 22(C) 33(D) 44(E) 66

126

What is the mass, in grams, of 1 mole of

KAl(SO4)2 .12H20?

(A) 132(B) 180(C) 394(D) 474(E) 516

127

What mass of aluminum will be completely oxidized by 2 moles of oxygen at STP?

(A) 18 g(B) 37.8 g(C) 50.4 g(D) 72.0 g(E) 100.8 g

128

In this reaction:CaCO3 + 2HCl CaCl2 + H2O + CO2

If 4.0 moles of HCl are available to the reaction with an unlimited supply of CaCO3, how many moles of CO2 can be produced at STP?

(A) 1.0(B) 1.5(C) 2.0(D) 2.5(E) 3.0

129

The following reaction occurs at STP:2H2O 2H2 + O2

How many liters of hydrogen gas can be produced by the breakdown of 72 grams of water?

(A) 5.6 liters(B) 11.2 liters(C) 22.4 liters(D) 44.8 liters(E) 89.6 liters

130

A sample of a gas at STP contains 3.01 x 1023 molecules and has a mass of 22.0 grams. This gas is most likely

(A) CO2

(B) O2

(C) N2

(D) CO(E) NO

131

The number of oxygen atoms in 0.50 mole of Al2(CO3)3 is

(A) 4.5 x 1023

(B) 9.0 x 1023

(C) 3.6 x 1024

(D) 2.7 x 1024

(E) 5.4 x 1024

132

4.0 grams of hydrogen are ignited with 4.0 grams of oxygen. How many grams of water can be formed?

(A) 0.50(B) 2.5(C) 4.5(D) 8.0(E) 36