unit 4 practice questions i.reactions: balancing, types questions 1-3 refer to the following: (a)1...
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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
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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
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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
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
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
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
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
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