Deck 6: Chemical Reactions: Mole and Mass Relationships

Question 1

How many molecules are there in 3.00 moles of NH₃?

A)1.00
B)3.00
C)17.00
D)1.20 × 10²⁴
E)1.81 × 10²⁴

Answer 1

1.81 × 10²⁴

Question 2

42.0 g Cl₂ contains ________ molecules Cl₂.

A)1.18
B)3.57 × 10²³
C)3.57 × 10²³.
D)1.78 × 10²³
E)0.592

Answer 2

3.57 × 10²³

Question 3

Which statement based on the mole concept is not correct?

A)The molar mass of a diatomic element is its atomic weight times two.
B)The number of atoms in one mole of platinum is the same as the number of atoms in one mole of uranium.
C)One mole of sodium chloride,NaCl,contains the same number of ions as one mole of calcium sulfate,CaSO₄.
D)One mole of methane,CH₄,contains the same number of atoms as one mole of carbon dioxide,CO₂.
E)One mole of bromine,Br₂,contains the same number of molecules as one mole of propane,C₃H₈.

Answer 3

One mole of methane,CH₄,contains the same number of atoms as one mole of carbon dioxide,CO₂.

Question 4

The formula weight of Al₂(SO₄)₃ is ________ grams.

A)214.14
B)278.02
C)315.14
D)342.14
E)450.14

Question 5

Calculate the number of moles of aspirin,C₉H₈O₄,in a 4.0 gram tablet.

A)2.2 × 10^-4
B)2.2
C)4.6 × 10^-3
D)0.022

Question 6

Which quantity contains Avogadro's number of molecules?

A)8.8 g CO₂
B)34 g of NH₃
C)9 g of H₂O
D)98 g of H₂SO₄

Question 7

The molar mass of butane,C₄H₁₀,is ________ grams.

A)22.01
B)49.05
C)52.08
D)58.12
E)68.24

Question 8

How many molecules are present in 1.36 g of AgNO₃?

A)3.84 × 10^-22
B)4.82 × 10²¹
C)1.36 × 10²³
D)7.52 × 10²⁵

Question 9

The molar mass of Fe(OH)₃ is ________ g.

A)72.86
B)74.88
C)89.87
D)104.86
E)106.87

Question 10

A thimble of water contains 4.0 × 10²¹ molecules.The number of moles of H₂O is:

A)2.4 × 10⁴⁵
B)6.6 × 10^-3
C)6.6 × 10^-23
D)2.4 × 10²³
E)2.4 × 10^-23

Question 11

How many molecules are present in 3.25 mol of C₂H₆O?

A)3.25
B)46.0
C)1.85 × 10²³
D)6.02 × 10²³
E)1.96 × 10²⁴

Question 12

105 g of MgCl₂ contains ________ mol MgCl₂.

A)105
B)6.62 × 10²³
C)1.10
D)1.76
E)1.06 × 10²⁴

Question 13

The formula weight of ammonium carbonate, (NH₄)₂CO₃,is ________ amu.

A)64.11
B)82.10
C)96.09
D)120.13
E)180.17

Question 14

The formula weight of copper(II)chloride is ________ g.

A)98.90
B)133.00
C)134.45
D)162.53
E)197.80

Question 15

Which statement concerning the mole is not correct?

A)The molar mass of any compound is equal to its molecular weight in grams.
B)A mole of metal contains N_A atoms of that metal.
C)A mole of any compound contains one mole of each kind of atom found in that compound.
D)A mole of a diatomic element contains 2 × N_A moles of atoms of the element.
E)All of these statements are correct.

Question 16

How many molecules are present in 4.25 mol of CCl₄?

A)9.26 × 10²⁵
B)2.56 × 10²⁴
C)653.69
D)153.81
E)36.91

Question 17

The molecular weight of PCl₃ is ________ amu.

A)66.42
B)136.00
C)137.33
D)139.00
E)199.26

Question 18

Which statement concerning the mole concept is not true?

A)The molar mass of a metal is its atomic weight expressed in grams.
B)The mole concept makes a connection between the mass of a substance and the number of particles or units of that substance.
C)One mole of any compound contains one mole of atoms.
D)One mole of sodium contains the same number of atoms as one mole of carbon.
E)One mole of water contains the same number of molecules as one mole of ammonia.

Question 19

The number of grams in 0.350 mol of Na is ________.

A)0.350
B)8.05
C)11.0
D)23.0
E)65.7

Question 20

50.0 g of Cl₂ contains ________ mol Cl₂.

A)50.0
B)1775
C)0.705
D)1.41
E)4.24 × 10²³

Question 21

Determine the number of moles of water produced when one mole of NH₃ reacts according to the balanced reaction shown.
4 NH₃ + 5 O₂ → 4 NO + 6 H₂O

A)1.00
B)1.25
C)1.50
D)0.67
E)1.33

Question 22

The percentage yield of a reaction can best be described as the ________ times 100%.

A)amount of product you could make if the reaction went to completion
B)total amount of materials involved in a reaction
C)amount of desired product divided by the amount of unwanted product
D)amount of product obtained divided by the maximum possible amount of product
E)amount of reactants left over divided by the original amounts

Question 23

In the reaction shown,how many moles of HCl are needed to react with 2.4 moles of Al?
2 Al + 6 HCl → 2 AlCl₃ + 3 H₂

A)0.8
B)1.3
C)4.8
D)6.4
E)7.2

Question 24

How many grams of C will be consumed when 5.00 grams of Na₂SO₄ react according to the balanced reaction shown?
Na₂SO₄ + 2 C → Na₂S + 2 CO₂

A)0.038 g
B)0.211 g
C)0.844 g
D)1.69 g
E)17.1 g

Question 25

In the balanced reaction shown,the mole ratio of Fe₂S₃ to O₂ is
Fe₂S₃ + 4 O₂ → 2 FeO + 3 SO₂

A)5 to 5.
B)1 to 4.
C)4 to 1.
D)1 to 2.
E)4 to 3.

Question 26

Interpret in words the equation:
P₄O₁₀ (s)+ 6 H₂O (l)→ 4 H₃PO₄ (aq)

A)One mole of solid tetraphosphorus decaoxide reacts with six moles of liquid water to produce four moles of phosphoric acid solution.
B)Zero moles of solid phosphoric oxide dissolve in six moles of water to produce four moles of phosphorous acid.
C)One mole of phosphorus(X)oxide combines with six moles of water to produce four moles of solution of hydrogen phosphate.
D)Four moles of solid phosphorus,five moles of diatomic oxygen gas,and six moles of liquid water react together to produce four moles of phosphoric acid in solution.
E)Four atoms of phosphorus,16 atoms of oxygen,and 12 atoms of hydrogen rearrange to produce four molecules of phosphoric acid.

Question 27

In the reaction shown,what is the mole ratio that would be used to determine the number of moles of H₂ that would be produced when 3.5 moles of AlCI₃ are produced?
2 Al + 6 HCl → 2 AlCI₃ + 3 H₂

A)

B)

C)

D)

E)

Question 28

Consider the reaction N₂ (g)+ O₂ (g)→ 2 NO (g).
a.How many g NO can be produced when 25.0 g of nitrogen reacts?
b.How many g NO can be produced when 25.0 g of oxygen reacts?
c.Based on your answers in a and b,predict the amount of NO that can be produced when 25.0 g nitrogen is reacted with 25.0 g of oxygen.
d.Explain the reasoning used in part c.

Question 29

The number of grams in 2.65 mol of SO₂ is

A)2.65.
B)64.1.
C)24.2.
D)170.
E)1.60 × 10²⁴.

Question 30

How many grams of fluorine are required to produce 20.0 grams of FeF₃ from the reaction shown?
2 Fe + 3F₂ → 2 FeF₃

A)4.49 g
B)5.05 g
C)6.74 g
D)10.1 g
E)20.2 g

Question 31

The number of grams in 7.00 moles of N₂ is ________.

A)7 × (6.02 × 10²³)
B)14.0
C)28.0
D)98.0
E)196

Question 32

In the reaction shown,what is the mole ratio that would be used to determine the number of moles of oxygen needed to react with 3.2 moles of C₄H₁₀?
2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O

A)

B)

C)

D)

E)

Question 33

How many moles of CO₂ are produced when 2.5 moles of O₂ react according to the following equation?
C₃H₅ + 5 O₂ → 3 CO₂ + 4 H₂O

A)1.5
B)3
C)5
D)6
E)18

Question 34

How many moles of NaHCO₃ are present in a 2.00 g sample?

A)2.38 × 10^-2 mol
B)1.27 × 10^-2 mol
C)2.00 mol
D)85.0 mol
E)168 mol

Question 35

A student weighed 0.550 g of lithium chloride,LiCl,to use in a reaction.How many moles is this?

A)77.08
B)42.39
C)23.31
D)5.11
E)0.0130

Question 36

The following equation represents the formation of nitrogen dioxide,a major component of smog,
2 NO + O₂ → 2 NO₂
If 0.68 mole of NO is reacted with 0.79 mole of O₂ to produce NO₂,the limiting reactant is ________.

A)both NO and O₂
B)NO
C)O₂
D)NO₂

Question 37

In the reaction 2 C + O₂ → 2 CO,how many moles of carbon are needed to produce 66.0 g of carbon monoxide?

A)0.424
B)1.18
C)2.36
D)4.71
E)28.3

Question 38

How much Ca(NO₃)₂ should be weighed out to have 0.650 mol?

A)66.4 g
B)97.6 g
C)107 g
D)133 g
E)165 g

Question 39

Given the following balanced equation,answer the following:
C₂H₅OH + 3 O₂ → 2 CO₂ + 3 H₂O
a)What is the theoretical yield of carbon dioxide in this reaction if 39.6 g of ethanol is burned in the presence of 54.8 g of oxygen?
b)What is the percent yield for this reaction if the actual amount of carbon dioxide formed is 45.5 grams?

Question 40

The balanced equation given below means:
CH₄ + 2 O₂ → CO₂ + 2H₂O

A)One mole of methane reacts with two moles of oxygen to produce one mole of carbon dioxide and 2 moles of water.
B)One gram of methane reacts with two grams of oxygen to produce one gram of carbon dioxide and two grams of water.
C)One molecule of methane reacts with two molecules of oxygen to produce one molecule of carbon dioxide and two molecules of water.
D)A,B and C are correct.
E)A and C are correct.

Question 41

Match the following.
The mass of 1.22 moles of iron(II)nitrate

A)208.2 g
B)212.4 g
C)219 g
D)225 g

Question 42

A solution containing 145.0 g AgNO₃ is mixed with a CaCl₂ solution and 98.4 of AgCl is recovered.Calculate the % yield of the reaction.

A)40.16%
B)61.11%
C)61.99%
D)80.44%
E)161.3%

Question 43

Match the following.
The molar mass of BaCI₂

A)208.2 g
B)212.4 g
C)219 g
D)225 g

Question 44

Match the following.
The mass of 2.25 moles of CaCO₃

A)208.2 g
B)212.4 g
C)219 g
D)225 g

Question 45

The reaction N₂ + 3 H₂ → 2 NH₃ is used to produce ammonia.When 450.g of hydrogen was reacted with nitrogen,1575 g of ammonia were produced.What is the percent yield of this reaction?

A)62.1%
B)41.5%
C)30.8%
D)20.7%
E)More information is needed to solve this problem.

Question 46

Match the following.
The molar mass of C₁₅H₃₂

A)208.2 g
B)212.4 g
C)219 g
D)225 g