Deck 4: Chemical Reactions

Question 1

How many molecules are present in one mole of glucose, C₆H₁₂O₆?

A) 6.92 ×10^-26
B) 3.34 × 10²¹
C) 6.02 × 10²³
D) 1.44 × 10²⁵

Answer 1

C

Question 2

What is the molecular weight of sucrose, C₁₂H₂₂O₁₁?

A) 180.2 amu
B) 319.6 amu
C) 342.3 amu
D) 360.4 amu

Answer 2

C

Question 3

What is the formula weight of barium phosphate, Ba₃(PO₄) ₂?

A) 232.3 amu
B) 537.9 amu
C) 559.6 amu
D) 601.9 amu

Answer 3

D

Question 4

Which of the following compounds has the largest formula weight?

A) KCl
B) NaCl
C) MgF₂
D) BF₃

Question 5

What is the molar mass of water, H₂O?

A) 17.01 g
B) 18.02 g
C) 17.01 amu
D) 18.02 amu

Question 6

The term molecular weight is strictly correct for which of the following?

A) ionic compounds
B) covalent compounds
C) both a and b
D) neither a nor b

Question 7

How many molecules are present in one mole of water, H₂O?

A) 1.66 × 10^-24
B) 3.00 × 10^-23
C) 3.24 × 10²³
D) 6.02 × 10²³

Question 8

The mass of an atom of ¹²C is exactly 12 atomic mass units. Which of the following describes a mole of ¹²C atoms?

A) a sample which contains 6.02 × 10²³ atoms of ¹²C
B) a sample which weighs exactly 12.011 grams
C) both a and b
D) neither a nor b

Question 9

What is the formula weight ammonium carbonate, (NH₄)₂CO₃?

A) 78.1 amu
B) 96.1 amu
C) 108.4 amu
D) 138.2 amu

Question 10

What is the formula weight of aluminum sulfate, Al₂(SO₄) ₃?

A) 75.1 amu
B) 150.2 amu
C) 342.2 amu
D) 369.7 amu

Question 11

Which of the following is the correct unit for formula weight?

A) atomic mass units
B) grams
C) ounces
D) pounds

Question 12

The reactants in a chemical reaction are analogous to which of the following?

A) a baked cake
B) the flour, eggs, chocolate used to bake a cake
C) both a and b
D) neither a nor b

Question 13

The mass of an atom of ¹²C is exactly 12 atomic mass units. Which of the following describes a mole of ¹²C atoms?

A) a sample which weighs exactly 12 atomic mass units
B) a sample which contains 6.02 × 10²³ atoms of ¹²C
C) both a and b
D) neither a nor b

Question 14

If you need a sample of 2.84 mol of Na₂S, how many grams do you need?

A) 0.00451 g
B) 2.84 g
C) 78.1 g
D) 222 g

Question 15

Which of the following compounds has the largest formula weight?

A) aluminum acetate
B) calcium acetate
C) potassium acetate
D) sodium acetate

Question 16

What is the molar mass of glucose, C₆H₁₂O₆?

A) 60.05 amu
B) 180.2 amu
C) 60.05 g
D) 180.2 g

Question 17

What is the molecular weight of ibuprofen, C₁₃H₁₈O₂?

A) 29.0 amu
B) 206.3 amu
C) 289.4 amu
D) 377.7 amu

Question 18

A person drinks 1.50 × 10³ g of water, H₂O, per day. How many moles is this?

A) 0.0120
B) 8.33
C) 83.3
D) 1.20 × 10²

Question 19

How many moles of marble, CaCO₃, are there in a 275 g piece of marble?

A) 4.57 × 10^-22
B) 0.364
C) 2.75
D) 275

Question 20

The term formula weight can be used with respect to which of the following?

A) ionic compounds
B)
B) covalent compounds
C) both a and b
D) neither a nor

Question 21

How many moles of oxygen atoms are present in 5.20 mol of Al₂(SO₄)₃?

A) 15.6
B) 20.8
C) 62.4
D) 3.76 × 10²⁵

Question 22

The atomic weight of platinum is less than that of gold. If you have a 10 g sample of each of these metals, which of the following is true?

A) You have fewer of atoms of platinum than of gold.
B) You have equal numbers of atoms of platinum and gold.
C) You have more atoms of platinum than of gold.
D) There is insufficient information to determine which of the above is true.

Question 23

A serving of a particular fruit dessert contains 20.0 g of sugar. If all the sugar is sucrose, C₁₂H₂₂O₁₁, how many molecules of sugar are present in this serving?

A) 0.0584
B) 17.1
C) 3.52 × 10²²
D) 1.03 × 10²⁵

Question 24

How many oxygen atoms are present in 5.20 mol of Al₂(SO₄)₃?

A) 62.4
B) 3.76 × 10²⁵
C) 9.39 × 10²⁴
D) 3.13 × 10²⁴

Question 25

0.117 mol of a particular substance weighs 21.9

A) 187 g
B) 187 amu
C) 0.00534 g
D) 0.00534 amu
G) What is the molar mass of this substance?

Question 26

How much does a sample of 5.75 mol diethyl ether, C₄H₁₀O, weigh?

A) 5.75 g
B) 12.9 g
C) 74.1
D) 426

Question 27

Which of the following is true of a chemical reaction?

A) In a chemical reaction, the number of moles of product always equals the number of moles of reactants.
B) In a chemical reaction, the mass of the products always equals the mass of the starting materials that have reacted.
C) Both a and b are true.
D) Both a and b are false.

Question 28

Which of the following is true of a balanced chemical reaction?

A) In a balanced chemical equation, number of molecules on the reactant side equals the number molecules on the product side.
B) In a balanced chemical equation, the number of atoms on the reactant side equals the number of atoms on the product side.
C) Both a and b are true.
D) Both a and b are false.

Question 29

A certain protein has a molar mass of 2.38 × 10⁵

A) 3.95 × 10^-19 g
B) 4.20 × 10^-6 g
C) 2.38 × 10⁵ g
D) 2.53 × 10¹⁸ g
G) What is the mass of one molecule of this protein?

Question 30

A typical deposit of cholesterol, C₂₇H₄₆O, in an artery has a mass of 3.90 mg. How many molecules of cholesterol are present in this deposit?

A) 6.07 × 10²¹
B) 6.07 × 10¹⁸
C) 0.00390
D) 1.65 × 10^-22

Question 31

g
D) 8.48 × 10²⁰ g

Question 32

The molecular weight of ethylene glycol is 62.0 amu. What is the mass of one molecule of ethylene glycol?

A) 9.70 × 10²¹ g
B) 62.0 g
C) 0.0161 g
D) 1.03 × 10^-22 g

Question 33

0.789 mol of a particular substance weighs 142

A) 0.00556 g
B) 0.00556 amu
C) 180 g
D) 180 amu
G) What is the molar mass of this substance?

Question 34

The atomic weight of copper is greater than that of chromium. If you have a 10 g sample of each of these metals, which of the following is true?

A) You have fewer of atoms of copper than of chromium.
B) You have equal numbers of atoms of copper and chromium.
C) You have more atoms of copper than of chromium.
D) There is insufficient information to determine which of the above is true.

Question 35

How many moles of hydrogen atoms are there in 2.50 mol of C₆H₁₂O₆?

A) 2.50
B) 30.0
C) 1.51 × 10²⁴
D) 1.81 × 10²⁵

Question 36

The atomic weight of copper is less than that of silver. If you have a 10 g sample of each of these metals, which of the following is true?

A) You have fewer of atoms of copper than of silver.
B) You have equal numbers of atoms of copper and silver.
C) You have more atoms of copper than of silver.
D) There is insufficient information to determine which of the above is true.

Question 37

The molar mass of gold is approximately 197

A) 3.06 × 10²¹ g
B) 197 g
C) 5.08 × 10^-3 g
D) 3.27 × 10^-22 g
G) What is the approximate mass of one atom of gold?

Question 38

How many hydrogen atoms are there in 2.50 mol of C₆H₁₂O₆?

A) 2.50
B) 12.0
C) 1.51 × 10²⁴
D) 1.81 × 10²⁵

Question 39

You have a sample of 1.204 × 10²⁴ atoms of gold. How much does this sample weigh?

A) 2.000 g
B) 98.5 g
C) 197.0 g
D) 394.0 g

Question 40

You have a sample of 3.01 × 10²³ atoms of silver. How much does this sample weigh?

A) 0.0500 g
B) 2.00 g
C) 53.9 g
D) 107.9 g

Question 41

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C₂H₄(g) + H₂O(g) → C₂H₅OH(l)
If water is present in excess, how many grams of ethanol can be produced from 7.24 mol of ethylene?

A) 7.24 g
B) 14.5 g
C) 203 g
D) 334 g

Question 42

Which of the following is true regarding mass relationships in a chemical reaction?

A) To determine mass relationships in a chemical reaction, you first need to know the balanced chemical equation for the reaction.
B) To convert from grams to moles and vice versa, you need to use molar mass as a conversion factor.
C) Both a and b are true.
D) Both a and b are false.

Question 43

For the reaction N₂(g) + 3 H₂(g) → 2 NH₃(g) which of the following can be determined using only the coefficients of the balanced chemical equation?

A) the number of molecules of NH₃ obtained if 4.2 mol of N₂ react completely to form NH₃
B) the number of moles of NH₃ obtained if 4.2 mol of N₂ react completely to form NH₃
C) both a and b
D) neither a nor b

Question 44

For the reaction N₂(g) + 3 H₂(g) → 2 NH₃(g) which of the following can be determined using only the coefficients of the balanced chemical equation?

A) the number of moles of NH₃ obtained if 4.2 mol of N₂ react completely to form NH₃
B) the weight of NH₃ obtained if 4.2 mol of N₂ react completely to form NH₃
C) both a and b
D) neither a nor b

Question 45

The reaction of nitric acid, HNO₃(aq), with calcium carbonate, CaCO₃(s) produces calcium nitrate, carbon dioxide, and water. Which of the following is the correct balanced equation for this reaction?

A) HNO₃(aq) + CaCO₃(s) → CaNO₃(aq) + CO₂(g) + H₂O(l)
B) 2 HNO₃(aq) + CaCO₃(s) → CaNO₃(aq) + CO₂(g) + H₂O(l)
C) HNO₃(aq) + CaCO₃(s) → Ca(NO₃)₂(aq) + CO₂(g) + H₂O(l)
D) 2 HNO₃(aq) + CaCO₃(s) → Ca(NO₃)₂(aq) + CO₂(g) + H₂O(l)

Question 46

When phosphoric acid, H₃PO₄(aq), reacts with solid magnesium hydroxide, Mg(OH)₂(s), the products are aqueous magnesium phosphate and water. Which of the following is the balanced equation for this reaction?

A) H₃PO₄(aq) + Mg(OH)₂(s) → MgPO₄(aq) + H₂O(l)
B) 2 H₃PO₄(aq) + Mg(OH)₂(s) → Mg(PO₄)₂(aq) + 2 H₂O(l)
C) 3 H₃PO₄(aq) + 2 Mg(OH)₂(s) → Mg₂(PO₄)₃(aq) + 2 H₂O(l)
D) 2 H₃PO₄(aq) + 3 Mg(OH)₂(s) → Mg₃(PO₄)₂(aq) + 6 H₂O(l)

Question 47

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C₂H₄(g) + H₂O(g) → C₂H₅OH(l)
If water is present in excess, how many moles of ethanol can be produced from 7.24 mol of ethylene?

A) 7.24
B) 14.5
C) 28.0
D) 46.0

Question 48

Which of the following is true of a conventionally balanced chemical equation?

A) The number of molecules on the left equal the number of molecules on the right.
B) The coefficients are all integers.
C) Both a and b are true.
D) Both a and b are false.

Question 49

In the industrial synthesis of acetic acid, methanol is reacted with carbon monoxide. The balanced equation for this reaction is: CH₃OH(g) + CO(g) → CH₃COOH(l)
How many grams of CO(g) are required to produce 49.4 g of acetic acid?

A) 23.0 g
B) 28.0 g
C) 60.1 g
D) 88.1 g

Question 50

In the industrial synthesis of acetic acid, methanol is reacted with carbon monoxide. The balanced equation for this reaction is: CH₃OH(g) + CO(g) → CH₃COOH(l)
How many grams of CO(g) are required to produce 16.6 mol of acetic acid?

A) 16.6 g
B) 33.2 g
C) 465 g
D) 996 g

Question 51

Which of the following is the correct set of integer coefficients for the balanced equation, respectively: ___ C₃H₈(g) + ___O₂(g) → ___CO₂(g) + ___H₂O(g)

A) 3, 8, 1, 2
B) 1, 5, 3, 4
C) 1, 5, 4, 3
D) 4, 3, 2, 1

Question 52

Sodium sulfite, Na₂SO₃(aq), is added to wine as an antioxidant since it reacts with the oxygen of the air to form sodium sulfate, Na₂SO₄(aq). Which of the following is the balanced equation for this reaction?

A) Na₂SO₃(aq) + O(g) → Na₂SO₄(aq)
B) Na₂SO₃(aq) + 2 O(g) → Na₂SO₄(aq)
C) 2 Na₂SO₃(aq) + O₂(g) → 2 Na₂SO₄(aq)
D) Na₂SO₃(aq) + O₂(g) → Na₂SO₄(aq)

Question 53

In a blast furnace, coke, which is solid carbon, reacts with O₂(g) to form carbon monoxide. The carbon monoxide then reacts with Fe₂O₃(s) to produce solid iron and carbon dioxide. Which of the following is the balanced equation for this combined process?

A) 2 Fe₂O₃(s) + 3 C(s) + 3 O₂(g) → 2 Fe(s) + 3 CO₂(g)
B) 2 Fe₂O₃(s) + 2 C(s) + 3 O₂(g) → 4 Fe(s) + 2 CO₂(g)
C) 2 Fe₂O₃(s) + 6 C(s) + 3 O₂(g) → 4 Fe(s) + 6 CO₂(g)
D) 2 Fe₂O₃(s) + C(s) + 3 O₂(g) → Fe(s) + CO₂(g)

Question 54

In a blast furnace, coke, which is solid carbon, reacts with O₂(g) to form carbon monoxide. The carbon monoxide then reacts with Fe₂O₃(s) to produce solid iron and carbon dioxide. Which of the following is the balanced equation for the reaction of carbon monoxide with Fe₂O₃(s)?

A) 2 Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g)
B) 2 Fe₂O₃(s) + 2 CO(g) → 4 Fe(s) + 2 CO₂(g)
C) 2 Fe₂O₃(s) + 3 CO(g) → 4 Fe(s) + 3 CO₂(g)
D) Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g)

Question 55

In the industrial synthesis of acetic acid, methanol is reacted with carbon monoxide. The balanced equation for this reaction is: CH₃OH(g) + CO(g) → CH₃COOH(l)
If ethanol is present in excess, how many moles of CO(g) are required to produce 16.6 moles of acetic acid?

A) 8.30
B) 16.6
C) 28.0
D) 33.2

Question 56

Which of the following is the correct set of integer coefficients for the balanced equation respectively: ___ C₅H₁₂(g) + ___O₂(g) → ___CO₂(g) + ___H₂O(g)

A) 1, 5, 5, 6
B) 1, 8, 5, 6
C) 5, 1, 8, 6
D) 5, 12, 2, 4

Question 57

For the reaction N₂(g) + 3 H₂(g) → 2 NH₃(g) which of the following can be determined using only the coefficients of the balanced chemical equation?

A) the number of molecules of NH₃ obtained if 4.2 mol of N₂ react completely to form NH₃
B) the weight of NH₃ obtained if 4.2 mol of N₂ react completely to form NH₃
C) both a and b
D) neither a nor b

Question 58

Which of the following is the correct set of integer coefficients for the balanced equation, respectively: ___ C₆H₁₄(g) + ___O₂(g) → ___CO₂(g) + ___H₂O(g)

A) 1, 1, 1, 1
B) 1, 3, 6, 7
C) 1, 9.5, 6, 7
D) 2, 19, 12, 14

Question 59

Which of the following is the correct set of integer coefficients for the balanced equation, respectively: ___ CO₂(g) + ___H₂O(l) → ___C₆H₁₂O₆(aq) + ___O₂(g)

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

Question 60

Which of the following is true regarding mass relationships in a chemical reaction?

A) To determine mass relationships in a chemical reaction, you first need to know the balanced chemical equation for the reaction.
B) To convert from grams to moles and vice versa, you need to use Avogadro's number as a conversion factor.
C) Both a and b are true.
D) Both a and b are false.

Question 61

Lime, CaO, is produced by the reaction CaCO₃(s) → CaO(s) + CO₂(g). What weight of CO₂ is obtained by the decomposition of 38.7 g of CaCO₃?

A) 15.5 g
B) 17.0 g
C) 21.7 g
D) 23.2 g

Question 62

When solutions of AgNO₃ and NaOH react, the balanced molecular equation is: 2 AgNO₃(aq) + 2 NaOH(aq) → Ag₂O(s) + 2 NaNO₃(aq) + H₂O(l)
How much Ag₂O is produced when 0.200 g of AgNO₃ and 0.200 g of NaOH react?

A) 0.127 g
B) 0.136 g
C) 0.273 g
D) 0.400 g

Question 63

Given the reaction 2 HgO(s) → 2 Hg(l) + O₂(g). What weight of elemental mercury will be obtained by the decomposition of 0.125 mol of HgO?

A) 13.5 g
B) 25.0 g
C) 27.0 g
D) 50.0 g

Question 64

The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g). What weight of oxygen is required to completely burn 19.8 g of octane?

A) 28.1 g
B) 34.7
C) 69.5
D) 139 g

Question 65

When solutions of AgNO₃ and NaOH react, the balanced molecular equation is: 2 AgNO₃(aq) + 2 NaOH(aq) → Ag₂O(s) + 2 NaNO₃(aq) + H₂O(l)
How much Ag₂O is produced when 2.00 g of AgNO₃ and 0.300 g of NaOH react?

A) 0.869 g
B) 1.43 g
C) 1.74 g
D) 2.30 g

Question 66

A bicycle manufacturer has a stock of 50 frames 70 wheels, and 160 reflectors. If each bicycle manufactured requires 4 reflectors, how many bicycles can the manufacturer make?

A) 25
B) 35
C) 40
D) 50

Question 67

In a particular experiment to prepare a compound, the theoretical yield is 34.7

A) 0.899%
B) 11.1%
C) 89.9%
D) 93.0%
G) If the actual yield is 31.2 g, what is the percent yield?

Question 68

A bicycle manufacturer has a stock of 50 frames 70 wheels, and 120 reflectors. If each bicycle manufactured requires 4 reflectors, how many bicycles can the manufacturer make?

A) 25
B) 30
C) 35
D) 50

Question 69

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq)
How much AgCl is produced when 3.10 g of AgNO₃ and 0.600 g of NaCl react?

A) 1.47 g
B) 2.23 g
C) 2.62 g
D) 3.70 g

Question 70

In an experiment to prepare aspirin, the percent yield was 94.3%

A) 94.3 g
B) 117 g
C) 132 g
D) 234 g
G) If the actual yield was 124.3 g, what was the theoretical yield for this experiment?

Question 71

The balanced equation for burning octane is: 2 C₈H₁₈(g) + 25 O₂(g) → 18 H₂O(g) + 16 CO₂(g) What weight of H₂O is produced by completely burning 19.8 g of octane?

A) 28.1 g
B) 34.7
C) 69.5
D) 139 g

Question 72

When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is: H₂SO₄(aq) + 2 NaOH(aq) → Na₂SO₄(aq) + 2 H₂O(l)
How much Na₂SO₄ is obtained when 4.00 g of H₂SO₄ reacts with 2.00 g of NaOH?

A) 0.650 g
B) 2.98 g
C) 3.55 g
D) 4.20 g

Question 73

Lime, CaO, is produced by the reaction CaCO₃(s) → CaO(s) + CO₂(g). What weight of CaO is obtained by the decomposition of 38.7 g of CaCO₃?

A) 15.5 g
B) 17.0 g
C) 21.7 g
D) 23.2 g

Question 74

O₂ can be produced by the reaction 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g). In one experiment 0.312 g of O₂ was formed. How much KClO₃ was decomposed?

A) 0.484 g
B) 0.797 g
C) 1.19 g
D) 1.79 g

Question 75

O₂ can be produced by the reaction 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g). In one experiment 0.312 g of O₂ was formed. How much KCl was produced?

A) 0.484 g
B) 0.797 g
C) 1.19 g
D) 1.79 g

Question 76

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq)
How much AgCl is produced when 3.10 g of AgNO₃ and 3.10 g of NaCl react?

A) 1.55 g
B) 2.62
C) 4.17 g
D) 6.20 g

Question 77

When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is: H₂SO₄(aq) + 2 NaOH(aq) → Na₂SO₄(aq) + 2 H₂O(l)
How much Na₂SO₄ is obtained when 4.00 g of H₂SO₄ reacts with 4.00 g of NaOH?

A) 2.98 g
B) 5.80 g
C) 7.10 g
D) 8.00 g

Question 78

Given the reaction 2 HgO(s) → 2 Hg(l) + O₂(g). What weight of elemental mercury will be obtained by the decomposition of 94.5 g of HgO?

A) 43.8 g
B) 78.5 g
C) 87.5 g
D) 175 g

Question 79

Ethanol is produced industrially by the acid catalyzed reaction of ethylene with water. The balanced equation for this reaction is: C₂H₄(g) + H₂O(g) → C₂H₅OH(l)
If water is present in excess, how many grams of ethanol can be produced from 42.7 g of ethylene?

A) 42.7 g
B) 46.1 g
C) 70.1 g
D) 92.2 g

Question 80

Diethyl ether can be made from ethanol. The reaction is: 2 C₂H₅OH(l) → (C₂H₅)₂O(l) + H₂O(l)
In one experiment 46.0 g of ethanol yielded 34.7 g of diethyl ether. What was the percent yield in this experiment?

A) 62.1%
B) 80.4%
C) 93.8%
D) 97.0%