Deck 4: Chemical Reactions

Question 1

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

Answer 1

C

Question 2

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 that weighs exactly 12 atomic mass units
B) a sample that contains 6.02 × 10²³ atoms of ¹²C
C) a sample that weighs exactly 12 atomic mass units and a sample that contains 6.02 x 10²³ atoms of ¹²C
D) neither a sample that weighs exactly 12 atomic mass units or a sample that contains 6.02 x 10²³ atoms of ¹²C

Answer 2

B

Question 3

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

Answer 3

C

Question 4

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 5

How many joules make a kilocalorie?

A) 2,184 joules
B) 3,184 joules
C) 4,184 joules
D) 5,184 joules

Question 6

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

Question 7

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

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

Question 8

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 9

To which of the following is the term molecular weight applicable?

A) ionic compounds
B) covalent compounds
C) both ionic and covalent compounds
D) neither ionic or covalent compounds

Question 10

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 11

Which of the following is analogous to the reactants in a chemical reaction?

A) a baked cake
B) the flour, eggs, and chocolate used to bake a cake
C) a baked cake and the flour, eggs, and chocolate used to bake a cake
D) neither a baked cake or the flour, eggs, and chocolate used to bake a cake

Question 12

To which of the following is the term formula weight applicable?

A) ionic compounds
B) covalent compounds
C) both ionic and covalent compounds
D) neither ionic or covalent compounds

Question 13

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

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

Question 14

What is the molecular weight of sucrose, C₁₂H₂₂O₁₁?

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

Question 15

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

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

Question 16

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 17

Which of the following compounds has the largest formula weight?

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

Question 18

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 19

Which of the following compounds has the largest formula weight?

A) KCl
B) NaCl
C) MgF₂
D) BF₃

Question 20

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

Question 21

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 22

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 23

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 24

0.789 mol of a particular substance weighs 142 g. What is the molar mass of this substance?

A) 0.00556 g
B) 0.00556 amu
C) 180 g
D) 180 amu

Question 25

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 26

A certain protein has a molar mass of 2.38 × 10⁵ g. What is the mass of one molecule of this protein?

A) 3.95 × 10^-19 g
B) 4.20 × 10^-6 g
C) 2.38 × 10⁵ g
D) 2.53 × 10¹⁸ g

Question 27

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 28

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) In a chemical reaction, the number of moles of product always equals the number of moles of reactants, and the mass of products always equals the mass of the starting materials that have reacted.
D) In a chemical reaction, the number of moles of product does not always equal the number of moles of reactants, and the mass of products does not always equal the mass of the starting materials that have reacted.

Question 29

0.117 mol of a particular substance weighs 21.9 g. What is the molar mass of this substance?

A) 187 g
B) 187 amu
C) 0.00534 g
D) 0.00534 amu

Question 30

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 31

A 900-g iron block is initially at 5°C. Heat of 5,000 cal is added to it. What is the final temperature of the iron block? The specific heat of iron is 0.11 cal/g·°C.

A) 45.5°C
B) 50.5°C
C) 55.5°C
D) 60.5°C

Question 32

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 33

The atomic weight of platinum is less than that of gold. Which of the following statements is true provided you have a 10-g sample of each of these metals?

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

Question 34

The temperature of an unknown substance weighing 500 grams rises by 30°C when 2,000 cal of heat is added to it. What is the specific heat of this substance?

A) 0.033 cal/g·°C
B) 0.133 cal/g·°C
C) 0.233 cal/g·°C
D) 0.433 cal/g·°C

Question 35

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 36

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 37

The molecular weight of cholesterol is 710 amu. What is the mass of one molecule of cholesterol?

A) 1.18 × 10^-21 g
B) 0.00141 g
C) 710 g
D) 8.48 × 10²⁰ g

Question 38

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 39

The atomic weight of copper is greater than that of chromium. Which of the following statements is true provided you have a 10-g sample of each of these metals?

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

Question 40

The atomic weight of copper is less than that of silver. Which of the following statements is true provided you have a 10-g sample of each of these metals?

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

Question 41

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

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

Question 42

Ethanol is produced industrially by the acid-catalyzed reaction of ethylene with water. The balanced equation for this reaction is as follows: 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 43

Which of the following is the SI unit for heat?

A) calorie
B) kilocalorie
C) joule
D) watt

Question 44

Which of the following is the correct set of integer coefficients for the balanced equation? ___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 45

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

Question 46

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

Question 47

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) To determine mass relationships in a chemical reaction, you first need to know the balanced chemical equation for the reaction, and to convert from grams to moles and vice versa, you need to use Avogadro's number as a conversion factor.
D) None of these are true.

Question 48

In the industrial synthesis of acetic acid, methanol is made to react with carbon monoxide. The balanced equation for this reaction is as follows: CH₃OH(g) + CO(g) → CH₃COOH(l)
If methanol 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 49

In the industrial synthesis of acetic acid, methanol is made to react with carbon monoxide. The balanced equation for this reaction is as follows: 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 50

Which of the following statements is true of the balanced equation 3H₂(g) + N₂(g) → 2NH₃(g)?

A) Three grams of hydrogen react with one gram of nitrogen to form two grams of ammonia.
B) Three moles of hydrogen react with one mole of nitrogen to form two moles of ammonia.
C) Three moles of hydrogen react with one gram of nitrogen to form two grams of ammonia, and three moles of hydrogen react with one mole of nitrogen to form two moles of ammonia.
D) None of these are true.

Question 51

Ethanol is produced industrially by the acid-catalyzed reaction of ethylene with water. The balanced equation for this reaction is as follows: 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 52

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

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) the number of molecules of NH₃ obtained if 4.2 mol of N₂ react completely to form NH_3, and the number of moles of NH₃ obtained if 4.2 mol of N₂ react completely to form NH_3.
D) None of these are true.

Question 53

Sodium sulfite, Na₂SO₃(aq), is added to wine as an antioxidant as it reacts with the oxygen in 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) + 2O(g) → Na₂SO₄(aq)
C) 2Na₂SO₃(aq) + O₂(g) → 2Na₂SO₄(aq)
D) Na₂SO₃(aq) + O₂(g) → Na₂SO₄(aq)

Question 54

Which of the following is the correct set of integer coefficients for the balanced equation? ___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 55

Which of the following is the correct set of integer coefficients for the balanced equation? ___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 56

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

Question 57

Which of the following is true of specific heat?

A) Specific heat is a chemical property.
B) All substances have the same specific heat.
C) Specific heat is the amount of heat needed to change the state of 1 g of a substance from solid to liquid.
D) Specific heat is the amount of heat needed to raise the temperature of 1 g of a substance by 1°C.

Question 58

Which of the following is the correct set of integer coefficients for the balanced equation? ___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 59

Which of the following statements is true of the balanced equation N₂(g) + 2O₂(g) → 2NO₂(g)?

A) One mole of nitrogen reacts with two moles of oxygen to form two moles of nitrogen dioxide.
B) One gram of nitrogen reacts with two grams of oxygen to form two grams of nitrogen dioxide.
C) One mole of nitrogen reacts with two moles of oxygen to form two moles of nitrogen dioxide, and one gram of nitrogen reacts with two grams of oxygen to form two grams of nitrogen dioxide.
D) None of these are true.

Question 60

Which of the following is a form of energy?

A) heat
B) temperature
C) volume
D) mass

Question 61

When solutions of AgNO₃ and NaOH react, the balanced molecular equation is as follows: 2AgNO₃(aq) + 2NaOH(aq) → Ag₂O(s) + 2NaNO₃(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 62

In an experiment, ammonia is produced by mixing 3 moles of nitrogen gas with 6 moles of hydrogen gas. The balanced equation for this reaction is as follows: N₂(g) + 3H₂(g) → 2NH₃(g)
What is the number of moles of ammonia produced?

A) 2
B) 3
C) 4
D) 6

Question 63

Given the reaction 2HgO(s) → 2Hg(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 64

O₂ can be produced by the reaction 2KClO₃(s) → 2KCl(s) + 3O₂(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 65

Diethyl ether can be made from ethanol. The reaction is as follows: 2C₂H₅OH(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%

Question 66

When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is as follows: H₂SO₄(aq) + 2NaOH(aq) → Na₂SO₄(aq) + 2H₂O(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 67

O₂ can be produced by the reaction 2KClO₃(s) → KCl(s) + 3O₂(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 68

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is as follows: 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 g
C) 4.17 g
D) 6.20 g

Question 69

Ethanol is produced industrially by the acid-catalyzed reaction of ethylene with water. The balanced equation for this reaction is as follows: 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 70

In an experiment to prepare aspirin, the percent yield was 94.3%. If the actual yield was 124.3 g, what was the theoretical yield for this experiment?

A) 94.3 g
B) 117 g
C) 132 g
D) 234 g

Question 71

When solutions of AgNO₃ and NaCl react, the balanced molecular equation is as follows: 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 72

When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is as follows: H₂SO₄(aq) + 2NaOH(aq) → Na₂SO₄(aq) + 2H₂O(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

In the industrial synthesis of acetic acid, methanol is made to react with carbon monoxide. The balanced equation for this reaction is as follows: 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 74

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 75

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 76

When solutions of AgNO₃ and NaOH react, the balanced molecular equation is as follows: 2AgNO₃(aq) + 2NaOH(aq) → Ag₂O(s) + 2NaNO₃(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 77

Given the reaction 2HgO(s) → 2Hg(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 78

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

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

Question 79

In an experiment, acetic acid is produced by mixing 5 moles of methanol with 2 moles of carbon monoxide. The balanced equation for this reaction is as follows: CH₃OH(l) + CO(g) → CH₃COOH(l)
What is the number of moles of acetic acid produced?

A) 2
B) 3
C) 5
D) 10

Question 80

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

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