Deck 4: Chemical Quantities and Chemical Reactions

Question 1

What is a biochemical pathway?

A) the path that nutrients take through the body when they are metabolized
B) the complex blood transport system
C) a chemical reaction in the body that releases energy
D) a chemical reaction that releases carbon dioxide
E) a particular sequence of chemical reactions in the body

Answer 1

a particular sequence of chemical reactions in the body

Question 2

Which statement best describes why we use moles when measuring quantities of atoms and molecules?

A) Moles are used because they are units of mass.
B) Moles are used because one mole is the same numerical value as the atomic mass of an element.
C) Moles are used because atoms and molecules are too small to measure singly.
D) Moles are used because chemists like moles.
E) Moles are not involved in measuring quantities of atoms and molecules.

Answer 2

Moles are used because atoms and molecules are too small to measure singly.

Question 3

A molecule of oxygen, O₂, has a molar mass of 32.00 g/mole. What is the mass of 4.52 *10²³ O₂ molecules?

A) 24 grams
B) 4.52 *10²³ amu
C) 4.52 * 10²³ grams
D) 0.75 grams
E) 0.23 grams

Answer 3

24 grams

Question 4

What is the mass of one mole of the hydroxide ion (^-OH)?

A) 8 g
B) 15 g
C) 17 g
D) 7 g
E) 5 g

Question 5

How many carbon atoms are in 1 mole of carbon?

A) 1
B) 12
C) 12.011
D) 6
E) 6.02 * 10²³

Question 6

How many grams of iron are in 1.28 moles of iron?

A) 0.0230 g
B) 20.3 g
C) 33.3 g
D) 43.6 g
E) 71.4 g

Question 7

Where in the body does ethanol metabolism occur?

A) the stomach
B) the liver
C) the kidneys
D) the small intestine
E) the mouth

Question 8

How many moles of carbon are in 27.1 g of carbon?

A) 2.26 moles
B) 325 moles
C) 0.443 moles
D) 4.52 moles
E) 163 moles

Question 9

Which of the following statements describes how molecular mass and molar mass differ?

A) Molecular mass is measured in amu, whereas molar mass is measured in grams/mole.
B) Molar mass is measured in amu, whereas molecular mass is measured in grams/mole.
C) A molar mass is the mass of one unit of an ionic lattice, whereas molecular mass is the mass of one molecule.
D) A molar mass is the mass of one molecule, whereas molecular mass is the mass of one unit of an ionic lattice.
E) There is no difference between these terms.

Question 10

Does one mole of the antibiotic penicillin G (C₁₆H₁₈N₂O₄S) weigh more or less than one mole of the antibiotic streptomycin (C₂₁H₃₉N₇O₁₂)?

A) Actually, they should weigh the same because a mole always has the same mass.
B) Actually, they should weigh the same because a mole always has the same number of particles in it.
C) Streptomycin should weigh more because its individual molecules are larger.
D) Penicillin should weigh more because its individual molecules are larger.
E) It is not possible to determine which one would weigh more because mole size varies.

Question 11

How many copper atoms are in 0.5 moles of copper?

A) 0.5
B) 14
C) 3
D) 6.02 * 10¹²
E) 3.01 * 10²³

Question 12

How many moles is 9.1*10²⁴ ions of Na⁺?

A) 5.5 *10⁴⁸ moles
B) 0.17 moles
C) 1 mole
D) 15 moles
E) 0.67 moles

Question 13

How many moles of the antibiotic tetracycline (C₂₂H₂₄N₂O₈) are in a 50-mg dose?

A) 8880 moles
B) 22.2 moles
C) 8.88 moles
D) 0.113 moles
E) 1.13 *10^-4 moles

Question 14

The ionic compound CaCO₃ has a formula mass of

A) 50 g/mole.
B) 50 amu.
C) 100 g/mole.
D) 100 amu.
E) 68.1 amu.

Question 15

An infant dose of acetaminophen (C₈H₉NO₂) is 0.080

A) 5.3 * 10^-4 molecules
B) 3.2 * 10²⁰ molecules
C) 7.2 * 10²³ molecules
D) 1.2 molecules
E) 2 * 10^-24 molecules

Question 16

Which of the following statements describes how formula mass and molecular mass differ?

A) A formula mass is measured in amu, whereas a molecular mass is measured in grams/mole.
B) A formula mass is measured in grams/mole, whereas a molecular mass is measured in amu.
C) A formula mass is the mass of one unit of an ionic lattice, whereas molecular mass is the mass of one molecule.
D) A formula mass is the mass of one molecule, whereas molecular mass is the mass of one unit of an ionic lattice.
E) There is no difference between these terms.

Question 17

Calculate the mass of one mole of dopamine, a neurotransmitter with the molecular formula C₈H₁₁NO₂.

A) 22.0 g
B) 43.0 g
C) 82.0 g
D) 153 g
E) 164 g

Question 18

Which of the following values is Avogadro's number?

A) 6
B) 6.02
C) 6.02 * 10²³
D) 6.02 * 10²⁶
E) 6.02 * 10¹²³

Question 19

Which of the following equations best describes how to calculate the molar mass of Mg(OH)₂?

A) 24.3 g/mole + 16.0 g/mole + 1.01 g/mole
B) 24.3 g/mole + 16.0 g/mole + (2 * 1.01 g/mole)
C) 24.3 g/mole + (2 *16.0 g/mole) + 1.01 g/mole
D) 24.3 g/mole + 2 * (16.0 g/mole + 1.01 g/mole)
E) 2 *(24.3 g/mole + 16.0 g/mole + 1.01 g/mole)

Question 20

Calculate the molecular mass of aspirin, C₉H₈O₄.

A) 29 g/mole
B) 126 g/mole
C) 180. g/mole
D) 126 amu
E) 180. amu

Question 21

Which of these figures illustrate chemical reactions?

A) I, II, and III are all chemical reactions.
B) Only I and II are chemical reactions.
C) Only I and III are chemical reactions.
D) Only II and III are chemical reactions.
E) None of these figures are chemical reactions.

Question 22

Below are several statements. Which of these statements apply to chemical reactions?

I. A chemical reaction always involves two reactants.
II. Physical changes are a type of chemical reaction.
III. Energy changes are involved in chemical reactions.
IV. Atoms are gained and lost during a chemical reaction.
V. Bonds are broken and new bonds formed during a chemical reaction.

A) All of these statements apply to chemical reactions.
B) Only I applies to chemical reactions.
C) I, II, and III all apply to chemical reactions.
D) IV and V both apply to chemical reactions.
E) III and V both apply to chemical reactions.

Question 23

If Jane Doe has a blood carbon dioxide concentration of 0.022 mol/L, how many carbon dioxide molecules are in each liter of her blood?

A) 3.7 *10^-26
B) 0.022
C) 1.32 *10²²
D) 6.02 * 10²³
E) 2.7 * 10²⁵

Question 24

Jane Doe has a cholesterol (C₂₇H₄₆O) count of 178 mg/dL. You would like to calculate the number of cholesterol molecules that Jane Doe has in each deciliter of blood. Which of the following calculations is used to solve this problem?

A)
B)
C)
D)
E)

Question 25

Jane Doe has her cholesterol measured and the resulting lab report gives a value of 0.548 *10^-3 mol/dL. You know that the normal range of cholesterol (C₂₇H₄₆O) is 0.100 - 0.240 g/dL. Is Jane Doe's cholesterol within the normal range?

A) No, it is above 0.240 g/dL.
B) No, it is below 0.100 g/dL.
C) Yes, it is between 0.100 g/dL and 0.240 g/dL.
D) Yes, it is above 0.240 g/dL.
E) Yes, it is below 0.100 g/dL.

Question 26

Which of the figures violates the conservation of mass?

A) All of these figures violate the conservation of mass.
B) Figure I violates the conservation of mass.
C) Figure II violates the conservation of mass.
D) Figure III violates the conservation of mass.
E) Figures II and III both violate the conservation of mass.

Question 27

Which of the following transformations is a chemical reaction?

A) water boiling
B) burning wood
C) condensation on the outside of a water glass
D) dry ice changing from a solid to a gas
E) All of the above

Question 28

A normal blood oxygen (O₂) level is 8.0 mmol/L. What is the normal mass of oxygen per liter of blood?

A) 2.50*10^-4 g
B) 0.256 g
C) 4.00 g
D) 256 g
E) 2.56 * 10⁵ g

Question 29

An important part of metabolism is the breakdown of proteins into smaller parts called amino acids. During the course of this reaction, some bonds are broken and others are formed. Select the choice that correctly lists the bonds that are broken and those that are formed.

A)a
B)b
C)c
D)d
E)e

Question 30

Which of the following must occur for there to be a chemical reaction?

A) Heat is released.
B) There is a change of state.
C) A gas is produced.
D) Bonds break and/or new ones are formed.
E) All of the above

Question 31

Which of the following transformations is illustrated in Figure II?

A) Figure II illustrates the breaking of hydrogen bonds.
B) Figure II illustrates the breaking of covalent bonds.
C) Figure II illustrates a chemical reaction.
D) Figure II illustrates a nuclear reaction.

Question 32

In which figure are new O-H bonds being formed?

A) Figure I
B) Figure II
C) Figure III
D) Figures I and II
E) Figures I and III

Question 33

If Jane Doe has a blood glucose (C₆H₁₂O₆) concentration of 0.102 g/dL, how many glucose molecules does she have in each deciliter of blood?

A) 3.41 * 10²⁶
B) 3.41 * 10²³
C) 3.41 *10²⁰
D) 6.41 * 10²²
E) 5.67 *10^-4

Question 34

Jane Doe has a cholesterol (C₂₇H₄₆O) count of 178 mg/dL. You would like to calculate the number of cholesterol molecules that Jane Doe has in each deciliter of blood. Which of the following unit conversions are required to calculate the number of cholesterol molecules per deciliter? I. 10 dL II. 1 mole III. 1 g____ IV. 6.02 * 10²³ molecules
1 L 387 g 1000 mg 1 mole

A) All of the conversions are needed.
B) I and IV
C) III and IV
D) I, II, and III
E) II, III, and IV

Question 35

Jane Doe has a cholesterol (C₂₇H₄₆O) count of 178 mg/dL. How many cholesterol molecules does Jane Doe have in each deciliter of blood?

A) 7.64 * 10^-22
B) 1.14 * 10^-22
C) 2.77 *10²⁰
D) 4.45 * 10²⁵
E) 2.77 * 10²⁶

Question 36

What are the products of the reaction illustrated in Figure I?

A) CH₄ and O₂
B) CO₂ and H₂O
C) CH₄ only
D) O₂ only
E) CO₂ only

Question 37

How is a nuclear reaction different from a chemical reaction?

A) They are identical.
B) Only in a chemical reaction can atoms change into different atoms.
C) Chemical reactions involve only the nucleus of the atom.
D) Only in a nuclear reaction can atoms change into different atoms.
E) Nuclear reactions release energy and chemical reactions absorb energy.

Question 38

A chemical reaction involves many changes, but not everything changes during a reaction. Which of the following is NOT a change that occurs during a chemical reaction?

A) Atoms change in number or identity.
B) Bonds break.
C) Heat is released and/or absorbed.
D) New bonds form.
E) New molecules are formed.

Question 39

Hydrogen fuel cells are a promising alternative to gasoline engines in part because they release water instead of carbon dioxide. In a hydrogen fuel cell, hydrogen gas (H₂) and oxygen gas (O₂) react to make water as shown below. Which of the following statements is a true statement about how this reaction occurs? 2 H₂(g) + O₂(g) → 2 H₂O(g)

A) Two molecules of H₂ and a molecule of O₂ must collide at one time.
B) A molecule of H₂ and a molecule of O₂ collide.
C) An O-H bond must break.
D) An H-H bond must form.
E) The reactants must undergo a change of state for this reaction to occur.

Question 40

Which of the following equations is used to convert 91.0 milligrams of urea (CH₄N₂O) to moles of urea?

A)

B)

C)

D)


E)

Question 41

Below are several chemical equations, each labeled with the names of parts of a chemical equation. Which has the parts labeled correctly.

A)a
B)b
C)c
D)d
E)e

Question 42

What does it mean for mass to be conserved?

A) Mass is neither created nor destroyed in the course of a chemical reaction.
B) Mass is a valuable resource and should not be wasted.
C) Molecules do not degrade under normal circumstances.
D) Atoms sometimes disappear over the course of a chemical reaction.
E) Atoms sometimes appear, disappear or are changed over the course of a chemical reaction.

Question 43

Coefficients are important components of chemical equations. What is the significance of coefficients in a chemical equation? I. Coefficients indicate the ratio of masses of molecules.
II) Coefficients indicate the ratio of numbers of atoms and molecules.
III) Coefficients indicate the ratio of numbers of moles of molecules and atoms.

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

Question 44

What is the meaning of the arrow in the following chemical equation?

A) Heat is released from the reaction.
B) A product is substituted for a reactant.
C) The reactants collide.
D) The reactants are transformed into the products.
E) Heat is applied to the reactants.

Question 45

Which of the following characteristics of a chemical reaction is never included in a chemical equation?

A) the quantity of reactants
B) the relative proportions of reactants and products
C) the amount of energy absorbed or released by the reaction
D) the identity of the products and reactants
E) the physical state of the reactants and products

Question 46

The following chemical equation, the decomposition of hydrogen peroxide to water, is not balanced. What must be done to the equation to make it balanced? 2 H₂O₂ (l) → 2 H₂O (l)

A) Change the coefficients from 2 to 1.
B) Add an atom of oxygen to the products.
C) Add a molecule of O₂ to the products.
D) Change the state of matter in the products.
E) Change the subscripts of H₂O to H₂O₂.

Question 47

The balanced equation for nitrogen fixing is given below. What do the numbers in front of the molecules (the coefficients) mean? N₂ + 3 H₂ → 2 NH₃

A) Three moles of H₂ react with one mole of N₂ to give two moles of NH₃.
B) Three grams of H₂ react with one gram of N₂ to give two grams of NH₃.
C) Three atoms of H react with one atom of N to give two molecules of NH₃.
D) Two grams of N react with six grams of H to give eight grams of NH₃.
E) All of the above

Question 48

What is the primary relationship between a chemical reaction and a chemical equation?

A) There is no relationship between a chemical reaction and a chemical equation.
B) A chemical equation is the written representation of a chemical reaction.
C) A chemical equation follows the law of conservation of mass but a chemical reaction does not.
D) A chemical equation shows the proportion of reactants and products but a chemical reaction does not necessarily reflect those proportions.
E) Chemical equations and chemical reactions are exactly the same thing.

Question 49

Hydrogen peroxide loses its potency when it is stored for extended periods of time because it spontaneously breaks down. The following figure illustrates this breakdown, but it is missing a product molecule. Which of the following symbols represents the missing product in this reaction?

A)a
B)b
C)c
D)d
E)e

Question 50

The following reaction is the formation of a peptide from two amino acids. This sort of reaction occurs in the body as part of the synthesis of proteins. This reaction is missing a component. Which of the following is missing? 2 NH₂CH₂COOH → NH₂CH₂CONHCH₂COOH

A) Nothing is missing.
B) H₂O is missing from the reactant side of the equation.
C) H₂O is missing from the product side of the equation.
D) O₂ is missing from the reactant side of the equation.
E) O₂ is missing from the product side of the equation.

Question 51

During metabolism, table sugar (sucrose) is broken down into monosaccharides. Which of the following equations could you use to determine the moles of monosaccharides produced when 3 moles of sucrose react with 3 moles of water?

A)a
B)b
C)c
D)d
E)e

Question 52

What does it mean for a chemical equation to be balanced?

A) A balanced chemical equation describes a chemical reaction found in nature.
B) A balanced chemical equation describes a chemical reaction that produces only some product, so there is an equal amount of reactant and product.
C) A balanced chemical equation contains an equal number of each type of atom on both sides of the equation.
D) A balanced chemical equation can run either forward or backward.
E) A balanced chemical equation represents a chemical reaction that is part of metabolism.

Question 53

The industrial nitrogen fixing reaction used in the preparation of fertilizers and other nitrogen containing compounds is called the Haber process. The chemical equation for this process is shown below. According to this reaction, how many moles of ammonia would you produce if you reacted one mole of N₂ with three moles of H₂? N₂ + 3 H₂ → 2 NH₃

A) 0
B) 1
C) 2
D) 3
E) 4

Question 54

In the body, glucose is broken down in the presence of oxygen into carbon dioxide and water. The balanced chemical equation for this reaction is shown below. According to this equation, how many molecules of carbon dioxide are produced when three molecules of glucose are metabolized in the presence of 18 moles of oxygen? C₆H₁₂O₆ + 6 O₂ → 6 CO₂ + 6 H₂O

A) 0
B) 6
C) 12
D) 18
E) 24

Question 55

Which of the following reactions is balanced?

A) CH₃CH₂CH₃ + O₂ → CO₂ + H₂O
B) CH₃CH₂CH₃ + O₂ → 3 CO₂ + 4 H₂O
C) CH₃CH₂CH₃ + 10 O₂ → 3 CO₂ + 4 H₂O
D) CH₃CH₂CH₃ + 5 O₂ → 3 CO₂ + 4 H₂O
E) None of these are balanced.

Question 56

The balanced equation for the combustion of propane is given below. What do the numbers in front of the molecules (the coefficients) mean? CH₃CH₂CH₃ + O₂ → 3 CO₂ + 4 H₂O

A) Three molecules of CO₂ are produced when one molecule of CH₃CH₂CH₃ reacts with one molecule of O₂.
B) Six molecules of CO₂ are produced when two molecules of CH₃CH₂CH₃ react with two molecules of O₂.
C) Nine moles of CO₂ are produced when three moles of CH₃CH₂CH₃ react with three moles of O₂.
D) Four moles of H₂O are produced when one mole of CH₃CH₂CH₃ reacts with one mole of O₂.
E) All of the above

Question 57

Under what circumstances is mass conserved?

A) Mass is conserved only in the laboratory.
B) Mass is conserved only theoretically.
C) Mass is conserved everywhere except the human body.
D) Mass is conserved in nature, but not in the laboratory.
E) Mass is conserved during all chemical reactions.

Question 58

Your friend combines vinegar (which contains acetic acid, CH₃COOH) and baking soda (NaHCO₃) and ends up with a runny foam. Your friend is pretty sure that the reaction produces water and carbon dioxide, which he can see just by looking at the foam, but he is unsure of what else the reaction produces. Given the partial reaction below, what do you tell your friend? NaHCO₃ + CH₃COOH → H₂O + CO₂ + ?

A) This reaction also produces CH₃COONa.
B) This reaction also produces CH₄.
C) This reaction also produces O₂.
D) This reaction only produces H₂O and CO₂.
E) This reaction probably produces something else, but it is not possible to determine the identity of the other product(s).

Question 59

The following chemical equation is not balanced. What must be done to the equation to make it balanced?

A) Change the coefficients to: 2 for Al, 3 for CuO and 3 for Cu.
B) Change the subscripts of CuO to CuO₃.
C) Add a molecule of AlO.
D) Change the state of matter in the reactants.
E) Change the subscripts of Al₂O₃ to be AlO.

Question 60

During metabolism, table sugar (sucrose) is broken down into monosaccharides. According to the following chemical equation, how many moles of monosaccharides will be produced when 6 moles of sucrose react with 6 moles of water? C₁₂H₂₂O₁₁ + H₂O → 2 C₆H₁₂O₆
Sucrose monosaccharides

A) 0
B) 2
C) 4
D) 6
E) 12

Question 61

A common, over-the-counter antacid is Al(OH)₃. This antacid reacts with gastric juice (HCl) in the stomach, producing AlCl₃ and H₂O. Which of the following equations can be used to correctly determine how much gastric juice (HCl) reacts with an antacid tablet containing 0.25 grams Al(OH)₃?

A)
B)
C)
D)
E)

Question 62

How many atoms of magnesium are present in the reactants of this chemical equation? Mg(OH)₂ + 2 HCl → MgCl₂ + 2 H₂O

A) 0
B) 1
C) 2
D) 3
E) 4

Question 63

Combustion reactions are ___________ because products of the reaction are _________ in potential energy than the reactants.

A) endothermic; higher
B) exothermic; higher
C) endothermic; lower
D) exothermic; lower
E) endothermic; the same

Question 64

The steps for performing stoichiometry calculations are diagramed below: According to these steps, which of the following equations would allow you to calculate the yield of monosaccharides when 28 g of sucrose is broken down as shown in the following equation?

A)a
B)b
C)c
D)d
E)e

Question 65

Pentane (C₅H₁₂) reacts with oxygen gas (O₂) to form carbon dioxide (CO₂) and water (H₂O) according to the following reaction. What is the coefficient for carbon dioxide in the balanced equation? C₅H₁₂ + _?_ O₂ → _?_ CO₂ + _?_ H₂O

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

Question 66

The balanced chemical equation for the combustion of propane (C₃H₈) is given below. How many grams of carbon dioxide (CO₂) are released when 35 g of propane are burned in the presence of excess oxygen? C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O

A) 0.80 g
B) 12 g
C) 35 g
D) 105 g
E) 1500 g

Question 67

How many atoms of hydrogen are present in the products of this chemical equation? Mg(OH)₂ + 2 HCl → MgCl₂ + 2 H₂O

A) 0
B) 1
C) 2
D) 3
E) 4

Question 68

Pentane (C₅H₁₂) reacts with oxygen gas (O₂) to form carbon dioxide (CO₂) and water (H₂O) according to the following reaction. What is the coefficient for oxygen in the balanced equation? C₅H₁₂ + _?_ O₂ → _?_ CO₂ + _?_ H₂O

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

Question 69

The name for the heat energy released or absorbed in a chemical reaction is

A) energy.
B) endothermic.
C) exothermic.
D) enthalpy.
E) entropy.

Question 70

According to the balanced chemical equation below, if, you react 28 grams of butene with excess hydrogen, how many grams of butane would you expect to get?

A) 0.0 g
B) 29 g
C) 58 g
D) 112 g
E) 116 g

Question 71

Is this chemical equation balanced? Mg(OH)₂ + 2 HCl → MgCl₂ + 2 H₂O

A) No. The number of magnesiums in the reactants is different from the number in the products.
B) No. The number of hydrogens in the reactants is different from the number in the products.
C) No. The number of oxygens in the reactants is different from the number in the products.
D) No. The number of chlorines in the reactants is different from the number in the products.
E) Yes. The same number of each type of atom is present in the reactants and products.

Question 72

Pentane (C₅H₁₂) reacts with oxygen gas (O₂) to form carbon dioxide (CO₂) and water (H₂O) according to the following reaction. What is the coefficient for water in the balanced equation?

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

Question 73

Acetylene (C₂H₂) is a small organic molecule used in the industrial preparation of many other molecules and also in welding. Acetylene is made from calcium carbide and water, resulting in acetylene and also calcium hydroxide. Which of the following choices is the correct balanced chemical equation for the preparation of acetylene?

A) CaC₂ + H₂O → CaO + C₂H₂
B) CaC₂ + H₂O → Ca(OH)₂ + C₂H₂
C) CaC₂ + 2 H₂O → Ca(OH)₂ + C₂H₂
D) CaC₂ + 2 H₂O → CaO + C₂H₂ + H₂O
E) 2 CaC₂ + H₂O → Ca(OH)₂ + 2 C₂H₂

Question 74

According to the balanced chemical equation below, if you react 3.0 mole of butene with 3.0 mole of hydrogen, how many moles of butane would you expect to get?

A) 0.0 moles
B) 1.0 mole
C) 2.0 moles
D) 3.0 moles
E) 6.0 moles

Question 75

Which of the following biological molecules are the major nutrients that make up the food that we eat?
I. proteins
II. nucleic acids
III. steroids
IV. fats
V. carbohydrates

A) All of these are major nutrients.
B) I, II, IV, and V
C) I and V
D) III, IV, and V
E) I, IV, and V

Question 76

By moving, breathing, and living, you do work every day. Work requires energy. Where does this energy come from?

A) The energy comes from food; it undergoes chemical reactions in the cells.
B) The energy does not come from anyplace; it is always in our bodies.
C) The energy comes from breaking bonds in food.
D) The energy comes from breaking bonds in food, oxygen, and water.
E) No one really understands where this energy comes from.

Question 77

How many atoms of oxygen are present in the reactants of this chemical equation? Mg(OH)₂ + 2 HCl → MgCl₂ + 2 H₂O

A) 0
B) 1
C) 2
D) 3
E) 4

Question 78

The balanced chemical equation for the combustion of butane is given below. How many grams of O₂ are needed to completely react with 5.0 g of butane in a butane lighter? 2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O

A) 0.42 g
B) 2.8 g
C) 6.0 g
D) 9.1 g
E) 18 g

Question 79

According to the balanced chemical equation below, if you react 3.0 mole of butene with 3.0 mole of hydrogen, how many grams of butane would you expect to get?

A) 0.0 grams
B) 3.0 gram
C) 58 grams
D) 56 grams
E) 170 grams

Question 80

Which of the following reactions is NOT balanced?

A) 2 Al + 6 HCl → 2 AlCl₃ + 3 H₂
B) Fe₂O₃ + 2 Al → 2 Fe + Al₂O₃
C) C₆H₁₂O₆ + 6 O₂ → 6 CO₂ + 6 H₂O
D) C₂H₅OH + O₂ → 2 CO₂ + 3 H₂O
E) CaO + 3 C → CaC₂ + CO