Chemistry for Life Sciences Chapter Exam Questions - 986 Verified Questions

Chemistry for Life Sciences

Chapter Exam Questions

Course Introduction

Chemistry for Life Sciences introduces students to fundamental chemical concepts and principles with an emphasis on their applications in biological systems. Topics include atomic structure, chemical bonding, thermodynamics, kinetics, acids and bases, and the chemistry of biomolecules such as carbohydrates, proteins, lipids, and nucleic acids. Through lectures, laboratory experiments, and problem-solving exercises, students learn how chemical processes underpin vital biological functions and develop skills in analytical thinking and scientific methodology relevant to careers in life sciences, medicine, and related fields.

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Introductory Chemistry An Active Learning Approach 6th Edition by Mark S. Cracolice

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Chapter 2: Matter and Energy

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Q1) Which of the following changes is/are endothermic for the underlined object?

i.baking a potato

ii.a person being burned by a pan

iii.a wood log burning

iv.a lit light bulb shining

v.a person digesting food

A)iii only

B)iii and iv

C)iii and iv.

D)i and iv

E)i and ii

Answer: E

Q2) Under what condition is the Law of Conservation of Energy not obeyed?

A)Digestion of food

B)Human (and some animal) metabolism of sports drinks

C)High speed travel, such as in military jets and the space shuttle

D)Nuclear changes

E)The Law of Conservation of Energy is always obeyed

Answer: D

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Page 3

Chapter 3: Measurement and Chemical Calculations

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Q1) What will be the cost in dollars for photocopies if you have 32 pages in a booklet,you need 175 booklets,and copies are 4.5 cents each?

A)$12.44

B)$24.61

C)$39.68

D)$252

E)$25,200

Answer: D

Q2) What is the volume of a 5.00 g pure aluminum cylinder if its density is 2.70 g/cm³?

A)5.00 cm³

B)1.85 cm³

C)13.5 cm³

D)0.540 cm³

E)7.41 × 10^-2 cm³

Answer: B

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4

Chapter 4: Introduction to Gases

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Q1) A fixed quantity of a gas is maintained at a constant temperature.The gas has a volume of 0.847 m³ at 735 torr.What is the pressure of the gas when the volume is changed to 0.905 m³?

A)0.00145 torr

B)0.00127 torr

C)781 torr

D)563 torr

E)688 torr

Q2) The volume of a sealed gas balloon is changed from 953 mL to 808 mL at constant temperature.The original pressure was 155 kPa.What is the pressure after the volume is reduced ?

A)0.00547 kPa

B)0.00761 kPa

C)131 kPa

D)183 kPa

E)1.19 × 10⁸ kPa

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Chapter 5: Atomic Theory: The Nuclear Model of the Atom

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Q1) Which of the following is the best explanation of why the mass of an atom is usually expressed in atomic mass units rather than grams?

A)An atomic mass unit is only used for carbon-12

B)The mass of one milliliter of water is one gram

C)The mass in grams is not known for atoms

D)The mass of an atom in grams is inconveniently small

E)Metric units such as grams are not applicable to atoms

Q2) Which of the following is not one of the main features of Dalton's atomic theory?

A)Each element is made up of tiny, individual particles called atoms

B)Atoms are indivisible; they cannot be created or destroyed

C)Mass differences among atoms of an element are caused by different numbers of neutrons

D)Atoms of one element are different from atoms of any other element

E)Atoms of one element may combine with atoms of another element to form chemical compounds

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Chapter 6: Chemical Nomenclature

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Q1) What are the names of the compounds Ni(HCO₃)₂ and CrCl₂?

A)nitrogen hydrogen carbonate, chromic chloride

B)nitrogen hydrogen carbonate, copper(II) chloride

C)nickel hydrogen carbonate, copper chloride

D)nickel(II) hydrogen carbonate, chromium(II) chloride

E)nickel hydrogen carbonate, chromium chloride

Q2) Which of the following is the correct formula for ammonia?

A)NH₃

B)NH₄⁺

C)Hg₂²⁺

D)Hg²⁺

E)None of the choices is correct

Q3) What are the formulas of the compounds zinc phosphide and potassium hydrogen phosphate?

A)Zn₂P₃, K₂HPO₄

B)Zn₃P₂, K₂HPO₄

C)Zn₂P₃, KHPO₄

D)Zn₃P₂, KHPO₄

E)Zn₂P₃, KH₂PO₄

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Chapter 7: Chemical Formula Relationships

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Q1) Calculate the mass of silver in a sample of silver sulfide that contains 0.890 g of sulfur.

A)1.08 g

B)1.78 g

C)3.00 g

D)5.99 g

E)6.89 g

Q2) A compound analyzes as 18.0% carbon,2.26% hydrogen,and 79.7% chlorine.Calculate the empirical formula of the compound.

A)C₄H₃Cl₄

B)C₃H₂Cl₂

C)C₃H₃Cl₂

D)C₂H₂Cl₃

E)C₂H₃Cl₃

Q3) List the number of atoms of each element in a formula unit of ammonium sulfate.

A)1 nitrogen atom, 4 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms

B)1 nitrogen atom, 3 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms

C)2 nitrogen atoms, 6 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms

D)2 nitrogen atoms, 8 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms

E)1 nitrogen atom, 4 hydrogen atoms, 2 sulfur atoms, 8 oxygen atoms

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Chapter 8: Chemical Reactions

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Q1) The combination of copper (II)nitrate and ammonium sulfide solutions yields a precipitate.Write the balanced chemical equation for this reaction.What is the coefficient for copper (II)nitrate?

A)3

B)1

C)5

D)2

E)4

Q2) When potassium contacts fluorine gas,potassium fluoride is produced.Write the balanced chemical equation for this reaction.What is the coefficient for potassium fluoride?

A)1

B)2

C)3

D)4

E)5

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Chapter 9: Chemical Change

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Q1) Which of the following is the best explanation of why a weak acid is a poor conductor?

A)The weak acid molecules undergo a precipitation reaction in aqueous solution

B)The weak acid molecules move too slowly to conduct well

C)It is only slightly ionized in water

D)It can form only dilute solutions in water

E)It will not dissolve in water

Q2) What ions are present in what ratio in an aqueous solution of iron(III)sulfate?

A)Fe₂²⁺(aq) + SO₄^2-(aq)

B)Fe₂²⁺(aq) + SO₃^2-(aq)

C)2 Fe³⁺(aq) + 12 SO^2-(aq)

D)2 Fe³⁺(aq) + 3 SO₄^2-(aq)

E)Fe³⁺(aq) + S^2-(aq) + O^2-(aq)

Q3) Which of the following is the best explanation of why a strong acid is an excellent conductor?

A)It is almost completely ionized in water

B)It undergoes a vigorous chemical reaction with the water molecules

C)It is immiscible in water

D)All acids are natural conductors

E)It reduces electronic vibration and thus allows greater conductivity

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Chapter 10: Quantity Relationships in Chemical Reactions

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Q1) How much energy is required to produce 1.00 kg of aluminum by the reaction 2 Al₂O₃(s)+ 3 C(s)+ 1.97 × 10³ kJ 4 Al(s)+ 3 CO₂(g)?

A)5.50 × 10^-5 kJ

B)7.52 × 10^-2 kJ

C)2.70 × 10³ kJ

D)7.30 × 10⁴ kJ

E)1.83 × 10⁴ kJ

Q2) How many moles of bromine will react with 0.0500 mole of C₂H₂ in the reaction C₂H₄ + Br₂ C₂H₄Br₂?

A)0.100 mol

B)0.186 mol

C)0.0250 mol

D)0.0500 mol

E)2.00 mol

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11

Chapter 11: Atomic Theory: The Quantum Model of the Atom

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Q1) Which of the following pairs of atomic numbers belong to elements whose atoms have the highest occupied energy level electron configuration of the form ns²np²?

A)23 and 26

B)4 and 20

C)30 and 80

D)6 and 82

E)22 and 72

Q2) Which general electron configuration is responsible for the family properties of noble gases?

A)ns¹

B)ns²

C)ns²np⁴

D)ns²np⁵

E)ns²np⁶

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Chapter 12: Chemical Bonding

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Q1) When a covalent bond forms,the atomic orbitals of the separated atoms:

A)repel one another

B)change from s orbitals to p orbitals

C)change from p, d, or f orbitals to s orbitals

D)cease to exist because the electrons transfer out of the orbitals

E)overlap

Q2) Which of the following correctly describes a cation?

A)A positively charged ion

B)An ion formed by the addition of electrons to the neutral atom

C)An ion formed mostly by the nonmetals

D)An ion that contains a greater number of electrons than protons

E)An ion formed by elements on the right side of the periodic table

Q3) Which of the following is the best classification for a bond in which bonding electrons are shared unequally?

A)Nonpolar covalent

B)Polar covalent

C)Electronegative

D)Multiple

E)Completely ionic

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Page 13

Chapter 13: Structure and Shape

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Q1) Which of the following molecules is/are polar?

i.HF

ii.BH₃

iii.CBr₂F₂

iv.PF₃

A)ii only

B)i and ii

C)ii and iv

D)i, iii, and iv

E)i, ii, iii, and iv

Q2) Which of the following types of compounds best describes organic compounds?

A)Carbon compounds

B)Molecular compounds

C)Ionic compounds

D)Covalent compounds

E)Ring compounds

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Chapter 14: The Ideal Gas Law and Its Applications

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Q1) What is the molar mass of a gas if 1.070 g of the gas occupies 264 mL at 100°C and 768 torr?

A)0.123 g/mol

B)0.162 g/mol

C)32.9 g/mol

D)64.0 g/mol

E)123 g/mol

Q2) Calculate the molar volume of a gas at 21°C and 3.73 atm.

A)0.462 L/mol

B)0.155 L/mol

C)351 L/mol

D)4.92 × 10³ L/mol

E)6.47 L/mol

Q3) Calculate the density of nitrogen dioxide at STP.

A)2.70 × 10^-3 g/L

B)0.487 g/L

C)22.7 g/L

D)2.03 g/L

E)1.88 g/L

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Page 15

Chapter 15: Gases, Liquids, and Solids

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Q1) The specific heat of solid gold is 0.13 J/g °C.How much heat is needed to raise the temperature of 25.0 g of gold from 23°C to its melting point at 1063°C?

A)3.5 kJ

B)3.4 kJ

C)0.14 kJ

D)2.0 × 10³ kJ

E)3.3 kJ

Q2) The total pressure exerted by the oxygen saturated with water vapor is 764 torr at a temperature at which water vapor pressure is 26 torr.Find the partial pressure of the oxygen.

A)0.0340 torr

B)29.4 torr

C)738 torr

D)790 torr

E)1.99 × 10⁴ torr

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16

Chapter 16: Solutions

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Q1) Identify the incorrect statement about events that occur between the time excess solid solute is first introduced to a liquid solvent and the time when the solution becomes saturated.Assume that the surface area of the solute remains constant throughout the process.

A)The rate of concentration change is zero when the solution is saturated

B)The net rate of concentration change is greatest at the beginning of the process

C)The rate of dissolving is greater than the rate of crystallization when the solution is one-half saturated

D)If temperature remains constant, the rate of dissolving is constant

E)If temperature remains constant, the rate of crystallization remains constant

Q2) Calculate the increase in boiling point of a solution made by dissolving 40.0 g of glucose,C₆H₁₂O₆,in 250.0 g of water.K_b for water is 0.52°C/m.

A)0.12°C

B)0.46°C

C)0.59°C

D)1.7°C

E)83.2°C

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Page 17

Chapter 17: Acidbase Proton Transferreactions

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Q1) According to Arrhenius theory,what is an acid?

A)A substance that contains a high concentration of hydrogen ions in solutions with water

B)A substance that will lower the hydrogen ion concentration when placed in water

C)A substance that has an H in its formula

D)An electron pair donor

E)An electron pair acceptor

Q2) A water solution is considered acidic when what is true?

A)[H⁺] = [OH^-]

B)[H⁺] < [OH^-]

C)[OH^- ] > [H⁺]

D)[H⁺] > [OH^-]

E)[H⁺] = K_w

Q3) What is the pH of a solution if [H⁺] = 3.1 × 10^-4 molar?

A)pH = 4.31

B)pH = 10.49

C)pH = -9.69

D)pH = -3.51

E)pH = 3.51

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Page 18

Chapter 18: Chemical Equilibrium

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Q1) Which of the following conditions is not found in a system that is at equilibrium?

A)Reactants and products are being converted into one another continually

B)The forward rate of reaction is equal to the rate of the reverse reaction

C)The concentration of reactants is equal to the concentration of the products

D)The system is closed and isolated from its surroundings

E)The reaction can be represented by an equation with a double arrow

Q2) How does a catalyst alter the rate of a reaction?

A)Catalysts replace part of the reactants

B)Catalysts provide the activation energy needed

C)A catalyst interferes with the attainment of chemical equilibrium

D)Catalysts provide more heat to the reaction, and the increased temperature leads to an increased reaction rate

E)Catalysts provide a reaction pathway with a lower energy of activation

Q3) If the position of equilibrium shifts to the left,what will happen?

A)The concentration of products will increase

B)The concentration of reactants will increase

C)The temperature will rise

D)The temperature will decrease

E)The concentrations of both products and reactants will increase

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Page 19

Chapter 19: Oxidationreduction Electron Transferreactions

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Q1) Reduction can be defined as...

A)a increase in oxidation number

B)the gain of protons

C)the loss of protons

D)a gain of electrons

E)a loss of electrons

Q2) What evidence suggests that Na⁺ ions are very weak oxidizing agents?

A)NaCl is a strong electrolyte

B)Na metal does not occur in the Earth's crust

C)NaOH is a strong base

D)Na metal is soft and can be cut with a knife

E)Na⁺ ions are a component of table salt

Q3) What is the oxidation number of sulfur in sulfite ion,SO₃^2-? A)+6 B)+4

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Chapter 20: Nuclear Chemistry

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Q1) A waste sample exhibits radioactivity.In order to determine the total level of radioactivity of the sample,which of the following should be used?

A)Geiger counter

B)scintillation counter

C)gamma camera scanner

D)a combination of a Geiger and a scintillation counter.

Q2) Which of the following is the best description of the main obstacle to be overcome before energy can be obtained from fusion?

A)Safe storage and disposal of the radioactive waste

B)Radiation emitted from the plant itself

C)The extremely high temperature needed to start and sustain the reaction

D)A more abundant source of fuel

E)Better purification methods to separate the fuel

Q3) Which of the following is the best definition of the term transmutation?

A)Conversion of an atom from one element to another by means of a nuclear change

B)A change that appears to take place by itself without outside influence

C)The nucleus of a helium atom, often emitted in nuclear disintegration

D)To change chemically into simpler substances

E)A high-energy photon emission in radioactive disintegration

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Page 21

Chapter 21: Organic Chemistry

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Q1) A certain compound is a gas at room temperature and undergoes only substitution reactions.Which of the following is most likely to be this compound?

A)C₄H₁₀

B)C₆H₁₀

C)C₇H₁₄

D)C₉H₁₈

E)Any of is a possibility

Q2) Which of the following compounds is/are (an)aldehyde(s)?

i.CH₃-OH

ii.CH₃-CO-CH₃

iii.CH₃-O-CH₃

iv.CH₃-CHO

v.CH₃-COO-CH₃

A)ii only

B)iii only

C)iv only

D)i and iv

E)ii, iii, and v

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Chapter 22: Biochemistry

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Q1) Which of the following bases is not found in RNA?

A)Thymine

B)Guanine

C)Cytosine

D)Uracil

E)Adenine

Q2) Which of the following bases is not found in DNA?

A)Thymine

B)Guanine

C)Cytosine

D)Uracil

E)Adenine

Q3) In simple sugars,every carbon but one contains a hydroxyl group; the remaining carbon is double bonded to an oxygen atom as a carbonyl group.What type of sugar has the carbonyl at the end of the carbon chain?

A)Cretose

B)Polysaccharide

C)Disaccharide

D)Aldose

E)Ketose

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