Chemistry for Life Sciences Exam Answer Key - 3323 Verified Questions

Chemistry for Life Sciences

Exam Answer Key

Course Introduction

Chemistry for Life Sciences introduces fundamental chemical principles with a focus on their relevance to biological systems. The course covers atomic and molecular structure, chemical bonding, thermodynamics, acids and bases, and the properties of solutions, all within the context of life processes. Emphasis is placed on understanding biochemical molecules, such as proteins, nucleic acids, lipids, and carbohydrates, and exploring how chemical reactions underpin cellular function, metabolism, and energy production. Designed for students pursuing life sciences, this course equips learners with the chemical foundation necessary to comprehend complex biological phenomena and prepares them for advanced study in biology, biochemistry, medicine, and related fields.

Recommended Textbook

General Chemistry Principles and Modern Applications 11th Edition by Ralph H. Petrucci

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28 Chapters

3323 Verified Questions

3323 Flashcards

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Page 2

Chapter 1: Matter: Its Properties and Measurement

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Sample Questions

Q1) If gasoline costs 98.5 cents per liter in Canada,what is the price in dollars per gallon?

A)$3.73

B)$3.94

C)$1.04

D)$4.16

Answer: A

Q2) Water is:

A)a mixture

B)a compound

C)an element

D)a molecule

E)an atom

Answer: B

Q3) The composition refers to the components of a sample of matter and their relative proportions.

A)True

B)False

Answer: True

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Chapter 2: Atoms and the Atomic Theory

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Sample Questions

Q1) Silver possesses two stable isotopes: ¹⁰⁷Ag (106.90 u)and ¹⁰⁹Ag (108.90 u).If the average atomic mass of Ag is 107.87 u,what is the percent abundance of ¹⁰⁷Ag?

A)48.5%

B)50.0%

C)51.5%

D)46.3%

E)53.8%

Answer: C

Q2) The three naturally occurring isotopes of magnesium are ²⁴Mg (23.985042 u,78.99%),²⁵Mg (24.985837,10.00%),and ²⁶Mg.What is the atomic mass of ²⁶Mg?

A)25.98 u

B)48.67 u

C)23.94 u

D)26.43 u

E)24.31 u

Answer: A

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Chapter 3: Chemical Compounds

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Sample Questions

Q1) What is the mass of 8.50 × 10²² molecules of NH₃?

A)0.00829 g

B)0.417 g

C)2.40 g

D)121 g

Answer: C

Q2) Choose the INCORRECT name formula combination.

A)HNO₂ nitrous acid

B)Fe₂(SO₄)₃ iron(III)sulfite

C)LiCN lithium cyanide

D)Na₂CO₃ sodium carbonate

E)Ba(OH)₂ barium hydroxide

Answer: B

Q3) What mass of ammonia,NH₃,contains the same number of molecules as 3.00 g of trichlorofluoromethane,CCl₃F?

A)0.0412 g

B)0.331 g

C)2.69 g

D)24.2 g

Answer: B

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Chapter 4: Chemical Reactions

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Sample Questions

Q1) In the following reaction: 2 KClO₃(s) 2 KCl(s)+ 3 O₂(g)

14.0 g KClO₃ yielded 1.40 g KCl.What is the percent yield?

A)6.08%

B)16.4%

C)11.0%

D)32.9%

E)10.0%

Q2) For the reaction symbolized as HCl(aq)+ NaOH(aq) NaCl(aq)+ H₂O(l)water is both:

A)a reactant and the solute

B)a reactant and the solvent

C)a product and the solute D)a product and the solvent E)a liquid and the intermediate

Q3) How many grams of NaOH (MW = 40.0 g mol^-1)are there in 250.0 mL of a 0.275 mol L^-1 NaOH solution?

Q4) How many grams of H₃PO₄ are in 265 mL of a 1.50 mol L^-1 solution of H₃PO₄ (aq)?

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Chapter 5: Introduction to Reactions in Aqueous Solutions

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Sample Questions

Q1) Which of the compounds of H₂C₂O_4,

Ca(OH)₂,KOH,and HI behave as acids when they are dissolved in water?

A)Ca(OH)₂ and KOH

B)H₂C₂O₄ and HI

C)only HI

D)only KOH

Q2) A solid forming from a mixture of solutions is called a precipitate.

A)True

B)False

Q3) In an acid-base neutralization reaction,38.74 mL of 0.500 mol L^-1 potassium hydroxide reacts with 50.00 mL of sulfuric acid solution.What is the concentration of the H₂SO₄ solution?

A)0.194 mol L^-1

B)0.387 mol L^-1

C)0.775 mol L^-1

D)1.29 mol L^-1

Q4) Soluble ionic compounds form strong electrolytes.

A)True

B)False

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Chapter 6: Gases

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Sample Questions

Q1) In a sample of air at STP,the ratio of the root-mean-square velocity of O₂ to that of N₂,that is u_rms(O₂)/u_rms(N₂),is equal to

A)0.88

B)0.94

C)1.00

D)1.07

E)1.14

Q2) If someone were to light a cigar at one end of a closed room,persons at the other end of the room might soon perceive an odor due to gaseous emissions from the cigar.Such a phenomenon is an example of:

A)monometry

B)ideality

C)effusion

D)diffusion

E)barometry

Q3) Pressure is a force per unit area with the SI unit of 1 pascal.

A)True

B)False

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Chapter 7: Thermochemistry

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Sample Questions

Q1) Given that _fH° [Ag₂S(s)] = -32.6 kJ/mole,what is the enthalpy change for the precipitation of argentite,Ag₂S(s)?

_fH° [Ag⁺(aq)] = +105.6 kJ/mol _fH° [S^2-(aq)] = +33.05 kJ/mol

A)-276.9 kJ/mol

B)-106.1 kJ/mol

C)+171.2 kJ/mol

D)+106.1 kJ/mol

E)+138.7 kJ/mol

Q2) 100.0 g of nickel at 150 °C was placed in 1.00 L of water at 25.0 °C.The final temperature of the nickel-water mixture was 26.3 °C.What is the specific heat of the nickel?

A)0.14 J/g °C

B)0.13 J/g °C

C)0.55 J/g °C

D)0.44 J/g °C

E)0.23 J/g °C

Q3) A closed system can exchange matter but not energy with the surroundings.

A)True

B)False

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Chapter 8: Electrons in Atoms

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Sample Questions

Q1) The principle that is based on electrons attempting to be as far apart as possible is the:

A)Heisenberg Principle

B)Pauli Exclusion Principle

C)Bohr Theory

D)Hund's Rule

E)Aufbau principle

Q2) Chlorine (atomic number = 17)has the electronic configuration: ________.

A)1s²2s²2p⁶3s²3d⁵

B)1s²2s²2p⁶2d⁵3s²

C)1s²2s²2p⁶3s²3p⁵ D)1s²2s²2d¹⁰3s²

E)1s²2s²2p⁶2d⁶3s¹

Q3) When an electron in an atom goes from a high energy state to a low one,what occurs?

A)Another electron goes from a low energy state to a high one.

B)The atom moves faster.

C)Light is given off.

D)Light is absorbed.

E)This process is not possible.

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Chapter 9: The Periodic Table and Some Atomic Properties

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Sample Questions

Q1) Paramagnetic is not the same as magnetic.

A)True

B)False

Q2) Elements in the first two groups are part of the main-group elements along with which of the following groups?

A)d-block elements

B)s-block elements

C)actinides

D)lanthanides

E)p-block elements

Q3) The effective nuclear charge for sodium is:

A)+10

B)+9

C)+1

D)+11

E)0

Q4) The electron affinity is the energy for an atom in its standard state to gain an electron.

A)True

B)False

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Chapter 10: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) Which of the following molecules is polar?

A)NBr₃

B)CH₄

C)CS₂

D)NH₄⁺

E)PCl₅

Q2) Which chloride should have the greatest covalent character?

A)NaCl

B)BeCl₂

C)KCl

D)BaCl₂

E)CaCl₂

Q3) Which of the following must be paramagnetic?

A)F₂

B)N₂

C)SO₂⁺

D)H₂

E)ClO₂^-

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Chapter 11: Chemical Bonding Ii: Valence Bond and

Molecular Orbital Theories

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Sample Questions

Q1) Which combination of hybrid orbital descriptions and electron-group geometry descriptions is INCORRECT?

A)sp/linear

B)sp²/trigonal planar

C)sp³/tetrahedral

D)sp³^d/square planar

E)sp³^d²/octahedral

Q2) According to MO theory,assuming that the molecular orbitals are the same as a diatomic molecule,which is an INCORRECT statement for CN^-?

A)The BO is 2.

B)There are no unpaired electrons.

C)The ₂_p is the highest filled level.

D)The molecule is diamagnetic.

E)There are 10 electrons in the n = 2 level orbitals.

Q3) Molecular orbitals can be formed by adding and subtracting atomic orbitals.

A)True

B)False

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Page 13

Chapter 12: Intermolecular Forces: Liquids and Solids

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Sample Questions

Q1) The heat of fusion for napthalene (C₁₀H₈)is 18.98 kJ/mol and for sodium is 2.60 kJ/mol.The amount of heat that would melt 37.0 grams of napthalene would melt how many grams of sodium?

A)0.909 g

B)1510 g

C)28.3 g

D)48.4 g

E)270.g

Q2) Arrange the following compounds in order of increasing boiling point: HCl,HBr,HI.

A)HCl,HBr,HI

B)HBr,HI,HCl

C)HI,HBr,HCl

D)HCl,HI,HBr

E)HI,HCl,HBr

Q3) The heat of deposition equals the negative of the heat of sublimation.

A)True

B)False

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14

Chapter 13: Spontaneous Change: Entropy and Gibbs Energy

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Sample Questions

Q1) A zero G means the system is at equilibrium.

A)True

B)False

Q2) Which of the following has the highest entropy?

A)1 mole of liquid water at 30 °C

B)1 mole of water vapor at 30 °C

C)1 mole of regular ice at -10 °C

D)1 mole of "dry ice" at -10 °C

E)1 mole of water under 10 atm of pressure at -10 °C

Q3) Which material has the largest entropy?

A)pure water

B)powdered sugar

C)salt water

D)crystalline salt

E)cannot be determined

Q4) As the activity a of a substances increases so does its chemical potential m.

A)True

B)False

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Chapter 14: Solutions and Their Physical Properties

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Sample Questions

Q1) Which of the following compounds has the highest aqueous solubility?

A)CaCl₂

B)SrI₂

C)CaI₂

D)MgI₂

E)CaBr₂

Q2) In the solution,a solute is present in the greatest quantity.

A)True

B)False

Q3) A magnesium sulfate heptahydrate solution,which is 18.00% by weight in the anhydrous compound,has a density at 20 °C of 1.20 g/mL.What is the molarity of the anhydrous compound in the solution? (Atomic masses in au: H = 1.0,O = 16.0,S = 32.1,Mg = 24.3)

A)5.54 M

B)1.79 M

C)1.82 M

D)1.25 M

E)1.49 M

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Chapter 15: Principles of Chemical Equilibrium

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Sample Questions

Q1) For the reaction below CO(g)+ 2 H₂(g) CH₃OH(g)

The equilibrium concentrations at 483 K are [CO] = 0.0753 M,[H₂] = 0.151 M,and [CH₃OH] = 0.0247 M.Calculate the value of K_c.

A)14.4

B)1.09

C)2.17

D)0.0694

E)0.917

Q2) Equilibrium constant K is constant except when one varies the:

A)concentrations of the reactants

B)temperature of the reaction

C)concentration of the products

D)partial pressures of the reactants

E)K always remains constant

Q3) Large value for equilibrium constant K means the reaction will be less complete at the equilibrium point.

A)True

B)False

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Page 17

Chapter 16: Acids and Bases

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Sample Questions

Q1) Choose the Br nsted-Lowry acids and bases in the following equation: HCO₃^- + OH^- H₂O + CO₃^2-

A)acids HCO₃^-,H₂O bases OH^-,CO₃^2-

B)acids OH^-,CO₃^2- bases HCO₃^-,H₂O

C)acids

H₂O,OH^- bases HCO₃^-,CO₃^2- D)acids HCO₃^-,OH^- bases CO₃^2-,H₂O

E)acids H₂O,CO₃^2- bases HCO₃^-,OH^-

Q2) Br nsted and Lowry suggested that bases be defined as proton acceptors.

A)True

B)False

Q3) The first ionization step is approximately 100% for H₂SO₃.

A)True

B)False

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Page 18

Chapter 17: Additional Aspects of Acidbase Equilibria

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Sample Questions

Q1) Determine the [C₂H₃O₂^-] of the following aqueous solution.Initial concentrations are given. [HC₂H₃O₂] = 0.250 M,[HI] = 0.120 M K_a (acetic acid)= 1.8 × 10^-5

A)8.6 × 10^-6M

B)3.8 × 10^-5M

C)1.8 × 10^-5M

D)0.25 M

E)0.37 M

Q2) Calculate the pH of a 1.00 L solution of 0.100 M NH₃(aq)after the addition of 0.010 mol HCl(g).For NH₃,pK_b = 4.74.

A)10.21

B)9.26

C)8.31

D)11.46

E)7.00

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Chapter 18: Solubility and Complex-Ion Equilibria

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Sample Questions

Q1) Concentrated aqueous solutions of iron (III)chloride,sodium hydroxide,and potassium nitrate are mixed together.The precipitate which forms is ________.

A)potassium hydroxide

B)sodium chloride

C)iron (III)hydroxide

D)iron (III)nitrate

E)nothing precipitates

Q2) What is the free Cu²⁺(aq)concentration if 0.020 M Cu²⁺(aq)solution is mixed with an equal volume of 4.0 M NH₃(aq)?

K_f for [Cu(NH₃)₄]²⁺ is 1.1 × 10¹³.

A)5.7 × 10^-15M

B)2.8 × 10^-16M

C)6.2 × 10^-17M

D)4.5 × 10^-15M

E)1.7 × 10^-16M

Q3) The pH of a solution may affect solubility only if the salt contains the OH^- ion.

A)True

B)False

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Chapter 19: Electrochemistry

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Sample Questions

Q1) Determine E°_cell for the reaction: 2 Ag⁺(aq)+ Mg(s) 2 Ag(s)+ Mg²⁺(aq).The half reactions are: Mg²⁺(aq)+ 2 e^- Mg(s)E° = -2.356 V Ag⁺(aq)+ e^- Ag(s)E° = 0.800 V

A)0.756 V

B)-0.756 V

C)3.156 V

D)-1.556 V

E)1.556 V

Q2) How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu²⁺ ions to produce 5.00 moles of copper metal?

A)0.187 hours

B)0.373 hours

C)2.68 hours

D)5.36 hours

Q3) A primary battery is recharged by passing electricity through the battery.

A)True

B)False

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Chapter 20: Chemical Kinetics

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Sample Questions

Q1) A heterogeneous catalyst is a catalyst that is in two phases of matter.

A)True

B)False

Q2) The reaction 2 H₂ + NO H₂O + 1/2N₂ is first order in H₂ and second order in NO.The rate law is ________.

A)k[H₂]²[NO]

B)k[H₂][NO]²

C)k[H₂]

D)k[H₂][NO]

E)k[H₂][NO]^-2

Q3) Calculate rate constant k for a first order reaction with a half-life of 75.0 min.

A)52.0 min^-1

B)1.54 × 10^-4 min^-1

C)1.33 × 10^-2 min^-1

D)9.24 × 10^-3 min^-1

E)2.67 × 10^-2 min^-1

Q4) Temperature has no effect on reaction rate.

A)True

B)False

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Chapter 21: Chemistry of the Main-Group Elements I:

Groups 1,2,13,and 14

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Sample Questions

Q1) What mass of potassium superoxide could be prepared from 15.6 g of potassium metal and excess oxygen?

A)37.6 g

B)15.6 g

C)22.0 g

D)28.4 g

E)0.399 g

Q2) Water treatment using a cation-exchange resin in the H⁺ form,followed by an anion-exchange resin in the OH^- form,unlike the processes using typical zeolites or synthetic resins regenerated by sodium chloride,can produce:

A)brine water

B)deionized water

C)distilled water

D)hard water

E)soft water

Q3) A magnesium fire can always be extinguished with carbon dioxide.

A)True

B)False

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Chapter 22: Chemistry of the Main-Group Elements Ii:

Groups 18,17,16,15,and Hydrogen

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Q1) Write an equation for the oxidation in aqueous acidic solution of Mn²⁺(aq)to MnO₄^-(aq)by XeO₃(aq),which is reduced to Xe(g).

A)6 Mn²(aq)⁺ + 5 XeO₃(aq) 6 MnO₄^-(aq)+ 5 Xe(g)

B)24 H₂O(l)+ 6 Mn²⁺(aq)+ 5 XeO₃(aq) 6 MnO₄^-(aq)+ 5 Xe(g)+ 18 H⁺(aq) C)H₂O(l)+ Mn²⁺(aq)+ XeO₃(aq) MnO₄^-(aq)+ Xe(g)+ 2 H⁺(aq)

D)24 H₂O(l)+ 6 Mn²⁺(aq)+ 5 XeO₃(aq)+ 30 H⁺(aq) 6 MnO₄^-(aq)+ 5 Xe(g)+ 15 H₂O + 48 H⁺(aq)

E)9 H₂O(l)+ 6 Mn²⁺(aq)+ 5 XeO₃(aq) 6 MnO₄^-(aq)+ 5 Xe(g)+ 18 H⁺(aq)

Q2) Hydrogen compounds are called hybrids.

A)True

B)False

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Chapter 23: The Transition Elements

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Q1) MnO₄^-(aq)produces what manganese-containing species when used as an oxidizing agent in weakly basic solution?

A)MnO₄^2-

B)Mn

C)Mn²⁺

D)Mn₂O₃

E)MnO₂

Q2) How many d electrons are there in CrO₇^2-?

A)0

B)1

C)2

D)3

Q3) Choose the INCORRECT statement.

A)Most representative element bonding involves s and p orbitals.

B)Most transition element bonding involves p orbitals.

C)Most representative elements are single oxidation states.

D)Most transition elements are multiple oxidation states.

E)Metallurgy is the study of metals.

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Chapter 24: Complex Ions and Coordination Compounds

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Q1) Choose the INCORRECT statement.

A)One popular chelating agent is EDTA.

B)[Cr(NH₃)₄Br]Cl and [Cr(NH₃)₄Cl]Br are examples of ionization isomerism.

C)Linkage isomers differ in the spatial arrangements among the ligands.

D)A tetrahedral complex cannot have a geometric isomer.

E)Enantiomers are optical isomers.

Q2) Coordination isomerism could be shown by:

A)Li[AlH₄]

B)[Ag(NH₃)₂][CuCl₂]

C)[Co(NH₃)₄Cl₂]Br

D)[Pt(H₂O)₄Cl₂]

E)[Fe(CN)₆](NH₃)₃

Q3) Give the correct name for [Fe(CO)₄].

A)tetracarbonyliron(0)

B)iron carbon monoxide

C)carbonylferrate(IV)

D)tetracarbonylferrate(0)

E)iron carbonyl

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Page 26

Chapter 25: Nuclear Chemistry

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Sample Questions

Q1) Half-life is:

I.the time for a sample to decay completely.

II.constant for a given radioisotope.

III.the time required for half of a sample to decay.

IV.inversely proportional to the decay constant.

A)I and II

B)I,II,and III

C)I and III

D)I,III,and IV

E)II,III,and IV

Q2) What total energy is released when 0.75 grams of ²³⁵U undergo fission if each atom averages 3.2 × 10^-11 J of energy released?

A)1.45 × 10¹³ J

B)6.01 × 10³¹ J

C)6.15 × 10¹⁰ J

D)6.15 × 10⁷ J

E)1.45 × 10¹⁰ J

Q3) Fission is the process of combining small nuclei into larger nuclei.

A)True

B)False

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Chapter 26: Structures of Organic Compounds

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Sample Questions

Q1) Give the name for CH₃CH =CHCH₃.

A)3-butene

B)2-butene

C)2-propene

D)2-pentene

E)2-butane

Q2) In alkene nomenclature "trans" stands for "on the same side" while "cis" means "across."

A)True

B)False

Q3) Which compound is a saturated hydrocarbon?

A)1-butyne

B)cycloheptene

C)3-methylheptane

D)2-heptyne

Q4) In the rings of heterocyclic compounds we can find one or more atoms that are not carbon atoms.

A)True

B)False

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Chapter 27: Reactions of Organic Compounds

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Q1) Suggest possible compounds for A and B in the following scheme: CH₃CH₂I + A CH₃CH₂SH + B

A)A is HS^- and B is I^-

B)A is H₂S and B is I₂

C)A is H₂S and B is HI

D)A is S^2- and B is I^-

E)A is H₂S and B is I^-

Q2) What is a dehydration reaction?

A)Dehydration is the elimination of water molecule from an alcohol molecule to produce alkene.

B)A dehydration reaction is the removal of one equivalent of H₂ from an alkane to produce alkene.

C)A dehydration reaction is one of the steps in chain-reaction polymerization.

D)A dehydration reaction is the removal of crystalline water.

E)A dehydration reaction is the deprotonation of a substrate with a strong base in E2 mechanism.

Q3) Electrophilic substitution reactions are typical reactions of aromatic compounds.

A)True

B)False

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Chapter 28: Chemistry of the Living State

Available Study Resources on Quizplus for this Chatper

104 Verified Questions

104 Flashcards

Source URL: https://quizplus.com/quiz/64257

Sample Questions

Q1) Choose the INCORRECT statement.

A)Peptides are amino acids joined by a peptide bond.

B)A tripeptide has three peptide bonds.

C)A protein is hydrolyzed to a mixture of -amino acids.

D)An -amino acid is a carboxylic acid with an amine group on the carbon atom.

E)Proteins are a polymer of amino acid units.

Q2) Which of the following compounds may display the property of optical isomerism?

A)3-pentanol

B)2-pentene

C)2-bromopropane

D)2-bromobutane

E)acetone

Q3) Compounds which are optical isomers of one another but differ in physical and chemical properties are known as what?

A)geometric isomers

B)enantiomers

C)racemic compounds

D)allotropes

E)diastereomers

Q4) The hydrolysis of tristearin produces the soap potassium stearate and ________.

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