Chemistry for Life Sciences Mock Exam - 2556 Verified Questions

Chemistry for Life Sciences

Mock Exam

Course Introduction

Chemistry for Life Sciences introduces the foundational principles of chemistry with an emphasis on their application to biological systems. The course covers key topics such as atomic structure, chemical bonding, thermodynamics, reaction kinetics, acids and bases, and the properties of solutions, all within a biological context. Students will explore the chemical behavior of biomolecules including carbohydrates, proteins, lipids, and nucleic acids, and learn how chemical processes underpin vital functions in living organisms. Through lectures, laboratory experiments, and problem-solving exercises, students will gain the essential chemical knowledge required to understand and pursue further studies in life sciences and related fields.

Recommended Textbook

General Chemistry The Essential Concepts 7th Edition by Raymond Chang

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Chapter 1: Introduction

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Sample Questions

Q1) Iridium is essentially tied with osmium for the distinction of being called the "densest element" with a density of 22.5 g/cm³. What would be the mass in pounds of a 1.0 ft * 1.0 ft * 1.0 ft cube of iridium? (1 lb = 453.6 g)

A)1.5 lb

B)5.2 lb

C)6.20 lb

D)1.4 * 10³ lb

E)6.4 * 10⁵ lb

Answer: D

Q2) You just measured a sugar cube and obtained the following information: mass = 3.48 g height = length = width = 1.3 cm

Determine the volume and density of the cube. Suppose the sugar cube was added to a cup of water. Before it dissolves, will the sugar cube float or sink to the bottom? Answer: Volume of the sugar cube = 2.2 cm³; density of the sugar cube = 1.6 g/cm³. Before dissolving, the sugar cube will sink in a cup of water.

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Chapter 2: Atoms, Molecules, and Ions

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Sample Questions

Q1) The formula for sodium sulfide is A)NaS.

B)K₂S.

C)NaS₂.

D)Na₂S.

E)SeS.

Answer: D

Q2) How many atoms are in one molecule of CaCl₂?

Answer: 3

Q3) Which of the following elements is most likely to be a good conductor of electricity? A)N

B)S

C)He

D)Cl

E)Fe

Answer: E

Q4) Name the following binary compound: NaH. Answer: sodium hydride

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Chapter 3: Stoichiometry

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Sample Questions

Q1) Phosgene, a poisonous gas used during WWI, is composed of 12.1% C, 16.2% O, and 71.1% Cl. What is the empirical formula of phosgene?

Answer: COCl₂

Q2) Calculate the mass of 4.50 moles of chlorine gas, Cl₂.

A)6.34 * 10^-2 g

B)4.5 g

C)15.7 g

D)160 g

E)319 g

Answer: E

Q3) When a 0.952 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 1.35 g of CO₂ and 0.826 g of H₂O are produced. What is the empirical formula of the compound?

Answer: CH₃O

Q4) If 0.66 mole of a substance has a mass of 99 g, what is the molecular mass of the substance?

Answer: 150 g

Q5) How many ICl₃ molecules are present in 1.75 kg of ICl₃?

Answer: 4.52 * 10²⁴

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Chapter 4: Reactions in Aqueous Solution

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Sample Questions

Q1) What is the chemical formula of the salt produced by the neutralization of hydrobromic acid with magnesium hydroxide?

A)MgBr

B)Mg₂Br₃

C)Mg₃Br₂

D)Mg₂Br

E)MgBr₂

Q2) Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: CH₃OH (methanol).

Q3) Which of the following compounds is a nonelectrolyte?

A)NaF

B)HNO₃

C)CH₃COOH (acetic acid)

D)NaOH

E)C₆H₁₂O₆(glucose)

Q4) Determine the oxidation number of each of the elements in K₂TaF₇?

Q5) Determine the oxidation number of each of the elements in Cs₂Cr₂O₇?

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Chapter 5: Gases

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Sample Questions

Q1) In a weather forecast on a Seattle radio station the barometric pressure was reported to be 29.4 inches. What is this pressure in SI units? (1 inch = 25.4 mm, 1 atm = 760 mmHg)

Q2) Samples of the following volatile liquids are opened simultaneously at one end of a room. If you are standing at the opposite end of this room, which species would you smell first? (Assume that your nose is equally sensitive to all these species.)

A)ethyl acetate (CH₃COOC₂H₅)

B)camphor (C₁₀H₁₆O)

C)diethyl ether (C₂H₅OC₂H₅)

D)naphthalene (C₁₀H₈)

E)pentanethiol (C₅H₁₁SH)

Q3) A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at -4.0°C. Which of these choices is its molecular formula?

A)NO

B)NO₂

C)N₃O₆

D)N₂O₄

E)N₂O₅

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Chapter 6: Energy Relationships in Chemical Reactions

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Sample Questions

Q1) The heat of solution of ammonium chloride is 15.2 kJ/mol. If a 6.134 g sample of NH₄Cl is added to 65.0 mL of water in a calorimeter at 24.5°C, what is the minimum temperature reached by the solution? (The specific heat of water = 4.18 J/g·°C; the heat capacity of the calorimeter = 365. J/°C.)

A)27.1°C

B)18.6°C

C)19.7°C

D)21.9°C

E)30.4°C

Q2) A feverish student weighing 75 kilograms was immersed in 400. kg of water at 4.0°C to try to reduce the fever. The student's body temperature dropped from 40.0°C to 37.0°C. Assuming the specific heat of the student to be 3.77 J/g·°C, what was the final temperature of the water?

Q3) What is the standard enthalpy of formation of H₂(g)at 25°C?

Q4) Thermal energy is

A)the energy stored within the structural units of chemical substances.

B)the energy associated with the random motion of atoms and molecules.

C)solar energy, i.e. energy that comes from the sun.

D)energy available by virtue of an object's position.

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Chapter 7: The Electronic Structure of Atoms

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Sample Questions

Q1) What is the energy in joules of a mole of photons associated with red light of wavelength 7.00 * 10² nm?

A)256 kJ

B)1.71 * 10⁵ J

C)4.72 * 10^-43 J

D)12.4 kJ

E)2.12 * 10⁴² J

Q2) A ground-state atom of manganese has ___ unpaired electrons and is _____.

A)0, diamagnetic

B)2, diamagnetic

C)3, paramagnetic

D)5, paramagnetic

E)7, paramagnetic

Q3) Which of the following is the electron configuration of an excited state of an oxygen atom?

A)1s²2s²2p⁴

B)1s²2s²2p⁵

C)1s²2s²2p³3s¹

D)1s²2s²2p⁶

E)1s²2s²2p³

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Chapter 8: The Periodic Table

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Sample Questions

Q1) Consider the following reaction 2A + 3F₂\(\rarr\)2AF₃.

What is a reasonable guess for the identity element A?

Q2) Why do the group 5A elements have relatively small electron affinities compared to the neighboring nonmetals in the corresponding rows?

Q3) The sulfide ion, S^2-, is isoelectronic with which one of the following?

A)O^2-

B)F^-

C)Na⁺

D)Al³⁺

E)K⁺

Q4) Which one of the following does not have [Xe] as its electronic configuration?

A)Te^2-

B)I^-

C)Cs⁺

D)Ba²⁺

E)Sn⁴⁺

Q5) Write the ground-state electron configuration for Ca²⁺.

Q6) Write the ground-state electron configuration for Mg²⁺.

Q7) Write the ground-state electron configuration for Br^-.

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Chapter 9: Chemical Bonding I: the Covalent Bond

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Sample Questions

Q1) What is the formal charge on phosphorus in a Lewis structure for the phosphate ion that satisfies the octet rule?

A)-2

B)-1

C)0

D)+1

E)+2

Q2) Which one of these polar covalent bonds would have the greatest percent ionic character?

A)H - Br

B)H - Cl

C)H - F

D)H - I

Q3) Classify the Ca - Cl bond in CaCl₂ as ionic, polar covalent, or nonpolar covalent.

A)ionic

B)polar covalent

C)nonpolar covalent

Q4) Write the Lewis dot symbol for the chloride ion.

Q5) Write a Lewis structure for OF₂.

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Chapter 10: Chemical Bonding Ii: Molecular Geometry and Hybridization

of Atomic

Orbitals

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Sample Questions

Q1) According to VSEPR theory, which one of the following molecules should have a geometry that is trigonal bipyramidal?

A)SF₄

B)XeF₄

C)NF₃

D)SF₆

E)PF₅

Q2) A homonuclear diatomic molecule is a molecule composed of three atoms of the same element.

A)True

B)False

Q3) Which should have the longer bond, B₂ or B₂?

Q4) Which of the following correctly lists species in order of increasing bond order?

A)C₂ < Li₂ < Be₂ < N₂

B)Be₂ < Li₂ < C₂ < N₂

C)N₂ < Be₂ < Li₂ < C₂

D)N₂ < C₂ < Li₂ < Be₂

E)Be₂ < C₂ < N₂ < Li₂

Q5) Indicate the number of \(\pi\)-bonds in C₂H₆.

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Chapter 11: Introduction to Organic Chemistry

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Sample Questions

Q1) The alkane with six carbon atoms is called

A)butane.

B)hexane.

C)heptane.

D)butene.

E)none of these.

Q2) Oxidation of the 2-propanol will produce a/an

A)aldehyde.

B)amine.

C)alkene.

D)ketone.

E)carboxylic acid.

Q3) Which of these statements describes a condensation reaction?

A)addition of H₂O to a double bond

B)linking an acid and an alcohol to make an ester and water

C)addition of H₂ to an alkene

D)oxidation of ethanol to acetaldehyde

E)hydrolysis of an ester

Q4) A compound with the formula C₆H₁₂ may or may not be a saturated hydrocarbon. Explain.

Page 13

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Chapter 12: Intermolecular Forces and Liquids and Solids

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Sample Questions

Q1) Of the pair of compounds given, which would have the stronger intermolecular forces of attraction?

NH₃ or PH₃

Q2) Each of the following substances is a gas at 25°C and 1 atmosphere pressure. Which one will liquefy most easily when compressed at a constant temperature?

A)F₂

B)H₂

C)HF

D)SiH₄

E)Ar

Q3) The meniscus for water is curved upward at the edges (i.e., it is "concave up"). Explain this phenomenon in terms of cohesion and adhesion.

Q4) Indicate all the types of intermolecular forces of attraction in SF₆(g).

Q5) Indicate all the types of intermolecular forces of attraction in SF₄(g).

Q6) Boron nitride, BN₃, melts at approximately at 3,000°C under high pressure. This material is almost as hard as diamond. What kind of crystal is this?

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Chapter 13: Physical Properties of Solutions

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Sample Questions

Q1) Pure benzene, C₆H₆, freezes at 5.5° and boils at 80.1°C. What is the boiling point of a solution consisting of cyclohexane (C₆H₁₂)dissolved in benzene if the freezing point of this solution is 0.0°C? (For benzene, K_f = 5.12 °C/m, K_b = 2.53 °C/m; for cyclohexane, K_f = 20.0 °C/m, K_b = 2.79°C/m)

A)82.8°C

B)91.2°C

C)80.9°C

D)77.4°C

E)83.1°C

Q2) Calculate the molality of 6.0 M H₂SO₄ solution. The density of the solution is 1.34 g/mL.

A)4.48 m

B)7.98 m

C)8.10 m

D)8.43 m

E)10.2 m

Q3) Define solvation.

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Page 15

Chapter 14: Chemical Kinetics

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Q1) Benzoyl chloride, C₆H₅COCl, reacts with water to form benzoic acid, C₆H₅COOH, and hydrochloric acid. This first-order reaction is 25% complete after 26 s. How much longer would one have to wait in order to obtain 99% conversion of benzoyl chloride to benzoic acid?

A)393 s

B)419 s

C)183 s

D)293 s

E)209 s

Q2) The reaction A + 2B \(\rarr\) products was found to follow the rate law: rate = k[A]²[B]. Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

A)5

B)6

C)12

D)18

E)None of these.

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Page 16

Chapter 15: Chemical Equilibrium

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Q1) Equilibrium is established for the reaction 2X(s)+ Y(g)\(\rarr\)2Z(g)at 500K, K_c = 100. Determine the concentration of Z in equilibrium with 0.2 mol X and 0.50 M Y at 500K.

A)3.2 M

B)3.5 M

C)4.5 M

D)7.1 M

E)None of these.

Q2) The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10^-18. Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?

Q3) What conditions are used in the Haber process to enhance the yield of ammonia? Explain why each condition affects the yield in terms of the Le Châtelier principle.

Q4) Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.

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Chapter 16: Acids and Bases

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Q1) A solution with a pH of 8 has a hydrogen ion concentration [H⁺] that is 30 times greater than that of a solution of pH 11.

A)True

B)False

Q2) Predict the direction in which the equilibrium will lie for the reaction H₂CO₃ + F\(\rarr\)HCO₃^- + HF. K_a1(H₂CO₃)= 4.2 * 10^-7; K_a(HF)= 7.1 * 10^-4

A)to the right

B)to the left

C)in the middle

Q3) The pH of a Ba(OH)₂ solution is 10.00. What is the H⁺ ion concentration of this solution?

A)4.0 * 10^-11 M

B)1.6 * 10^-10 M

C)1.3 * 10^-5 M

D)1.0 * 10^-10 M

E)10. M

Q4) Calculate the pOH of a solution containing 0.25 g of HCl in 800. mL of solution.

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Chapter 17: Acid-Base Equilibria and Solubility Equilibria

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Q1) The K_sp of CaF₂ is 4 * 10^-11. What is the maximum concentration of Ca²⁺ possible in a 0.10 M NaF solution?

Q2) What volume of 0.200 M potassium hydroxide should be added to 300. mL of 0.150 M propanoic acid (C₂H₅COOH)to obtain a solution with a pH of 5.25? [K_a(C₂H₅COOH)= 1.34 * 10^-5]

A)32 mL

B)210 mL

C)160 mL

D)65 mL

E)13 mL

Q3) Write an equation showing the net reaction that occurs when a strong acid is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 * 10^-7, K_a2 = 2.4 * 10^-8):

Q4) An environmental chemist obtained a 200. mL sample of lake water believed to be contaminated with a single monoprotic strong acid. Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint. What is the concentration of H⁺ in the lake?

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Chapter 18: Thermodynamics

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Q1) In the gas phase, methyl isocyanate (CH₃NC)isomerizes to acetonitrile (CH₃CN), H₃C-N\(\equiv\)C (g) \(\rarr\) H₃C-C \(\equiv\) N (g)

With \(\Delta\)H° = -89.5 kJ/mol and \(\Delta\)G° = -73.8 kJ/mol at 25°C. Find the equilibrium constant for this reaction at 100°C.

A)1.68 * 10^-10

B)5.96 * 10⁹

C)2.16 * 10¹⁰

D)4.63 * 10^-11

E)8.64 * 10¹²

Q2) For a certain reaction, \(\Delta\)G° = 87 kJ/mol, \(\Delta\)H° = 100 kJ/mol at STP. At what temperature, in K, is the reaction in equilibrium, assuming that \(\Delta\)S° and \(\Delta\)H° are temperature-independent?

Q3) Dissolving an ionic solid in water always results in an increase in entropy.

A)True

B)False

Q4) Choose the substance with the higher entropy per mole at a given temperature: 1 mole of N₂(g)in a 22.4 L container or 1 mole of N₂(g)in a 2.24 L container.

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Chapter 19: Redox Reactions and Electrochemistry

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Q1) How long will it take to produce 78 g of Al metal by the reduction of Al³⁺ in an electrolytic cell with a current of 2.0 A?

A)0.01 s

B)420 s

C)13 h

D)116 h

E)1.0 * 10¹² s

Q2) Consider an electrochemical cell based on the following cell diagram: Pt | Pu³⁺(aq), Pu⁴⁺(aq)|| Cl₂(g), Cl^-(aq)|

Pt

Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu⁴⁺/Pu³⁺)?

A)2.37 V

B)1.01 V

C)-1.71 V

D)-1.01 V

E)1.71 V

Q3) Will H₂(g)form when Cu is placed in 1.0 M HCl?

Q4) Will H₂(g)form when Ag is placed in 1.0 M HCl?

Page 21

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Chapter 20: The Chemistry of Coordination Compounds

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Q1) In the following pair of complex ions, choose the one that absorbs light at a longer wavelength.

A)[Co(H₂O)₆]²⁺

B)[Co(NH₃)₆]²⁺

Q2) The oxidation number of Co in [Co(NH₃)₄Cl₂]Cl is +1.

A)True

B)False

Q3) Which of these complex ions would absorb light with the longest wavelength?

A)[Co(H₂O)₆]²⁺

B)[Co(NH₃)₆]²⁺

C)[CoF₆]^4-

D)[Co(CN)₆]^4-

E)[Co(en)₆]²⁺

Q4) In the following pair of complex ions, choose the one that absorbs light at a shorter wavelength.

A)[Co(NH)₆]³⁺

B)[CoCl₆]^3-

Q5) Name the complex ion [Ni(CN)₄]^2-.

Q6) What is the coordination number of silver in [Ag(NH₃)₂]Cl?

Page 22

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Chapter 21: Nuclear Chemistry

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Q1) The radioisotope potassium-40 decays to argon-40 by positron emission with a half-life of 1.3 * 10⁹ yr. A sample of moon rock was found to contain 78 argon-40 atoms for every 22 potassium-40 atoms. The age of the rock is

A)8.1* 10^-10 yr.

B)2.4 * 10⁹ yr.

C)2.8 * 10⁹ yr.

D)4.6 * 10⁹ yr.

E)6.8 * 10⁹ yr.

Q2) Charcoal found under a stone at Stonehenge, England, has a carbon-14 activity that is 0.60 that of new wood. How old is the charcoal? (The half-life of carbon-14 is 5,730 years.)

A)Less than 5,730 yr

B)Between 5,730 and 11,460 yr

C)Between 11,460 and 17,190 yr

D)More than 17,190 yr

Q3) Which type of radiation is the least penetrating?

A)alpha

B)beta

C)gamma

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Page 23

Chapter 22: Organic Polymerssynthetic and Natural

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Q1) The primary structure of a protein refers to the unique amino acid sequence of the polypeptide chain.

A)True

B)False

Q2) The intermolecular force between bases on the opposite strands of DNA responsible for its double-helical structure is

A)hydrogen bonding.

B)dispersion force.

C)covalent bonding.

D)ionic force.

E)dipole-dipole force.

Q3) Which one of these materials is a copolymer?

A)Styrene-butadiene

B)polyvinyl chloride

C)polypropylene

D)poly-cis-isoprene

E)polyethylene

Q4) Both DNA and RNA have double-helical structures.

A)True

B)False

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