Physical Chemistry I Midterm Exam - 1986 Verified Questions

Course Introduction

Physical Chemistry I Midterm Exam

Physical Chemistry I introduces the fundamental principles that govern the physical and chemical behavior of matter. Topics include the laws of thermodynamics, properties of gases, phase equilibria, chemical equilibria, solutions, and the molecular basis of heat, work, and energy transformations. Through a combination of mathematical models and conceptual understanding, students will explore how molecular structure and interactions influence macroscopic chemical phenomena. This course lays the groundwork for advanced studies in chemistry and related scientific fields by developing analytical problem-solving skills and a deep comprehension of physical and chemical processes.

Recommended Textbook

Chemical Principles 6th Edition by Professor Peter Atkins

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Page 2

Chapter 1: The Quantum World

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Q1) What is the energy of a mole of photons with a frequency of 3.8 * 10¹⁴ /sec?

A)1.5 * 10⁵J/mol

B)1.5 * 10^-5J/mol

C)6.7 * 10^-⁷J/mol

D)6.7 * 10⁷J/mol

E)3.8 * 10^-5J/mol

Answer: A

Q2) Radiation with a frequency of 3.9*10¹⁴/sec has what wavelength?

A)1.3 *10⁶ m

B)7.7*10^-7 cm

C)7.7*10^-7 m

D)3.1*10⁶ m

E)1.3*10⁶ cm

Answer: C

Q3) Visible light,microwaves,and x-rays travel through empty space at 3.00 * 10⁸ m^-¹.

A)True

B)False

Answer: True

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Chapter 2: Quantum Mechanics in Action: Atoms

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Q1) For F^-,write the ground-state electron configuration.

A)[Ne]2p⁵

B)[Ne]

C)[Ar]

D)[He]2p⁵

E)[He]1s²

Answer: B

Q2) Which atom has the highest first ionization energy?

A)Pb

B)Sn

C)Ge

D)Si

Answer: D

Q3) Which of the following has the largest effective nuclear charge?

A)F

B)Na

C)Li

D)He

E)N Answer: A

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Chapter 3: Chemical Bonds

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Q1) How many resonance structures can be drawn for N₂O?

A)0

B)3

C)2

D)1

Answer: B

Q2) Which of the following compounds contains the strongest bonds to hydrogen?

A)SiH₄

B)CH₄

C)HF

D)H₂S

E)H₂O

Answer: C

Q3) Because of the octet rule,the gaseous O²^- ion is stable.

A)True

B)False

Answer: False

Q4) How many valence electrons are present in W⁴⁺?

Answer: 2

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Chapter 4: Molecular Shape and Structure

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Q1) The molecules OF₂ and O₃ both have bent shapes.What are the approximate bond angles in OF₂ and O₃,respectively?

A)109^o and 120^o

B)Both 109^o

C)Both 120^o

D)Both 180^o

E)109^o and 180^o

Q2) What is the shape of SO₃²^-?

A)T-shaped

B)Trigonal pyramidal

C)Seesaw

D)Tetrahedral

E)Trigonal planar

Q3) Draw the Lewis structure of the cyanamide ion,NCNH^-,and give the number of lone pairs of electrons and the number of \(\sigma\)- and \(\pi\)-bonds.

Q4) The OSO bond angle in the sulfite ion is ___________________ (greater than/equal to/ less than)109.5S1U1P1\(\circ\)S1S1P0.

Q5) Name all the angles in a trigonal bipyramidal geometry.

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Chapter 5: The Properties of Gases

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Q1) A sample of gas with a volume of 750 mL exerts a pressure of 98.0 kPa at 30S1U1P1\(\circ\)S1S1P0C.What pressure will the sample exert when it is compressed to 250 mL and cooled to -25S1U1P1\(\circ\)S1S1P0C?

A)353 kPa

B)241 kPa

C)359 kPa

D)39.9 kPa

E)26.7 kPa

Q2) The value of the gas law constant,R,in units of L.kPa.mol^-¹.K^-¹ is

A)62.4

B)0.0821

C)0.0752

D)7.62

E)8.31

Q3) A sample of nitrogen gas collected at 24S1U1P1\(\circ\)S1S1P0C and 745 Torr has a vapor pressure of 745 Torr.True or false?

A)True

B)False

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Page 7

Chapter 6: Liquids and Solids

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Q1) If the interaction between two species is proportional to 1/r²,which of the following is likely involved?

A)Chloromethane molecules in the liquid phase

B)Na⁺ and H₂O

C)Bromine molecules in the liquid phase

D)Chloromethane molecules in the gas phase

E)Ions in an ionic solid

Q2) How many tetrahedral holes are there in a face-centered cubic unit cell?

A)8

B)12

C)1

D)4

E)6

Q3) Which of the following molecular solids has the highest melting point?

A)Sucrose,C₁₂H₂₂O₁₁

B)Carbon dioxide,CO₂

C)H₂O

D)TiCl₄

E)Benzene,C₆H₆

Q4) Which has the higher boiling point,HCl or HI?

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Chapter 7: Inorganic Materials

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Q1) What element besides iron and carbon is necessary to produced stainless steel?

A)Chromium.

B)Vanadium.

C)Phosphorus.

D)Sulfur.

E)Zinc.

Q2) What term is used for the emission of light from molecules excited by radiation of higher frequency?

A)Phosphorescence

B)Fluorescence

C)Both A and B,above.

D)None of the above.

Q3) Malleability refers to a metal's ability to be hammered into a specific shape.

A)True

B)False

Q4) When a magnet is brought near a ferrofluid,the particles in the fluid try to align themselves with the magnetic field.

A)True

B)False

Q5) What contaminant causes the red "terra cotta" color in most ceramics?

Page 9

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Chapter 8: Thermodynamics: The First Law

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Q1) The standard enthalpy of formation of ammonia gas is -46.11 kJ.mol^-1 at 298 K.What is the standard reaction enthalpy for the Haber process at 500S1U1P1\(\circ\)S1S1P0C? The molar heat capacities of nitrogen,hydrogen,and ammonia are 29.12,28.82,and 35.06 kJ.mol^-1respectively.

A)(-97.65 kJ.mol^-1)

B)(-113.81 kJ.mol^-1)

C)(-56.91 kJ.mol^-1)

D)(-92.22 kJ.mol^-1)

E)(-103.09 kJ.mol^-1)

Q2) Combustion reactions can be exothermic or endothermic.

A)True

B)False

Q3) for the reaction

N₂O₅(s)\(\rightarrow\) 2NO₂(g)+ ½O₂(g),\(\Delta\)H_r = 109.5 kJ.mol^-1 at 298 K at constant temperature and pressure,\(\Delta\)H > \(\Delta\)U.

A)True

B)False

Q4) Work is reported in joules; and 1 joule = ____________

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Chapter 9: Thermodynamics: The Second and Third Laws

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Q1) Consider the reaction Cl₂(g)\(\rightarrow\) 2Cl(g)

Which of the following statement regarding this reaction is true?

A)The reaction is spontaneous at high temperatures.

B)The reaction is spontaneous at low temperatures.

C)The reaction is not spontaneous at any temperature.

D)The reaction is spontaneous at all temperatures.

Q2) Use Trouton's constant to estimate the enthalpy of condensation of diethyl ether,which boils at 309 K.

A)(-26 kJ.mol^-1)

B)+26 kJ.mol^-1

C)(-275 kJ.mol^-1)

D)(-85 kJ.mol^-1)

E)+85 kJ.mol^-1

Q3) Which of the following has the lowest standard molar entropy?

A)C(graphite)

B)P₄(s)

C)S₈(s)

D)C₆₀(s)

E)C(diamond)

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Page 11

Chapter 10: Physical Equilibria

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Q1) Which of the following 1.0 M solutions contains the most particles?

A)Ethylene glycol

B)Potassium chloride

C)Magnesium sulfate

D)Glucose

E)Sodium sulfate

Q2) The condition called the bends results from the rapid release of nitrogen gas in the bloodstream when the diver returns to the surface.Would argon gas or hydrogen gas be suitable replacements for nitrogen gas in "compressed air?" Explain.

Q3) The vapor pressure of methanol at 25S1U1P1\(\circ\)S1S1P0C is 123 Torr and its enthalpy of vaporization is 35.3 kJ.mol^-1.Estimate the normal boiling point of methanol.Assume the enthalpy of vaporization is independent of temperature.

A)450 K

B)342 K

C)315 K

D)373 K

E)Not enough information given.

Q4) What is the vapor pressure of carbon disulfide at its normal boiling point?

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Page 12

Chapter 11: Chemical Equilibria

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Q1) Consider the reaction 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g),K = 10⁸⁰ at a certain temperature.

Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

A)6 M.

B)0 M.

C)3 M.

D)12 M.

E)18 M.

Q2) Calculate the vapor pressure of ethyl alcohol,C₂H₅OH(l),at 298 K.The standard free energies of formation of C₂H₅OH(l)and C₂H₅OH(g)are -174.8 and -168.6 kJ.mol^-1,respectively.

A)0.082 atm

B)0.92 atm

C)0.0032 atm

D)1.0 atm

E)Not enough information given to permit the calculation.

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Page 13

Chapter 12: Acids and Bases

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Q1) Estimate the pH of 0.10 M Na₂HPO₄(aq)given pK_a1 = 2.12,pK_a2 = 7.21,and pK_a3 = 12.68 for phosphoric acid.

A)12.68

B)9.94

C)7.40

D)4.67

E)2.12

Q2) All of the following are strong bases in water except

A)NaHCO₃

B)CaO

C)Na₂O

D)Na₂SO₄

Q3) Bond polarity tends to dominate the trend of acid strengths for binary acids of elements of the same period.

A)True

B)False

Q4) What is the conjugate acid of O^2-?

Q5) Write the autoprotolysis reaction for liquid ammonia.

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Chapter 13: Aqueous Equilibria

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Q1) What is the main factor that directly determines the pH of any buffer?

Q2) You have available the following reagents as 0.10 M aqueous solutions: NaOH,HCl,HCN (pK_a = 9.31),aniline (pK_b = 9.13),HNO₂ (pK_a = 3.25),and CH₃NH₂ (pK_b = 3.34).Which two reagents would you use to make a buffer with a pH of 10.6?

A)NaOH and HCN

B)HCl and aniline

C)HCl and CH₃NH₂

D)NaOH and HNO₂

Q3) When pyridinium chloride is added to C₅H₅N(aq),

A)the pH of the solution does not change.

B)the pH of the solution increases.

C)the pH of the solution decreases.

D)the K_b increases.

E)the equilibrium concentration of NH₃(aq)decreases.

Q4) In the titration of 0.300 M H₃PO₄(aq)with 0.300 M NaOH(aq),the first stoichiometric point occurs at pH < 7 whereas in the titration of 0.300 M HCOOH(aq)with 0.300 M NaOH(aq)the stoichiometric point occurs at pH > 7.Explain.

Q5) What is the main factor that determines the pH of any buffer?

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Chapter 14: Electrochemistry

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Q1) The galvanic cell shown above uses the half-cells Pb²⁺/Pb and Zn²⁺/Zn,and a salt bridge containing KCl(aq).The voltmeter gives a positive voltage reading.The electrode B could be inert platinum metal or zinc.

A)True

B)False

Q2) If 8686 C of charge is passed through molten magnesium chloride,calculate the number of moles of Mg(l)produced.

A)0.0225 mol

B)0.0450 mol

C)2.00 mol

D)0.0110 mol

E)0.0900 mol

Q3) In the cell shown above,A is a standard Ag⁺/Ag electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is +0.80 V,which electrode is negative?

Q4) When KI(aq)is electrolyzed at a concentration of 1 M,the product at the anode is I₂.

A)True

B)False

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Chapter 15: Chemical Kinetics

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Q1) The reaction between nitrogen dioxide and carbon monoxide is thought to occur by the mechanism 2NO₂(g)\(\rightarrow\) NO₃(g)+ NO(g) K₁,slow NO₃(g)+ CO(g)\(\rightarrow\)NO₂(g)+ CO₂(g) K₂,fast

The rate law for this mechanism is

A)rate = k₁k₂[NO₂]²[CO].

B)rate = (k₁/k₂)[NO₂]²[CO].

C)rate = k₁[NO₃][NO].

D)rate = k₂[NO₃][CO].

E)rate = k₁[NO₂]².

Q2) For a second-order reaction,a straight line is obtained from a plot of

A)1/[A] vs t.

B)ln(1/t)vs [A].

C)[A] vs t.

D)ln[A] vs t.

E)ln(t)vs [A].

Q3) What is the half-life of a second order reaction?

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Chapter 16: The Elements: the Main Group Elements

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Q1) Sulfur dioxide can act as both an oxidizing agent and a reducing agent; explain.

Q2) Lead is obtained from the oxide PbO by

A)reduction with aluminum.

B)treatment with concentrated sulfuric acid.

C)reduction with carbon.

D)reduction with CO(g).

E)heating to 1600S1U1P1\(\circ\)S1S1P0C.

Q3) What reaction produces diborane?

A)BH₃(g)and B(s).

B)BF₃(g)and NaBH₄(s).

C)B(s)and H₂(g).

D)B(s)and NH₃(g).

E)BCl₃(g)and NaH(s).

Q4) The compound BeI₂ is an ionic compound.

A)True

B)False

Q5) Which Group 13 element is most likely to have an oxidation number of +1 in its compounds?

Q6) Write the formula of the hydride ion.

Q7) Write an equation for the first ionization energy of sodium.

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Chapter 17: The Elements: The D Block

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Q1) Complexes with coordination number 4 are either tetrahedral or octahedral.

A)True

B)False

Q2) Consider the complexes fac- and mer-triaquatrichlororuthenium(III)chloride.Neither of these complexes is chiral.

A)True

B)False

Q3) The atomic radii of the Period 6 d-metals are

A)smaller than expected,and about the same as the Period 5 d-metals.

B)about the same as the lanthanides.

C)larger than the atomic radii of the Period 5 d-metals.

D)about the same as the Period 4 d-metals.

E)large because of the lanthanide contraction.

Q4) Which of the following complex ions is likely to absorb at 600-700 nm?

A)[Co(OH₂)₆]²⁺

B)[Co(NO₂)₆]^4-

C)[Co(NH₃)₆]²⁺

D)[Co(CN)₆]^4-

E)[CoCl₄]^2-

Q5) What do all rhodium complexes have in common?

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Chapter 18: Nuclear Chemistry

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Q1) Calculate the energy change when one ²³⁵U nucleus undergoes the fission reaction ²³⁵U + n \(\rightarrow\) ¹⁴²Ba + ⁹²Kr + 2n

The masses needed are ²³⁵U,235.04 u; ¹⁴²Ba,141.92 u; ⁹²Kr,91.92 u; n,1.0087 u.

A)-3.2 * 10^-28 J

B)+1.8 * 10^-10 J

C)-1.7 * 10^-10 J

D)+2.9 * 10^-11 J

E)-2.8 * 10^-11 J

Q2) A 9.9-g sample of iodine-131 is stored for exactly 3 weeks.If the decay constant is 0.0861 day^-1,what mass of the isotope remains?

A)0.15 g

B)7.6 g

C)1.6 g

D)2.6 g

E)5.5 g

Q3) Complete the nuclear reaction ⁹⁷Mo + ²H \(\rightarrow\) _____ + 2n

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Page 20

Chapter 19: Organic Chemistry I

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Q1) Which of the following pairs react?

A)CH₄(g)and KMnO₄(aq)

B)CH₄(g)and NaOH(aq)

C)CH₄(g)and Cl₂(g)

D)CH₄(g)and HNO₃(l)

E)CH₄(g)and H₂SO₄(l)

Q2) Name the compound

CH₃CH(CH₃)CH(CH₂CH₃)C(CH₃)₃.

A)2,4,4-trimethyl-3-ethylpentane

B)2,2,4-trimethyl-3-ethylpentane

C)Decane

D)1,2-tetramethylpentane

E)2,2-dimethyl-3-ethyl-4-methylpentane

Q3) When 2-methyl-1-butene reacts with HBr,the reaction occurs in two steps.Draw the structure of the intermediate.(Hint: Intermediate carbocations are most stable when formed at tertiary carbons.)

Q4) Why do alkanes not react with boiling nitric acid?

Q5) When 2-methyl-1-butene reacts with HBr,the reaction occurs in two steps.The attacking agent in the first step is __________.

Page 21

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Chapter 20: Organic Chemistry II

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Q1) The typical amino acid,NH₂CHRCOOH,has pK_a1 and pK_a2 of 2.4 and 9.8,respectively.What is(are)the major species in an aqueous solution whose pH is 2.5?

Q2) When aldehydes react with Tollens reagent,

A)a red precipitate forms.

B)silver ions are produced.

C)a ketone is produced.

D)the aldehyde reduces silver ions.

E)an alcohol is produced.

Q3) Identify compounds 1 and 2 in the reaction scheme below. CH₃CHCH₂ + H⁺/H₂O \(\rightarrow\) 1 + K₂Cr₂O₇/H⁺ \(\rightarrow\) 2

Q4) Kevlar is produced from HOOC-C₆H₄-COOH and H₂N-C₆H₄-NH₂.Write the formula for Kevlar.

Q5) Which atom of formaldehyde,H₂CO,is a Lewis acid site?

Q6) Which atom of formaldehyde,H₂CO,is susceptible to attack by a nucleophilic reagent?

Q7) What reactants would be used to synthesize diethyl ether?

Page 22

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