Pharm Practice Exam

7/30/2019 Pharm Practice Exam

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C161f11fv1 1

Chemistry 161 Final Exam December 16, 2011

Student Name (Print): ____________________

Recitation Section Number: Recitation Instructor: __________________The exam booklet has 55 questions for credit and one additional question to check the color of your

exam booklet. Please answer all 56 questions on the OpScan sheet. There is no penalty for guessing.

If you do not find the exact answer, bubble in the best choice. At the end of the 3 hour exam period,please hand in only this top sheet and your OpScan form. If you finish early, please do not disturb

your fellow students. A proctor will check your picture ID, OpScan form, signature and calculator

during the exam. The use of calculators with permanent memories (graphing calculators), cell

phones, pagers, PDAs or other electronic devices other than a basic scientific calculator is

expressly forbidden. The last page of the booklet contains a periodic table along with other usefuldata. The use of any other notes or information on this test or taking extra time to bubble in your

answers will be considered a violation of the Academic Honesty provisions of the student code. Exam

scores will be posted as soon as possible.DO NOT OPEN BOOKLET UNTIL INSTRUCTED

ON THE OpScan FORM (Use a #2 pencil or darker)

1. SIGN your name across the top of the form.

2. Code the following information (blacken circles)

Your Name (LAST NAME FIRST)

Your RU ID NUMBER

[Start under Box A and continue to Box I]

Your RECITATION SECTION NUMBER in K & L[Sections 01-09, code a 0 under box K]

Your EXAM FORM NUMBERunder box P

Section Numbers and Initials of instructors are listed on the next page

BL = B. Langowski, DS = D. Siegel, , GG = G. Govindarajoo, HS = H. Sangari

RP = R. Porcja, NS = N. Shankar, FG = F. Guerra, PS = P. Sahoo, RA = R. Agarwal

YS = Y. Shin, HZ = H. Zhang, KS = K. Sethi, EH = E. Hove, NM = N. Marky

Periods: 1 = 8:25- 9:20 or 9:30-10:25, 2 = 11:10-12:05

3 = 11:45-12:40, 12:15-1:10 or 12:50-1:45

5 = 3:35-4:30, 6 = 5:15-6:10, 8 = 8:25p-9:20p

3. In the Birthdate section bubble 1411

Your EXAM FORM is


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Sec Per. Instr Sec Per. Instr Sec Per. Instr

01 M3 FG 19 M1 HS 37 M8 RP

02 M5 FG 20 M3 GG 40 M2 EH

03 M5 GG 21 M3 NM 41 W2 KS04 W3 PS 22 W1 KS 50 T1 BL

05 W5 PS 23 W1 HZ 51 T1 HS

06 W5 RA 24 W3 GG 52 F1 NS

07 F3 FG 25 Th1 KS 53 F1 HS

08 F5 FG 26 Th1 NS 54 F3 NS

09 F5 NS 27 Th3 KS 55 T3 HS

OS EH

Please bubble 99

28 Th3 NS

29 Th3 DS

12 M2 NM 30 M6 BL

13 W2 HZ 31 M6 RP

14 W2 RA 32 M6 PS

15 Th2 KS 33 W6 RP

16 M2 HS 34 W6 RA

17 W2 NM 35 M8 BL

18 M1 EH 36 M8 YS


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Your EXAM FORM is1 Which one of the following molecules is the most polarizable?

A. H2

B. F2C. Cl2D. Br2

E. I2

2 A 54.4 g sample of aluminum (specific heat 0.902 J/g C) is heated to 99.00C and then dropped

into 65.0 g of water in a calorimeter at an initial temperature of 23.19C. What is the final

temperature of the mixture? The specific heat of water is 4.180 J/g C.

A. 42.81 C

B. 34.79 C

C. 28.43 C

D. 47.13 C

E. 52.71 C

3 Which of the following species show resonance?X. NO2

-

Y. O3Z. CO2

A. Z onlyB. Y and Z

C. X only

D.X and Y

E. X and Z


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4 Calculate the lattice energy of calcium chloride from the following data:

Enthalpy of sublimation of calcium: +178.2 kJ/mol

Bond energy of chlorine: +243 kJ/mol

First ionization energy of calcium: +590 kJ/mol

Second ionization energy of calcium: +1145 kJ/mol

Electron affinity of chlorine: Cl-(g) Cl(g) +e- +349 kJ/mol

Hfcalcium chloride: -795.8 kJ/mol

A. 2254 kJ/mol

B. 858 kJ/mol

C. 2133 kJ/molD. 2603 kJ/mol

E. 3049 kJ/mol

5 Which one of the following lists is correctly in order from lowest to highest first ionization energy?A. Li < Be < B < O < F

B. F < O < Be < B < Li

C. Li < B < Be < O < FD. B < Li < Be < F < O

E. O < F < B < Be < Li

6 Which of the following molecules are polar?

W. BeF2 Y. NCl3

X. H2O Z. CO2

A.X and Y onlyB. W, X, and Y only

C. X only

D.W and X onlyE. All of them


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7 A solution is made by dissolving 54.0g of silver nitrate in enough water to make 350.0 mL. A

10.00mL portion of this solution is then diluted to a final volume of 250.0 mL. What is the total

concentration of ions present in the final solution?

A. 0.0726MB. 0.0363M

C. 0.908M

D. 1.82ME. 0.0122M

8 If X represents the central atom in the following compounds, what is the proper order of decreasing

F-X-F angle in the compounds below? (Largest angle first, smallest angel last)

I. BF3 II. CF4 III. PF3

A. II > III > I

B. I > II > III

C. II > I > IIID. I > III > II

E. III > I > II

9 A 250 mL container of CO2 exerting a pressure of 1.00 atm is connected through a valve to a 500

mL container of O2 exerting a pressure of 2.00 atm. When the valve is opened, the gases mix,

forming a 750 mL mixture of CO2 and O2. What is the total pressure of this mixture?

A. 1.50 atmB. 1.67 atm

C. 1.33 atm

D. 2.50 atm

E. 3.00 atm


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10 Which molecule or ion has the same shape as ICl4-?

A. SF4

B. XeCl4

C. CCl4D. PH4

+

E.

BrF4+

11 To produce Mn(ClO4)x, 3.62 g of ClO4-are needed for every 1.00 g of Mn. What is x?

A. 1

B. 2

C. 3

D. 4

E. 5

12 Which has the highest number of unpaired electrons?

A. Fe2+

B. Mn2+

C. Cr3+

D. Cu+

E. Cr


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13 In solid form, which of the following is an example of a covalent network crystal?

A. CH4B. CO2

C.NaCl

D. SiO2

E. CaCl2

14 What is the maximum amount of H2O that can from starting with 0.24 mol of NH3 and 0.35 mol of

O2?NH3 + O2 H2O + NO2 (unbalanced)

A. 0.42 mol

B. 0.30 molC. 0.36 mol

D. 0.24 mol

E. 0.48 mol

15 A compound contains only C, H, N and O. Combustion of 15.0 g of the compound produces 23.2 g

CO2, 5.70 g H2O and 2.96 g N2. What is the empirical formula of the compound?

A. C2H3NO

B. C2H4N2O3

C. C2H5NO2

D. C3H3N3O2

E. C5H6N2O3


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16 Which of the following elements is a transition metal?

A. Mg

B. Ge

C. ID.V

E. Sm

17 The rate of effusion of an unknown gas was measured and found to be 55.4 mL/min. Under the

same conditions, the rate of effusion of O2 is found to be 51.8 mL/min. Which of the followingcould be the unknown gas?

A. HFB. F2

C. N2

D. CH4E. CO2

18 What is the ground state configuration of V2+

?

A. [Ar] 3d1

4s2

B. [Ar] 3d3 4s2C. [Ar] 3d

54s

2

D. [Ar] 3d3

E. [Ar] 3d5


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19 Consider the following balanced redox reaction:

2Cr3+

(aq) + 4OH-(aq) +3MnO2(s) 2CrO4

2-(aq) + 2H2O(l) + 3Mn

2+(aq)

Which of the following is true?

A. Cr3+ is the oxidizing agentB. The element Mn is reduced

C. OH-is reduced to H2O

D. OH-is oxidized to H2O

E. The reaction occurs in acidic solution.

20 An ionic crystal of aluminum oxide has a cubic unit cell with aluminum ions at the center of eachedge and at the center of the cube. What is the total number of aluminum and oxide ions in the unitcell ofAl2O3?

A. 5 ionsB. 7 ionsC. 10 ions

D. 15 ions

E. 20 ions

21 If a 100 gram sample of a compound is found to contain 8 percent hydrogen by mass, which one of

the following statements is correct?

A. A 50 gram sample of the same compound would contain 4 percent hydrogen by mass

B. A 10 gram sample of the same compound would contain 8 grams of hydrogen.C. 80 grams of the compound would contain 10 grams of hydrogen.

D. A 40 gram sample of the compound would contain 8 percent hydrogen by mass.

E. 40 grams of this compound would contain 4 grams of hydrogen.


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22 Consider the set of isoelectronic atoms and ions S2-

, Cl-, Ar, K

+, and Ca

2+. Which is the correct

arrangement of relative radii?

A. S2-

> Cl-> Ar > K

+> Ca

2+

B. Ca2+

> K+

> Ar > Cl-> S

2-

C. S2-

> Cl-> Ar < K

+< Ca

2+

D.

S

2-

< Cl

-

< Ar > K

+

> Ca

2+

E. Ar < Cl-< K

+< Ca

2+< S

2-

23 How many sigma and pi bonds are in the following structure?

C

C

C

C

CC C

C

C

C

N

H

H

H

H HH

H

H

H

A 15 5B 20 5

C 15 5

D 20 6

E 18 7


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24 Consider the following unbalanced equation:

CaN2C (s) + H2O (l) CaCO3 (s) + NH3 (g)

What is the percent yield of NH3 (g) in this reaction if 12.5 g of NH3 is produced when 60.0 g

CaN2C is reacted with 28.0 g of water?

A. 98.0 %

B. 47.2 %C. 51.4 %

D. 70.8 %E. 39.6 %

25 Consider the following series of reactions (unbalanced). Starting with 3.0 moles of ammonia, (and

excess of the rest of the reactants), how many moles of calcium nitrate could be obtained? (assume100% yield)

NH3 + O2 N2O5 + H2ON2O5 + H2O HNO3

HNO3 + Ca(OH)2 Ca(NO3)2 + H2O

A. 1.5 molesB. 2.0 moles

C. 2.5 moles

D. 4.0 moles

E. 3.0 moles

26 Magnesium (used in the manufacture of light alloys) reacts with iron(III) chloride to formmagnesium chloride and iron.

3Mg(s) + 2FeCl3(s) 3MgCl2(s) + 2Fe(s)

A mixture of 41.0 g of magnesium and 175 g of iron(III) chloride is allowed to react. Identify the

limiting reactant and determine the mass of the excess reactant present in the vessel when thereaction is complete.

A. Limiting reactant is Mg; 67 g of FeCl3 remain.

B. Limiting reactant is Mg; 134 g of FeCl3 remain.

C. Limiting reactant is Mg; 104 g of FeCl3 remain.D. Limiting reactant is FeCl3; 87 g of Mg remain.

E. Limiting reactant is FeCl3; 1.7g of Mg remain.


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27 At a given temperature and pressure, it takes 24 hours for a 1.5-L sample of He gas to effuse

through a porous membrane. How long does it take for 1.5-L of O2 gas to effuse under the same

conditions through the same membrane?

A. 8.5 hB. 12 h

C.

48 hD. 60. h

E. 68 h

28 The threshold frequency to eject an electron from the surface of a metal is

3.15 x 1014

s-1

. What is the kinetic energy of an electron ejected from the surface of the same metalif it is bombarded with a light of 354nm?

A. 2.09 x 10-19 JB. 5.62 x 10

-19J

C. 7.71 x 10-19

J

D. 6.85 x 10-19

JE. 3.53 x 10

-19J

29 The Lewis structure of which of the following compounds can exhibit an expanded octet?

A. SO3

B. O3C.NO2

D. BeH2E. OF2


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30 How many protons, electrons and neutrons are in the47

Ti2+

ion?

protons electrons neutrons

A 22 22 23

B 20 22 25

C 22 20 25

D 22 24 25E 25 20 22

31 Which one of the following is a redox reaction?

A. 2Na(g) + Cl2(g) 2NaCl(s)

B. Ba2+

(aq) + SO42-

(aq) BaSO4(s)

C. K2Cr2O7(aq) + 2KOH(aq) 2K2CrO4(aq) + H2O(l)D.Na2CO3(s) + 2HCl(aq) 2NaCl(aq) + CO2(g) + H2O(l)

E. H2O(l) H+(aq) + OH

-(aq)

32 Which of the following is a heterogeneous mixture?

A. Copper wire

B. A steel girderC. Muddy water

D. Salt waterE. Filtered, dry air


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33 Which pair of the following species have identical Lewis structures?

W. NO2-

X. CO2 Y. O3 Z. SF2

A. W and XB. X and Z

C. X and YD. W and Y

E. Y and Z

34 An iron supplement pill contains iron in the form of Fe2+

. The iron is analyzed by titration with

KMnO4 solution (source of MnO4- ions). The reaction is:

5Fe

2+

(aq) + MnO4-

(aq) + 8H

+

(aq)

Mn

2+

(aq) + 4H2O(

) + 5Fe

3+

(aq)

The iron in the pill reacts completely with 25.0 mL of 0.0100 M KMnO4 according to the reactionabove. What is the mass of iron in the pill?

A. 14.0 mgB. 2.80 mg

C. 69.8 mg

D. 21.0 mg

E. 42.0 mg

35 Which pair of molecules or ions are both planar

W. CH3+, CH3

-X. NH3, BF3 Y. NH3, CH3

-Z. BF3, CH3

+

A. Y and Z

B. Y only

C. Z onlyD. W and X

E. W and Y


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36 H2O has significant hydrogen bonding, while H2S does not. This can best be explained by which

of the following statements?

A.H2O is bent while H2S is linearB. The H-O bond in H2O is stronger than the H-S bond in H2S

C. Sulfur has a higher ionization energy than oxygen

D. Sulfur is larger and less electronegative than oxygenE. H2S is a larger molecule with stronger London forces

37 All of the following properties increase with increasing intermolecular forces, except:

A. Surface tensionB. Melting temperature

C. Vapor pressure

D.ViscosityE. Boiling temperature

38 The Heisenberg Uncertainty principle says that we cannot know both the position and the

momentum of a particle to infinite certainty at the same time. One reason for this is because:

A. Particles are also waves and so dont have a defined momentum.B. The equipment is not sensitive enough to measure both at the same time.

C. The particles are traveling too fast to measure both position and momentum.D. The photons do not have a well-defined position and so cannot be used to find particles.

E. Observing an objects position with photons changes the momentum because the photons

have momentum.


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39 In which of the following pairs does the ion have a larger radius than does the neutral atom?

A. Cl/Cl+

B. Al/Al3+

C.Na/Na+

D. Li/Li+

E. Cl/Cl-

40 A 150 mL of O2(g) is collected over water at 20 C and 758 torr. What volume will the same

sample of oxygen occupy at STP when it is dry? The vapor pressure of water at20 C is 17.54 torr.

A. 125 mLB. 136 mL

C. 144 mL

D. 165 mLE. 175 mL


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41 Consider the phase diagram below.

T (K)Based on the above phase diagram, which of the following statements is TRUE?

A. The critical pressure is 50 torr.

B. At 120K, the material will transform from gas to liquid to solid as the pressure is increased.

C. At 120K the solid will turn to a liquid as the pressure is increased.D. The triple point occurs at 300K and 400 torr.

E. The boiling point at 400 torr is approximately 115K.

42 Calculate the enthalpy of formation of CH4(g) from the following thermochemical equations.

CH4(g) + 4F2(g) CF4(g) + 4HF(g) H = -1942 kJ/mol

C(graphite) + 2F2(g) CF4(g) H = -933 kJ/mol

H2(g) + F2(g) 2HF(g) H = -542 kJ/mol

A. +94 kJ/mol

B. -88 kJ/mol

C. -54 kJ/mol

D. +83 kJ/molE. -75 kJ/mol

0

50

100

150

200

250

300

350

400

450

500

0 50 100 150 200 250 300 350

P

Torr


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43 A 1.50 gram sample of a gas occupies a volume of 542 mL at a pressure of 675 Torr and a

temperature of 20oC. What is the molar mass of this gas?

A. 60.0 g/mol

B. 75.0 g/molC. 90.0 g/mol

D. 105 g/molE. 120 g/mol

44 Which compound has the highest lattice energy (i.e., the strongest ionic interactions)?

A. LiF

B. NaFC. LiCl

D. NaBr

E. LiI

45 What mass of calcium citrate, Ca3(C6 H5 O7 )2, (Molar Mass = 498.44 g/mol) is required to furnish

1.25 g of calcium?

A. 5.18 gB. 3.02 g

C. 15.5 g

D. 8.75 g

E. 3.63 g


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C161f11fv1 19

46 Which of the following compounds is incorrectly named?

A. CuI; copper(I) iodide

B. Ba(NO2)2; barium nitriteC. P2O5; diphosphorus pentoxide

D.H2SO3; sulfurous acid

E. AlBr3; aluminum tribromide

47 What is the correct result of the below calculation, rounded to the correct number of significant

figure (s)?

821.212.5

3.9444.15

A. 0.4

B. 0.43

C. 0.425D. 0.4254

E. 0.42538

48 Lithium forms compounds which are used in dry cells and storage batteries and in high-temperature

lubricants. It has two naturally occurring isotopes,6Li (isotopic mass = 6.015121 u) and

7Li

(isotopic mass = 7.016003 u). Lithium has an atomic mass of 6.9409 u. What is the percentabundance

6Li?

A. 92.50%

B. 86.66%C. 46.16%

D. 7.504%

E. 6.080%


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49The density of water is 1.00

g

cm3. What is this density in

kg

m3?

A. 1.00 x 106

B. 1.00C. 1.00 x 10

3

D. 1.00 x 10-3

E. 1.00 x 10-6

50 What is the total heat necessary to convert 20.0 g of ice at - 20C to liquid water at 18C? Hfus of

ice = 6.01 kJ/mol, specific heat of ice = 2.108 J/g C, specific heat of water = 4.18 J/g C.

A. 9.02 kJ

B. 8.17 kJC. 7.52 kJD. 2.34 kJ

E. 4.17 kJ

51 What color is your exam?

A.white

B.pinkC. green

D. yellow


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C161f11fv1 21

ConstantsandFormulas

1 J = 1 kg m2/s2 R = 0.08206 L atm mol-1 K-1 = 8.3145 J mol-1 K-11 J = 1 kg m2/s2 NA = 6. 022 x 1023 mol-11 Latm = 101.325 J h = 6.626 x 10

-34

JsT(F) = 9F/5C T(C) + 32F c = 2.998 x 108 m/s

T(K) = T(C) + 273.15 g = 9.80665 m/s2

d

QQE 21

2

21

d

QQF

FC = V (L + S)

E = h c = )4/( hpx

B = 2.179 10-18J

1.097 10

H = U + PVqp = nH qv = nU

PV = nRT % 100

Soluble Exceptions Insoluble

Li+, Na

+, K

+, Rb

+, Cs

+, NH4

+none

NO3, CH3COO, ClO3 noneCl, Br, I Ag

+, Hg2

2+, Pb

2+

SO42

Ca2+

, Sr2+

, Ba2+

, Ag+, Hg2

2+, Pb

2+

Li+, Na

+, K

+, Rb

+, Cs

+, Ba

2+OH

Li+, Na

+, K

+, Rb

+, Cs

+, NH4

+CO3

2, PO4

3, S

2,CrO4

2

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