gre chemistry3

8/3/2019 GRE Chemistry3

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THE GRE CHEMISTRY TEST

Time: no Minutes

150 Questions

\

Directions: Choose the best answer for each question tuui mark

the letter of your selection on the corresponding cnswei- sheet,

1. For an ideal solution, which of the following is fare true?

componentsI. l1H = 0 III.

Psolution" ' L : p.

mixing i 1

II. . D . Smixing

= 0 componentsIV. 1I G . = -RL:n.lnx.

mixin g i1 1

(A) I , III and IV CD) I and III

(B) III and IV (E) I only

(C) I, II and III

2. Select the correct product of the following reaction:

AU ,~ ?aq.HCl

92

(A) O-ChIOl

(B) 2,6-dii

ee ) p-chlo

Choose the

of nitrylcli

(A) 6

(8) 0

(C) 3

Arrange th

strength:

(A) O-H••

(B) Q-H.

e c ) O-H.

(D) N-H.

(E) F-H..

W.hl.ch s

(A) Agel

(B) NaF

(C) CuBr

Reacno.n:



o

(A) o-chloroau.iline (D) 2,6-dichlorobenzene

(B) 2, 6-dichloroaniline (E) 2,4 ,6-trichloroaniline

(Cj p-chloroaniline

3. Choose the number of fundamental vibrational modes in a molecule

of nitryl -chloride , .

(A.) .6

(B) 0

(C) 3

(D) 4

(E) 2

~4rrangethe following hydrogen bonds in order of increasing

strength: O-~ .•. Cl; O-H••. N; F-H.•. O and N-H.•• ).

_) O~H••. CI< F-H ••. O < C)-H... N< N-H .•• 0

B) O-H•.. N<O-H... Clc N-H .•• 0< F-H•.. O

C) O-N•• _CI< N-H ..• O< O-H, .. N < F-H•.. 0

) N-H ••• 0< a-H ••. N< F-H ••• 0 < O-H••• Cl

E) F-H•••0 <N-H.•. 0<O-H... Cl <O-H.••N

Which substance has the greatest lattice energy?

A) AigCl

~,~~(C) Cu~r

S. The product of the reaction below was subject to an infrared

spectral analysis. Based on its IR spectra pictured below, one

can deduce that the product is:

Reaction: CU-CH CI + Mg ether CO2 H2S04s 2. ____.._. H20 ~product

93



(A) o-Chloroaniline (D) 2',6-dichlorobenzene

(B) 2, 6-di!chloroaniline (E) 2.4 ,6-trichloroaniline

(C) p-ehloroaniline

Choose the number of fundamental vibr'ational modes in a molecule

of nitryl chloride,

(A) 6

(B) 0

(C) 3

(D) ,4

(E) '2

Arrange the following hydrogen bonds in order of increasing

strength: O-~••• 01; O-H••. N; F-H •.. 0 and N-Ji ••• ).

(A)O-H •.• 01< F-H ••• 0 <O-'H.•• N<N-H••• 0

(B) O-H•.• N<O-H..• Cl< N-H. 000< F-H .•• O

(0) O-H.•• Cl< N-H.•• O<O-H .•. N<F-H ... O

CD ) N-Hoo.O< O-H... N< F-H.,.O <O-H. ooCl

(E) F-H ... O<N-H ••• O<O-H ... Cl <O-H ... N

Which substance has the greatest lattice energy?

CA ) Agel

(B) NaF

(D) KI

(E) MgO

(C) CuBr

6. The product of the reaction below was subject to an infraredspectral analysis. Based on its IR spectra pictured below. one

can deduce that the product is;

Reaction: CH,CH2C1 + Mg ether C02 ~ ~ ~ g 4 product

93



Wavenumber,-I

em

I-' I-'

IV I-'

o 0

~~-r~~-r~--~~~~~o~.~o~--~--~--~----T-'100

80

60

40

20

9 105 6 7 8

Wave length, 11

(A) a.cetaldehyde

(B) propanol

(D) acetone

(E) propionic acid

(C) ethanoic acid

7. A chromatogram obtained using a differential detector would mostclosely resemble which one of the following diagrams?

Water has a

vaporpressl

sucrose is 0

(A) 15.2 to:

(B) 23.8 to.

{C) 29.7 to

Which one 01

able to ionic

CA ) high m 4

eB) fragilit

(C) crystal

state)

Indicate the

transformati

(Ql

Qltil

(B) (C) til(A)§ s (A) H20; HI.

0.ilUlQlQ)

(B) LiAlHIo;H

H H0 0

LiAlHlo;.jJ .jJ

(e)oQl Q J

H .jJ.,-1

- 2 ((D) H2O. H iime

Q Tillie· Time

(E) LiAlHlo;

(E)CD)

94

In an adiaba

(A) increas

(B) decreas

(C) remain



Water has a vapor pressure of 23.76 torr at 25~C. What is the

vapor peess ure of a solution of sucrose. if' the mole fraction of

sucrose is O.250?

(A) 15.2 torr

(B) 23.8 torr

(D) 5.9 torr

(E) 17.8 torr

(C) 29..7 torr

Which one of the following characteristics is not usually attribut-

able to ionic substances?

(A) high meltlng point

(B) fragility

(D) deform when struck

(E) well defined three-dimen-

sional structure

(C) crystalline (in the solid

state)

Indicate the reagents and/or compounds required to carry out the

transformation shnwnbelow:

0=0 ?1, 6- hexanedione

(A) H20; HzSO 4 ; heat; KMnO 4 ; 03; Zn

C E l LiAlH4;K2Cr207. H20; NH20H

(G) LiAIH4i NaOH, heat; KMn04

+CD ) H20. H ; KaCr.207; NH20H

(E) LiAlH4; H2S01t,heat; O s i Zn

In an adiabatic system. if work is done. the temperature must:

(A) increase. (D) inceease then decrease.

(B) decrease. (E) decrease then increase.

(C) remain the same.

95



12. The Perkin reaction in which o-chlorobenzaldehyde is heated with

acetic any hydride and its salt sodium acetate, results in the pro-duction of:

CH2r.:HCOOH

Cl~ (C)

l).

CH=CH20H

&Cl

~

-.

(A) (B)

CH=CHCOOH

C 1 D . (E)

~

(D)

13. The quality of a particular monochromator is dependent upon

which of the following characteristics? .

L light gathering power III. radiant output purity

II. spectral band width IV. high signal to noise ratio

(A) I; II and III (D) II and IV

(B) I and IV· (E) all of the above (I-IV)

,

(e) II,III and IV

14. In the plot below of A Irt-1cm2morl ver-sus I(c/mol dm-3) them .slope is equal to:

150

148

~ 146oS

"'."144o~'~ 142

~ 140

138~~~~ __.~~~

0·000 0·080 0-160

v (cImo!' dr, i"3)

96

(A) A 0

m

(B) the Kohl

(e) the molal

To distinguisl!

one would use

(A) Sandrnay,

(B) Wittig rei

(e) Ninhydri:

!!'embers of tlmanufacture «

produce aerosThe name of 1 )

(A) alkaline e

(B) noble gas

(e) actinides.

The coordtnatk

CA ) 3

(B) 6

ee ) 2

If each of the j

of them would

tion. Which re

.+CA ) 03/Zn ,H

(B) HI

(e) hot KMnO



19. The·following three analytical methods - spectrophotometry (S).

photoluminescence (P) and fluorometry (F) - have differences ir;

theirl'espective sensitivities. Ar-range them in order, from the

least to the most sensitive, and then choose the correspondinganswer.

(A) P < F < S (D) P<S<F

(B) S=F<P (E) none of the above

(C) F>P >8

20. In a galvanic cell the following reaction takes place:

+ -2HzO ~ 02(g) + 4H + 4e

.Itoccurs at the:

(A) cathode. (D) external conductor.

(B) anode. (E) none of the above

(C) cathode and anode.

21. Which of the addition reactions below will not proceed under or-dinary circumstances?

(A) I and II ·(D) I. II and III

(B) IV only (E) I, II and IV

(C) III only

22. A compound that is 17%sulfur (atomic weight 32.1) reacted com-

pletely to Yield 1.8 grams of HZS2.07 (molecular weight 178.1).

Which of the choices below should. be used to find the total weig:-of the original compound?

98

.8--x:~8.1

1.8 x178.1

1.8) 118.1 x

_ch of the

rmction?

(D)

A)

) Clem

)

e MaxweH

eli by Which



fA)1.8 2 17

(D)1.8 x 2(32. ,0 100'

-- x--' x- x 17178.1 32.1 100 178.1 1

(B)1.8 x 32.1 , 100

(E)1.8 2(32.1) x17

178.1-1- x l'r -,-- x

178.1 T Im

(e)1.8 1 17

178.1 x 2(32.1) x 100

Which of the compounds below is the product of the following

reaction?

icon

(0) (E)

The above reaction (Q. #23) is known as a:

(A) Wolff-Kishner reduction. (D) Baeyer-VilIiger oxidation.

(B) Clemmensen reduction. (E) Roaenmund reduction.

(C) Friedel-Crafts reaction.

The Maxwell distribution of molecular velocities is bes,t represent-

ed by which of the following diagrams?

99



_3. The rate constant of a chemical l'eactiGl'lis characterized by all of

the following except:

(A) it is always dependent upon the composition of the reaction

mixture.

(B) it depends exponentially upon the temperature.

(C) itis proportional to e-Il&/Rt (where Eis the reaction's act-

ivation energy).

CD) the ~urim equation can be used to calculate it;

(E) itoften follows the Arrhenius rate law',

The c;iistribution of molecular speeds is dependent upon the mol-

ecular mass. Above, the speeds of Hz0, Hz, O2. and CO 2 (vs ,

the probability of the speed occurring) are shown. Select the

answer which matches each molecule with its corresponding speeddistribution curve.

01> = :.,_j

H::loUo

'C IO J(l)

g .

lHo

. : > ,

.j.J

·rlH

·rl

.or(j

,Q

oi o . l

c, 200 400 EOO 800 1000

speed m/s

(A) (D- H20; (ID- 02; @- G02;@- H2

(B) c ' D - H2; 1])- HzO; @- C02; @- 02

(C) C D - 02; (ID- C02; @- H20; @- H2

CD) C D -C02; ® -H2; ® -02; ® -H20

(E) (})- HzO; (ID- C02; @- HZi@- 02

101



32. All of the following tests are used to identify aldehydes except:

The boiling po1. Tollens' test IV. the ammonia test attractive fore

substances (NU. Fehling's test V. Benedict's test boiling points

-III. Baeyer's test (A) HF> CO

(A) I, II and V (D) 11 arid IV (13 ) Baelz > II

(B) III and .IV (E) III only eC) HF> Ba(]

(e) IV only

30. tHg;zClz(s) ~ iH2(g) -+ HgC:l)+ HCl(aq) (not balanced.) • For thereaction above;

lise = -31. 0 JIk molem

L\G8 = -25.82 kJ/molem

T = 298 k

L\E8 = -27.61 kJ/molem

Using the appropriate information. calculate the enthalpy of thereaotton , '

CA) -38.69 kJ Imole (D) -21. 76 kJ Imole

(E), 0 kJ/mole,B) -35.06 kJ/mole

(C) -16.58 kJ Irnole

31. Transmetallation of an aryl bromide (or iodide) with an alkyllith-

fum results in the production of a reagent that is capable of

undergoing the Same reactions as the Grf.gnard' reagents; thisreagent is:

(A) arylmetal. (D) arylhalide,

(B) arylIithium. (E) alkyllithillm-bromide.

(C) a1kylbromide (or iodide).

102

Bor a second or

(A) the half li~

(B) the rate ca

(G)

tWDreage]

no express

two reagen

(D) a plot of 1

(E) the concan

t0rs of til

The amount of 4

ing the sample

What per-cerrtag

O.30M AgNOa j

14.0g sample?

26'.7(.3)(1(A) --"35.5(1

26.7P)(3(B} 1000

26.7(35.(G) (.3)(1000

Argon at 35°(j

is allowed to 4

temperature c

could be 0



Fo!' a second order reaetion alii.of the following are true except:

(A) the half life is not independent of the initial concentration.

(B) the rate can have a first order dependence on each of the

two reagents. ~

(C) no expression for the variation in the concentrations of the

two reagents can be derived.

(D) a plot _of l/[Alt

against t is linear.

(E, the concentratioIf Of the reactant does not decrease by fac-tors of t in a' series of regularly spaced time intervals.

4. 'Fhe amount of chloride in a water supply is determined by titrat-

ingthe sample a'-gainst AgN03 as follows:

AgNO!(aq.) + CC(aq) -+ AgCl(s) + NO~(aq.)

What percentage of chloride is present in the water if 26.7 ml ofO.30MAgNO

sis neceasary to react with all of the chloride in a

14.0g sample? (Atomic weight Cl = 35.5.)

(A)26.7 (.3) (1000) (D)

26.7(14)(.3)

35.5(14) (1000)(35.5)

(B)26.7,3)(35.5)(100)

(E)26.7(14)

100U(14) (.3)( 1000)(35. 5)

(C)26.7(35.5)

(.3){1000){14)

The boiling point of a aubs'tance is indicative of the intermolecular

attractive forces' present. With this in mind, list the following

substances (Ne, HF, BaClz• Hz and CO) in order of decreasing

boiling points and then 'select the correct answer.

(A) HF> CO >BaC1z > H2> Ne (D) Hz > HF> BaClz·? CO> Ne

(B) BaC1z > HF> CO >Ne > Hz (E) Bael2 > co » HF > Hz > Ne

(C) HF> BaC1z . > Ne > Hz > CO

Argon at 35°C and 1 atm. pressure in a container of volume 400crrf

is allowed to expand to 800cm3 and is simultaneously heated to a

temperature of 115°C. The entropy change that would resultcould be obtained by solving which of the following equations?

103.



(A) nRln(1l5°C/35°G) + nC In(800cm 3/400cm3)v,m

(B) nRln[(388k/308k) + (80012m3J400cm3)]

(C) nR(800cm 3/400cm3) + nC (38S'k/30Sk)

v,m

(D) nC, In[(800cm3/400cm3) - (115°C/35°G)]

v,m

(E) nRln(800cm3/400cm3) + nC In(38Sk/30Sk)

v,m

37. Detectors are often used in conjunction with chromatographic

columns. They measure the separated sol utes as' they emerge.

All of the features listed below are used in evaluating a detector

except for

(A) stability. (D) noise level.

(B) mass flow rate. (E) response time.

(G) Iirieari ty ,

3S. The Aufbau principle is one that governs

(A) Coulomb potential. (D) electronic configuration.

(B) vapor pressure. (E) the entropy.

(C) critical molar volume.

:;\,9. Suppose that a sample has been analyzed by two different methods

yielding standard deviations Sl and S2' Before t can be calculated

81 and S2 have to be examined to determine whethe:r or not the

difference between them is significant. Given the following in-

formation and the table below, calculate the variance-ratio (v II')

and determine if Sl and S2 differ- significantly.

Method 1 Method 2

Xl ::c 41. 24 X 2 = 42.34

S1 = 0.11 S2 = 0.13

nl = 4 n2 = 5

104

F Va

n - 1

forsmaller S'2

3 9.

4 6.

5 5.

6 4 .10 3.

20 3 .

(A) v/r=1.40

(B) vir = 0.72

(e) vir = 7.34

(D) v I I ' ; : : 4.66

(E) none oftn

The isomers of

C A ) 2. 3-expoyl

(B) tetrahydr<J

(C) t-butyl et

To conver-t brOil

of steps is requ

them in the app

response,

Note: Each on~or not a1

1) dry etl2) excess

3) carbon

(A) 6,1,5.3,5.

(B) 1,5.6.6,3,

(C) 5.1 ,6 ,3.7 •



F Values at the 95%Probability Level

n - 1 n - 1 for

for larger S2

smaller S2 3 4 5 6 10 20

:3 9.28 9.12 9.01 8.94 8.79 8.66

4 6.59 6.39 6.26 6.16 5.96 5.80

5 5.41 5.19 5.05 4.95 4.74 4.56

6 4.'16 4.53 4.39 4.28 4.06 3.8710 3.71 3.48 3.33 3;22 2.98 2.77

20 3.10 2.87 2.71 2.60 2.35 2.12

(A) v ir= 1.40, no sigpificant differenc~

(B) v/r:= 0.72, no significant difference

(C) vIr >7.34, the difference is significant

(D) v lr > 4.66, the difference is significant

(E) none of the above

The isomers of butanone include aUof the following except:

(A) 2, 3-expoYbutane. (D) ethyl vinyl ether.

(E) 1,2-butenol.(B) tetrahydrofuran.

(C) t-butyl ether .

To convert bromobenzene into mefhyl benzoate a : certain sequence

of steps is required. TheSE;!teps are listed below. Arrange

them in the appropriate· order and then choose the corresponding

response.

Note: Each one of the steps may be used once. more than once.

or not at all.

1) dry ether2) excess methanol

3) carbon dioxide

4) mineral acid catalyst

5) magnesium

6) HBr7) sodium bicarbonate

(A) 6,1,5,3.5.7.2 (D) 6,5.1,3.2.7.4

(B) 1,5,6,6,3.2,4 (E) 5.1,3,6.2.4,4

(C) 5.1,6,3,7.2 .7

105



42. The name of the compound pictured below is:

CBS

/N -_ C H

-,C H 3

CH" 3

(A) N,N-methylisopropyl-p-methyl aniline

(B) p-isopropyl-p-methylaminotoluene

(C) N,N-dimethyl-}!'l-methylaminotoluene

(D) p-methylisopropylamine-phenyl methane

(E) N-met hyI isopropy l-amin otol uerie

43. In an isolated system this reaction:

Zn(s) + 2H+ (aq) :;. ,H2(g) + Zn2+(aq)

is 'much more likely to take place than this reaction

Zn(s) + C-J+(aq) :t Cu(s) _ + Zn2+(aq).

Which one of the following makes it possible to conclude this'?

(A) Third Law of Thermodynamics

(B) First Law of Thermodynamics

(C) Einstein-Stark Law

(D) Dulong and Petit's Law

(E) Seeond Law of Thermodynamics

44. _In this low boiling azeotrope diagram. select the point where the

azeotrope occurs.

o

106

(A) Q )

(B) @

(C) ®

Elements not f e

and Involving I

as the

(A)

(B) hlilogens.

( C) actinides.

Which of the fo

(A) B··· Cl

(B) a - v - r

(C) p •• ·Br

The evolution

inmineral acid

CA ) an aromati

(B) a tertiary

(C) an aliphatl

(D) an aromati

CE) an alipha:ti

A certainspect

must be applied

molecules. In



(A) 0 0

(II) C I D

(e) ® .

(D) ®

(E) ® _

Elements not found in nature, synthestzed in nuclear reactions

and involving completion of the Sf electronic orbitals are known

as the

(A) lanthanides. -(D) transition metals.

(B) halogens. (E) rare gases.

(C) actinides.

_6. Whichof the follo.wingbonds (0' 0) is the least polar?

(A) B···ci

(B) H·0·1

(e) p •• oBr

(D) C·· ·CI

(E) C·· •1

ti... The evolution of nitrogen gas upon the addition of sodium nitrite

in tnineral acid solution identifies the presence of

(A) an aromatic secondary amine.

(B) a tertiary amine.

(C) an aliphatic primary amine,

(D) an aromatic primary amine.

(E) an aliphatic tertiary amlne ,

:lB. A certain spectroscopic tool used for structure determination

must be applied in the vapor phase. Its use is restricted to small-molecules. In additio-n. itmakes its determinations based on the

energy differences between molecular rotational states. This

teebnique is known as:

107



(A) infrared spectroscepy , (D) mass spectroscopy.

(B) n.m.r. spectroscopy. (E) microwave spectroscopy.

(C) ultraviolet spectroscopy.

49. Using the Laplace equation, calculate the pressure differential ina water bubble with a radius of O. Irnm , ( y ;:: 7 x 10- 2_ N1m )water

(A) 700 N1 m 2

(B) 1400 N 1m 2

(C ) 1000 N 1m 2

CD ) 1200 N1m 2

(E) 70 N 1m 2

50. The stability of a molecule is related to the strength of its cova-

lent bonds. Based on this, select the most stable molecule.

(A) 0;<. (D) C12

(E) HF

51. An isotope :~i;Pudisintegrates by emitting 5a and 213 particles.

The new isotope formed by this process is:

(D) 2~~pU

(E) 2~~RnB) 2~~Fr

(C) 2~~Am

52. Indicate which one of the statements below, regarding nucleo-philicity in a polar pratte solvent , is incorrect.

(A) Nucleophilicity is the affinity of a base for a carbon atom.

(B) P- is more reactive towards methyl iodide than ci".

(C) Second row elements are invariably more nucleophilic thanfirst-row elements of comparable basicity.

.(D) .The rate of an SN2 reaction may be markedly affected by the

nucleophilicily of the attacking group.

108

(E_) The m

53. Reactant fa

by which 0:

(A) an inc

(B) a deer

(0) no ehs

(D) first a

(E) none c

54. A mixture o

heated at 7

and a small

The aqueoulayers arethe chief pr

(A) ethyfr

(B) ethyl i

(e) dimeth

-5. What is the

(A) 5,5-dh

CB) cyelop-

ketal

(e) 3-meth

A cell that i:



(E) The more basic electron pairs tend to be more nuc)eop't l .1."t t t : .

·3. Reactant formation iJl an endothermic reaction would be favored

by which of the following?

(A) an increase in temperature

(B) a decrease in temperature

(e) no change in temperature

(D) first an increase and then a decrease in temperature


-4. A mixture of ethyl acetate and alcohol-free'so<;lium ethoxide isheated at 780 C for eight hours. The mixture is then cooled to 100.

and a small quantity of 33% aqueous acetic acid is slowly added.

The aqueous layer is washed with ether and the combined organiclayers are dried and distilled. Which of the compounds below is

the chief prod uot of the reaction?

(A) ethyl' acetoacetate (D) diethyl malonate

(ll) ethyl isobutyrate (E) ethyl malonic acid

(e) dimethyl adipic acid

What is the principal product of the following reaction?

C ) = o +

(A) 5.5~dimethyl pentanal (D) 2-methyl cYClopentanone

(E) cyclopentane dmiethyl

acetal(B) cyclopentanone dimethyl

ketal

(C) 3-methyl-l ,5-pentanedione

A eell that is described as being "without a liquid junction:"

1 0 9



(A) cannot exist. CD) has a flowing junctionmodification.

(B) has only one electrode.(E) has one electrode in two

electrolytes.0) has two electrodes in the

Same electrolyte.

57. Ifan aromatic or aryl halide is reacted with a strong base such assodium amide .(NaNH2)' and elimination takes place; all of the-following may result except:

(C) ©0:

(A) (B)

(E)D)

58. The heat flow of a system under isochoric conditions is a directmeasurement of

(A,) work. ,CD) fI G .

(B) fiE.

(e) 8 H

(E) entropy.

59'. Select the graph that is typical of the height equivalent of a

theoretical plate (HETP) vs. mobile phase velocity for gas-liquid

and liquid ehromatognaphy (GLC and LC, respectivety) .

(E)

--GLC(A)I

~I~'~~

.------

Mobile phase velocity Mobile phase

110

Mobile p!

(E) ~71Mobile pi

The sfabilitYl

higher bellistructure is

(A) Eaeyer

(B) Pitzer s

(0) dipole-j

500 4(

8.0 7.0



(D)

GLC & LC

Mobile phase velac ity Mobile phase velac ity

(E)

Mobile phase veloc ity

~o . The stability of most cyclcalkanes (which is indicated by their

1:ri.gherboiling and melting points) as well as their non-planar

structure is not dependent upon;

(A) Baeyer strain. CD) Strecker strain.

(B) Pitzer strain-. (E) nonbonded interactions ,

(C) dipele-dipole interactions.

51. 'rhe nmr spe?tra for an isomer of Cr,HBBr2 is shown 'below:

s o o

area 1

8.0 7.0 6.0 5.0 4.0PPM (6)

3.0 2.0 1.0 o

111



Based on this spectra the name of the isomer is:

(A) 1, 1-dibromobutane. (D) 1,2-cis-dibromobutane.

(B) 1, 3-9ibromobutane. (E) l,3-dibromo-2-methyl

propane.

(C) 1-bromo- 2-bromomethyl

propane.

62. For the reaction below

2HN3 +2NO + H202 +4N2

with the following molar enthalpies (at 25°C):'

8 .HNa - Hm = +264,0 kJ /rrrole

eNz - H = 0 kJ Imole

m eH2° 2 - H = -187. 8 kJ Imole

e mNO - H, = +90.25 kJ Imole

m

The chan ge in the standard enthalpy for the reaction is:.

CA ) -896.3 kJ. (D) +742.6kJ.

(B) +937.4 kJ. (E) none of the above

(C) -309.5 kJ

63. , The above calculation is based on a concept presented in.

(A) Dulong's & : Petit's Law. (D) Debye- Hiickel theory.

(B) Graham's Law. (E) Hess's Law.

(C) .Henry's Law.

64. Calculate the pOH of a solution made by mixing 70 ml of 0.10M

NH 3 and 60 ml of 0.05M H'Cl, The reaction is NBs + H30+ +

NH+ + H20 with k = 1.8 x 10-3• -1; b NH3

-3 (0.007) (IO,03J(A) -log(1.8 x 10 ) -log -- CB) logO.8 x 10-

3) - log(_O.04

0.003

112

(c ) -10 g(1. S

(E) -logO. e

Nonmetals wh

(A) are less

(B) have grl

(C) are mort

CD) have la

(E)

Carboxylic ac

catalytic' arnot

(A) azides.

(B) epoxides

(C) ethers.

Which one of

(A) fr-ee-z-ad

(C) E2

Catechol is tn

o~

CI/!catechol --=-ii

What is the



-3) I f 4. O~(C) -log(l. 8 x 10 . + og~3. O~

(E) -10g(1.8 x 10-3) - log (0.004) .0.003

Nonmetals when compared to metals:

CA ) are less electronegative and have smaller atomic radii.

(B) have greater ionization energies and larger atomic radii.

(e) are more electronegative and have smaller atomic radii.

(D) have larger atomic radii and are more electronegative.

(E, have smaller atomic radii and lower ionization energies.

Carboxylic aeids xeact readily with alcohols in the presence of

catalytic amounts of mineral acids to yield compounds called:

CA ) azides. (D) esters.

(E) epoxides.

(C) ethers.

(E) ketones.

Whichone of the following reactions is not usually stereospecific?

(A) free-radical substitution (D) hydrogenation with Pd/Hz

(E) addition of halogens to

oletins

Catechol is treated with four reagents. as follows:

O~

)C-CH2.C1

Clcatechol _Hel

+CHaNH2B -He]· +

C~ DPd

A POCI,

Whatis the structure of D?

113



OM OH OH Which of the foU

(A)

~OH

(B)COOH (C) distribution of e'

OIl

I.

HzC-CHz-CH3 H-C-CIlz-CH3 H~C-CH -NH-CHI r 2 3 A) I and IVOH OH

B) II, III and IOH OH

e n o COOHC) I.rr and II

(D) (E)

H2C-CHOH-NH:

69. In the presence of Niewland catalyst (NR.Cl > Cuel), acetylenedimerizes to form , which upon hydrogenation yields

The two blanks are best completed by which two

substances, respectively?

1. allylacetylene III. 1,3- butadiene

II. 2-butene IV. vinylacetylene

(A) I and III CD) IV and III

(B) II and I (E) none of the above pairs

(e) II and IV

70. The best way to distingUish the presence of two enantiomers

would be:

(A) compare their melting points.

(B) place one of them into solution and pass polarized light

through it.

(e) dissolve each one (individually), in a particular solvent and

then compare their respective solubilities.

(D) examine them for color differences.

(E) compare their respective abilities.

114

Arrange the folIo

H 30+. HzO. Hz.

A) H20 < HF< I

B) HF'< H20 < I

C) Hz < HF < H i

D) H2 < H20 < ]

E) H20 < H z < I

Calculate the nun

acid. (Atomic wei

(A) 27.3(2)(6.02

(B)27.3(2)

163.5

(C)163.5(27.3!

2(6.02 x 10'23

The above



Whicftof the following e~pressions repl'esent(s) a . measure of the

distribution of energy:·

1.. the temperature IU. S (entropy)

lI. E (internal energy) IV. the partition function

(A) I and IV(D) I only

(B) II, III and IV(E) III and IV

(e) I. II' and HI

-2. Arrange the following acids in ord-er of increasing strength:

H30+, H20. H2. eels e02H, H"O~ and HF.

+ -(A) H20 <HF < H2< HaD < HSO", <, GClaC02H

(B) HF < H20 < H2 < BSO; <CCIsC02lJ <HsO+

- + -(e) -H2 < HF < ~O < celsC02H <HsO < HSO",

- +(D) H2< H20 < HF < RSO", <ce13e02H <H aD

+ -(E) H20< ~ < a sO < HF< Hso",<eCl!C02H

-3. Calculate the number of carbon atoms in 27. 3g of trichloroacetic

acid. (Atomic weigbts: C = 12.0, Cl = 35.5, 0 = 16.0, H = 1.0)

(A) 27.3(2)(6.02 xl023)J163.5

(B)27.3(2)

163.5

(D) 27.3(6. 02x 1023)(163.5)

2(12.0)

(E) {673 J , .(6. 02 x 1fi3)

163.5(27.3)

(e) 2(6.02 x 1021)

.t.

The above reaction could best be described as a:

U5



A O . 56g sample of itt'!>n are is dissolved in acid ~the iron is oxi-

di.zed to the +3 state and then precipitated as Fe20g • xH20. This

precipitate is fille'red', washed and ignited to Fe20a' The Fe 203

weighs 0.29g. The reaction is: 2Pe'+ + F~03(S) and the atomicweights Of Iron and oxygen are 55.9 and 16.0 ,respectively. The

percentage of iron in the sample would be equal to:

(A) 100,x0.56 x (55.9)20 . 2 9 1 5 9 . 8

(B) 100x0.,29[(2 x 55.9)/159.8]

0.56

100 )(0.29 x

0.56

(e) 2(55.9) 159.8

(D) 100 x55.9[(2 ~ 159.8) 10.29]

0.56

(E) 100 )([ ( 2 )( 159.8)/0.56]0.29

55.9

One method of reducing carboxylic acid derivatives to aldehydes

is the Stephen reduction. The reaction involves an intermediate

wllich is readily hydrolyzed to the aldehyde .. If the original

carl:!oxylic acid derivative is • nit~ eN and the resulting

aldehyde is © r e B a the interm,ediate is of the form:

(D)

(A)

(e)

©'=:: < :1

on '

(E)

(©- C H = N H t ) : n C l : -

117



80. The graphs below show the behavior of various gases. Which of

these gases exhibits behavior that deviates most significantly

from that expected for an ideal gas?

Temperat ur_e Pressure' Temperat ure

(B) Their elec

(C) Slight dif1

isotope efl

the rate a

CD ) They have

(E) The first

(A) (B)C J

Gas A sr:l0

,> -

(!) x§

C J

.-I ~0 rJ)

t> Ul

(p, const. )C J~p..

Gas B

(C)

The instrument

as well as thatsults in photo~

(n, T const.)

(D)ill .

~-iJro~CJP-i

a lE -t

<

(!)

~UlUlCJ. . . .p.,

(B)C J

~.-I

o> -

(A) an atomicD

(E)

(C) an electro

spectrome

(n, const.) (T, const.)

Vol ime PressureIf an alkene gi'

ozone followed

(B) cns-cn :

81. _Which of the statements below about carbonate error is not true?

(A) If methyl orange is used as the indicator this type of error

will be maximized,

(B) It will be minimized if barium hydroxide is used as the

titrant. (C) eHa-GH-(lI I(j(e) Sodium hydroxide can be prepared and then protected in

such a way as to avoid .thi.s 'type of error.

(E) A solution that has sodium carbonate at the bottom of its

container has minimal error of this kind.

The two missin

(D) Ifthe titrant is stored in a bottle equipped with a tube con-

tainin gAscarite this error will be diminished. _

SE i2

82. Which of the following statements is true of isotopes?

(A) They, have different atomic numbers and the same atomic

masses.

118



(B) Their electzonic 'configurations differ.

(e) Slight differences in chemical behavior of isotopes (calledisotope effects) influence rather the kind of reaction than

the rate of reaction itself.

(D) They have identical chemical behaviors.

(El The first ones discovered were those of neon.

The instrument that is used. to determine the weight of a proton

as well as that of an electron. and is capable of record ing its re-

sults in photographic form is:

(A) an atomic spectroscope. (D) a spectrophotometer.

(B) a mass spectrograph. (E) a spectrcphctcgraphic

analyzer.

(C} an electron paramagneticspectrometer.

'1 If an alkene gives 2-butanone and propanal when treated with

ozone followed by zinc and wa.ter, what is it.s structure?

(A) CH3-CH2-C=CH-CH2-C H3 (D) CH3-CH2.,-cH2

I ICBs CH

I ICH3 CH

I I(B) CH3--Clh-cH=CH-C H-CH 3 CHa

(e) CHa-CH-C--CH2--CHa (E) CHa-C=C H-C lh -cH2-cH3I I ICH2. CBs

The two missing structures A and B are respectively:

SE. NHCOOlI3

GHaCOOH Br2

q B rHCl NaOH

AB

b . CHaCOOH alcohol

5'50 fl

-:- CHa

119



Liquid

~ #5::l.j..l

1 1 1 #2-1Q)

~ #6f . l

#3

A 0.667 B

In th.e above phase diagram numbers are assigned to specificareas. Select the answer which correctly describes the phases

present in a given area.

(A) #3 - solid A and solid A2B (D) #5 - solid B and liquid AB2

(B) #1 - liquid A

(CJ #6 - solid B and solid AB2

In the lab. an acid is usually chosen as a permanent referencestandard in preference to a base. In selecting an acid to lise ina

standard solution all of the following factors should be considered

except:

(A) the acid should be highly dissociated.

(B) the acid should not be volatile. _

(C) salts of the acid should be soluble.

(D) the acid should be a strong oxidizing agent.

(E) a solution of the acid should be stable.

Aeeordmg to Gibbs phase rule. the number of degrees of 'freedom

for a four component system of one phases is:

(A) 5.

(B) 3.

(C) 4.

(D) 2.

(E) 7.

121



91 .

Orbital Diagram

1 1 1 1 I

The above arrangement of electrons in the orbitals of a carbonatom is based on

(A) Heisenberg's Uncertainty

Principle.(D) HundsRule.

(E) Pauli's Exclusion Principle.(B) Lewis' Law.

rc) Bohr's Model.

92. Based on the Third Law of Thermodynamics we know that all per-

fect crystals at absolute zero have:

(A) the same enthalpy. (D) the same crystal lattices.

(B) differing b.A values. (E) two of the above, (A)

and (C).

(C) the same entropy.

93. The vibrational degrees of freedom for a linear and a nonlinear

polyatomic molecule of seven atoms each, are respectively:

(A) 30and 32. CD) 30 and 29.

(B) 29 and 30. (E) none of the above

(C) 28 and 29.

94. Which of the following graphs best represents the Maxwell distri-

bution of molecular speeds and its dependence on temperature?

122

0-~~j.j

j.j

::II,)

> ' 1 , ). . ,0

-

-i'lj_ ,Q)

.0 il.l1: 1 a .~ til

; : . " ' ". . . . . 0

0 speed

0-c :- "-1

1. 1highj

>.utemperatu:r;Ju

.....

.....tI ,. ... ., Q ) I

~ 8 . '~m1) !

::..~I

speed

tr>s : :."j.j

E. 1 .1 high:l

; . . g~ 0

-i'lj

--I Q)

.:; Q)

~ a ..:: !J]

:~. : . . . 0

speeGl

Based on the CO)

statement from a

(A) heavier. mel

protons the

(B) a stable mneven with t

(e) unstable n~

stable confi

(D) usually ligll

and protom



(Bl

temperature'

o s p e ed

(D)

high

temperature

low

temperature

o

s;;oj

H

E) ~ high

~8 temperature. ;.J 0.,-j

.-I'lli

.,-j 4 1; 0 ; 4 1

2~oH'!-'Ip.. 0

s p e ed

Based on the concept of nuclear stability. choose the coreect

statement from among the following:

~(Al heavier. more stable nuclei have somewhat larger numbers of

protons than neutrons.

(B) a stable nucleus cannot have its configuration transformed

even with the addition of energy from the outside.

(el unstable nuclei do not spontaneouslyahange to nuclei with

stable configllrations.

(D) usually lighter stable nuclei have equal numbers of neutrons

and protons.

123



(E) nuclei cal) never have an equal number of protons and

neutrons.

96. The energy of a molecule between'two phases is intermediate be-

tween that of the bee molecule and that of the molecule in the

bulk. Its potential energy would be reduced if itis moved into

the bulk thus, molecules are under the influence of a force which

tends to draw them into the bulk, This force is called the:

(A) flux. (D) surface tension.

(B) adhesive force. (E) none of the above

(C) fugacity.

97. The formula below represents a member of the class of compounds

which are known as:

(A) steroids (D) soaps

I

(B) carbohydrates (E) acids

(C) vitamins

98. The expression for W, in the First Law of Thermodynamics , if

negative, implies all of the following, except: .

(A) work has been done by the system.

(B) the total internal energy has decreased.

(C) a negative amount of work has been done on the system.

(D) the system has lost heat.

(E/ work has been done on the outside world.

99, Asmall sample of some compound is heated with a piece of sodiummetal until the sodium melts , Alcohol, aqueous acid and later

silver nitrate solution are added and a silver precipitate appears .

The ori ginalcompound must contain:

124

CA) an epexidj

eBl an aldehy]

(e) a halogen,

A rem gas ,d U

the ideal gas laWaals equationthis equation.

CA) p ~ (V - 1 1

(B) [ p + ; 2 J

(C) (p - b) ( V

(D) p ; ; : : nRT/~

(E) pV = (nR,]

Which of the foi

J H

rn~

H



(A) an epoxide.

(B) an aldehyde.

(e) a halogen.

(D) an alkali metal.

(E) a phen.ol.

A :real gas ,due to its intermolecular interactions, does not obey

the ideal gas law. Instead its behavior is described by the Van der

Waals equation of state. Choose the letter that correctly shows

this equation.

(A) p = (V - nb) /(nRT) - an zlv 2

(B) ( p + ;2] (V - nb) = nRT

(e) (p - b ) ( V - a ; n = nRT

(D) p : ; : : nRT l(an'l) - V + rib

(EJ pV = (nRT - b) lan2

_1. WRichof the following pairs are anomeric?

IH

HO

OH

HH

n F lO-· c-

H8. (.1H

°OH

CHzOH

0H$CH2~

OH H I

H H 0

n - ~ ~ H I

125



(A) I only

(B) II and III

(C) I. II and

H HO

OH H The sepa!l!atio

ratio of tne:

CHzOHH OR

CA) retention

I V

~" o ~ r : liOR H (B) distribl.i1

OH R

OH HOR H eC) resolutio

°H OH CHzOH

The Schrodin

(A) the polai

(A) I. III and IV (D) I and IV (B) the ener

(B) IIonly (E) I and III(e) the magI

(0) I only

102. For the reaction below: Relaxation m e

CaCOa(g) + CaO(s) + COz(g)

when taking place at a high temperature the following is true:

(A) reaction

(B) fast rea4

(A) lIH<O,LlG_::_O and L IS >0

(B) LlH~O, lIG < 0 and LIS < 0

, (C) liS >0, lIa< ° and lIH :> 0

CD) lIG~O, L i l i >0 and LIS > 0

(E) liS < 0, lIH > 0 and lIG < 0

(e) equilihri

The Bohr thE

whieh of the

I. the eleeellipties

II. the orb

103. Nuclear magnetic resonance (nmr ) spectroscopy js characterized

by which of the folloWing feature( s)?III . transi til

I chemical shift III minimal sensitivity to waterIV. the free

II Rayleigh scattering IV the ability to analyze caf-

feine samples

126



(A) I only

(8) II and III

(e) I. II and IV

(D) I J n, III and iv

(E) I and IV

The separ'ation factor (s or 0.) for a specific column is equal to the

ratio of the:

(B) distribution coefficients.

(D) eddy diffusions.

(E) two of the above

(A) retention times.

(C) resolutions.

The Schrodinger equation when solved for any system gives:

(A) the polarizability.(D) the mean free path.

(B) the energy fluctuation. (E) the wave function.

(C) the magnetogyric ratio.

Relaxation methods are crucial for the study of:

(A) r~E\ctionkinetics.(D) slow r,eactions.

(B) fast l'eactions.(E) rate theory.

(e) equilibrium constants ..

, .

The Bohr theory for "hydrogenlike" atoms consists (in part). of

which of the following postulate(s)?

1. the electron moves around the nucleus of charge +Ze in an

elliptical orbit.·

II. the orbit has constant energy.

III. transitions between orbits generate .spectral lines .

.IV. the frequency of the spectral lines is given by hI {\.E.

127



(A) I, II and III CD) II only

(E) IV onlyB) I and IV

(C) tr and III

108. Aldehydes and ketones exist in solution as an equilibrium mixture

of two isomeric forms. These two forms are:

I. keto form III. enol form

II. aldol form IV. iso form

(A) I and IV (D) I and III

(B) II and III (E) none of the preceedingcombinations

(C) U and IV

l09.Displacement reactions that proceed by the SN2 mechanism aremost successful with compounds that are:

(A) secondary halides with branches at C-2.

(B) neopen tyl system

(C) primary compounds with no branches at the S -carbon.

(D) tertiary compounds with no branches at the S -carbon.

(E) primary halides WIth branches at the c+carbon,

110~ The alkylation of malonic esters with a, JJ -dibromides is a genera;method for the synthesis of:

(A) acetoacetic esters. (D) five-carbon rings

(B) straight chain carboxylic

acids(E) dials

(e) ketones

111. For a homologous series (n-hexane, n-heptane, n-octane and n-nonane), select the graph that appropriately represents the rela:-

tionship between the number of carbon atoms and the logarithm c;

the retention volurne (VR).

128

(D)

-

#

A sample of amme

tube as shown.

( a) C ol l ec ti on G

be e n co ll e ct e d,

p re ss ure s ins ide

collected.

The ammoniumnit

tion. NHttN02(s)

will be collected Iiwater and gas tell

pressure of wa1ie



(B)

f c arbo n at oms carbon at oms

(D) (E)

# carbon at oms

(e)

~ ~ - - - - - - - - ~ - - - -IJlor-l

# c arbo n at oms

# carbon at oms

A sampJe of ammonium nitrite weighing 6.36g is heated in a test

tube as shown.

(a)

Gas vol ume

measurement

(b)

(a~ Collection of a gas over wat er. (b) When the gas has

be en coll ect e d, the bot t le is rais ed or. lClwered to equaliz e

p Ee s s ure s inside and out s ide be fore measuring vol ume of gas

collected.

The ammonium nitrite decomposes according to the following reac-

tion. NHItN02(s) -+ N2(g) + 2H20(g). What total volume of N2

will be cellected in the beaker? (Barometric pressure is 750minHg.water and gas temperature are 26,oe. MWNHItNQz= 64.0 and vapor

pressure of water at 26De = 25mmHg.)

129



5.36 :(760) (299)(0 0821)64.0 (750 - 25) .

(5.361(760V 299 1l64.0j l725)lo.0821)

( A ) .5 .3 6( 7 50 ) (299)64.0

5.36(725)(B) (0.0821)(64.0)(299)

(D)

(E)

5.36(750 - 25),

(e) 64.0(:299)(0.0821)

113. In order to successfully achieve a difficult gas-liquid chromato-

graphic (OLe) separation, which one of the following gases would

be the best to use as a .carrier gas? .

(D) nitrogenA) hydrogen

(B) helium (E) argon

(e) carbon dioxide

.114. Arrange the following compounds in order of decreasing boiling

points.

(A) eH~--C-CH!

~

(B) eHa--CH-CHs

b H

(e) / , 0

CH3-GHrD. ~H

(A) B > E >A>e>F>D

(B) E > B > A > e > D > F

(e) A > B > E > F > e > D

(E) - /0eHa--CHz--C

~OH

CH3-'O-CHal f )

(D)

(E)

E>A>B>e>F>D

B>A>e>E>D>F

115. If one measures the gradient of the e. m. f. of a cell with respect

to temperature the end result will be a value for

(A) fj Hof the cell reaction. (D) the heat of the cell reaction.

(B) 1 1 S of the cell reaction. (E) 1 1 Gof the cell reaction.

(e) Q of the cell.

130

The kinetic usumptions e x e

(A) a gas C O !

motion.

(8) gas pari!

(C)at high

(D) gas par1

(E) none of

7. What type of

central atom

(A) Sp2 hyli

(B)

(C) sps hy

(D)

(E) Spl hy1:

18. Tke possible

for polyatomi

erate', that ii

(A) occur 9!

(B) occur 8!

cy.

(e) decreas

U9. The number

has is:

(A) 26

(B) 24

(C) 12



_6. The kinetic theory of gases is based on all of the following as-

sumptions except:

(A) a gas consists of many particles of mass m, in continual

motion.

(B) 'gas particles have negligible size,

(0) at high pressures gas particles are difficult. to compress.

(D) .gas particles interact only by undergoing elastic collisions,


....... What type' of orbital hybridization and geometry is used by the

central atom of NH 2-?

(A) sp 2 hybridization and trigonal planar.

(B) sp 2 hybridization and tetrahedral geometry.

(0) sps hybridization and trigonai planar.

CD ) sp hybridization and linear geometry.

(E) sp 3 hybridization and tetrahedral geometry •

...~8. 'l'he possible number of infrared absorption bands is very large

for polyatomic molecules. Many of these vibrations are degen-

erate, that is, they:

fA) occur as overtones. (D) fluctuate periodic81ly.

(B) occur at the same frequen- (E) occur at i the wavelengthcy. of the fundamental node.

(C) decrease over time.

:19. The' number of stereoisomers that D-glucose (a six carbon sugar)

has is:

(A) 26

(B) 24

(e) 12

CD) 16

(E) 8

131



120.

" 1ot C H z -tn"n LH - - eft'

k +Bre ~iH z - fH - C H =C H z

H Br

C H - CH = C H - C HI 2 I zH Br

Based on the above diagram one can conclude that:

(A) 1,2 addition is most likely to occur at a low' temperature.

(B) 1,4 addition is most likely to take place at a low temperature

,(C) 1,2 addition is favored by a hi gh temperature.

(D) 1,2 addition and 1,4 addition are equaIly likely to occur atany given temperature.


121. A perpetual motion machine capable of generating increasing

amounts of energy without interacting with its surroundings can-not exist. This is best explained by the

(A) First Law ofThermodynamics.

(B) Third Law of Thermodynamics.

(C) Energy Conservation Principle.

(D) Gibbs-Helmholtz, equation.

(E) Second Law of Thermodynamics .

122. C7H7N02 has infrared absorption peaks at 6.5 and 7,.5 (microns

On the other hand , it has no peaks between 5.7 and 6. 0 ~ •it is vigorously oxidized with permanganate solution, the produc:-

is 'benzoic acid. The structure of this organic compound is onemore of the foUowing:

1 3 2

I

II

(A) II

(B) I

(c) I

_3. In theexpan

area(s

(A)

(B)

e e l no



OR

I ~ O Hc~ N

II

© O ,

(A) II only

(B) I and II

(e) III only

III

eHO

IV.~

N . O H

(D) I. II and IV

(E) II and III

. .

123. In the diagram shown. the reversible isothermal work ofexpansipn done on the system is represented by which

area(s)?

V·l

Volume

(A) ~ area only

(B) I I I I I I area only

(D) & d and 1 1 1 1 1 1 areas


(C) no work is done

1 3 3



124. Whichone of the following represents the behavior of Helmholtzfree energy (A), under constant volume and temperature condi-

tions, for spontaneous, non-spontaneous or equilibrium situa-tions?

S-pontaneous EquilibriumProcess

(A) + +

(B) 0

(C) 0

(D) 0 +

(E) + 0

Non-spontaneousProcess

+

o

125. The height equivalent of a theoretical plate (HETP) has all of thefollowing eharacteriatics except for:

(A) itis defined by the van Deemter equation.

(B) it describes a certain length of chromatographic column.

(C) the smaller; this value is, the better the separation attainable

(D) the inverse of this quantity times the total column length isequal to the number of theoretical plates in the column.

(E) equilibrium is attained at each height equivalent.

126 .In a 7.35 Q , tank, at 27°G, the pressure of nitrogen gas is 2300

lblin 2. What volume would the. gas in this "tank occupy at 1 atm.

(or 14.7 Ib/in2) pressure?

(A) 4600 Q ,

(B) 460· 9 ."

(C) 115 9,

(D) 230£

(E) 1150£

127. The basic data of chemical kine:tics aee the concentrations of the

reactants and products as a function of time. There are severalmethods available for monitoring the concentrations of reactants

and products. Of the methods listed. below select the one that isnot used.

134

CA ) Thermal

(B) Recording

(Cl Measureml

CD) Periodic tl

analysis

(.E) Monitorinj

In examinin g tl

motion of the nconsider the ml

static nuclear 1

the

(A) Borrr-Opp

(B) Euler's c1

(C) Hittorf m e

(D) Iindemam

(E)

Liquid-membraJ

held between t

to separate th

greater tenden

interface the f c

as it proceeds

(Al EExt:::: k~

(D) EExt:::: k



(A) Thermal analysis

(B) Recording of the pressure.as a function of time

(C} Measurement of the angle of optical rotation

(D) Periodic bleeding of the reaction mixture fo!, chromatographic

analysis

(E) Monitoring of the conductivity of a solution .

......8. In examining the structure of molecules it was discovered that the

motion of the nuclei could be negleeted and. it was sllfficient to

cONsider the motion and distribution of the electrons alone for

static nuclear position purposes. This ass~mption was based on

the

(A) Born-Oppenheimer approximation.

(BJ Euler's chain relation.

(e) Hittorf met.hod ,

(D) Lindemann mechanism.

(E) Kraichman's, equations.

9. Liquid-membrme electrodes contain a liquid exchanger which isheld between two porous glass (or plastic) membranes. It serves

to separate the test solution from the internal solution and has a

greater tendency to bond calcium than any; other ion. At each

interface the following reaction occurs:

Ca2+(aq) + Ex2 - :: CaEx

as it proceeds a potential develQPs. This potential is equal to:

k' 0.05.91

(~)aq(A)EExt;: 1- -1- og ( )

a1Ext

O 59(al)

(B) E = k +....JL_ log ExtExt 2 2 (a

2)Ext

.. ' (av .

(

el E = k + 0.05.91 Ext

Ext . 2 1 og (a )1aq

O 09 (al)

(D) E = kl + •. 5 10' . a9Ext ~ g (al)Ex!

1 3 5



(al) ,

'" k~ - O . 20,59og 'ag(E) EExt ~az)Ext

130. The average osmotic pressure 'IT, of blood is 12.3 atm at 27°C.

What oonoent ration of glucose, C6H1206, will be isotonic with

blood?

(A) 2.0M

(B) 0'.5M

(C) 1.OM

(D) 0.025M

(E) 1.5M

131. 6. Hf

. of NOCl( g) from the gaseous elements:ormation

tN2(g) + !Oz(g) + tC12(g) '" NOCl(g)

is equal to 12.6 kcal/mole at 25°G. Assuming the gases are ideal,6. E would equal which one of the following? (1kcal = 4.184 kJ)

(A) 12.6 kJ (D) 74,220J

(B) 46,300 J (E) insufficient information

given to find tEo .

(C) 53.8 kJ

132. Assuming that the energy of an electron is quantized, which of

the following statements is not true?

,(A) The centrifugal force created by the electron's motion about

the nucleus is counterbalanced by the electrostatic attraction

between the nucleus and the elect.ron ,

(B) The radius (R) of an electron's orbit about the nucleus is

equal to R = n 2 a o /z, (where z = atomic number, ao = size of

the orbit and n = quantum number).

(C) If the principal quantum number (n ) of an electron is known,

only the size of its orbit and the energy of the electron can

be calculated.

(D) As the principal quantum number increases, the difference iI:.

energy between the levels decreases.

(E) The energy (,E) of an electron in a 'hydrogenlike' ion is

equal to E = -kz'2/nZ (z = atomic number, k = a constant and

n = quantum number).

136

All of the follC

existence of h

CA) the parti

(8) ccllieions

(e) there arE

such a g,

(D) the avers

proportic

(E) the gas I

A sample of ir

by a chemist

x : : : : 10.5:

The Bureau'sresults differ

needed. )

N t

bel' of de

servatrons ,

n

(A) not by m

(B) signiflcru

(e) can't be



.1.3. All of the fQUowingassumptions would be in agreement with the

existence of ideal gases I except one , which is:

(A) the par-ticles of such a gas are in random motion.

(8) collisions between the gas particles are elastic.

(C) there are no mutual interactions between the particles of

such a gas.

(D) the average tr-analatlonal.Jdnetfc energy of the particles is

proportional to the absolute temperature.

(E) the gas particles have zero volume. ,

_ -4 . . A sample of iron ore from the Bureau of Standards was analyzed

by a chemist and the following results were obtained:

x = 10.53 (%iron), s '" 0.05. n = 10.

The Bureau's value for this sample is 10.61'%iron. Howdo theseresults differ at a 95%probability level? (Use the table below as

needed. )

Some Values of Student's t

Number of

umber of degrees of Probability

-servations, fr-eedom , levels

n n - 1 50% 90% 95% 99%

2 1 1.000 6.314 12.706 63.66

3, 2 o.sie 2.920 4.303 9.925

4 3 0.765 2.353 3.182 5.8415 4 0.741 2.132 2.776 4.604

6 5 0.727 2.015 2.571 4.032

7 6 0.718 1.~43 2.447, 3.707

8 7 0.711 ' 1.895 2.365 3.500

9 8 0.706 1.860 2.306 3.355

10 9 0.703 ~.833 2.262 3.250

11 10 0.,700 1.812 2.228 3.169

21 20 0.687 1.725 2.086 2.845

'"00 0.674 1.645 1.960 2.576

(A) not by much (D) not by much , but still can't

be used(B) significantly

can't be determined

(E) results vary, but are still

(C) within the range of use

137



135. 2. 4 liter of HN03 solution reacts with 63 ml of 1. 9NEa(OH)2 to pro-

duce a neutral solution. Whatis the molarity (M) of the original

HNO3 solution?

(A)63( 1.9) M

CD)63(1.9)

1000(2.4) lOOfl(2)(2.4) M

(E}63( 1.9)

(E)63(1.9)

1000 M 100(2.4) M

(e)2(63)(1. 9)

1000 M

136. Kirchhoffts Law is applicable to a system when:

(A) the temperature is a constant.

(B) all the heat capacities are known in the range being exam-

ined.

(C) the heat capacity is measured at constant volume.

(D) only certain specific species are present.

(E) one assumes that all the heat capacity values are independent

of temperature.

137. The charge on an electron was determined by measurement of the

effect of arr electric field on the. rate at which charged oil droplets

fell under the influence of gravity. This discovery was made by

(A). J,J. Thomson. (D) H. Becquerel.

(E) E. Rutherford. (E) W.C. Roentgen.

(C) R. Millikan

\

138. The van der Waals equation of state has two constant terms (a

and b), that are not present in the combined gas law. The follow-

ing is true' of the terms 'a' and 'b":

(A) 'b' cor-rects for 'the intermolecular forces of interaction and

'a' for the included volurne of the molecules.

(B) 'a' corrects for the exterrial pressure of the gas and 'b' forthe internal pressure of the ,gas.

(C) 'a' corrects for the force of intermolecular interaction and

'b' for the excluded' volume of the molecules .

138

(D) 'b) carre

repulsio

fE) none of 1

Living tissues

tion of the fIualmost constan

the many buf:liseveral of the

inthe blood.

(A) proteins

(B) hemogloti

(C) chlorides

Whicn of the ~

metal? i

(A) Bismuth

fB) Lead

(C) Tin

All of the folIo

(A) itis a me

(B) the natuf

(C) it is not.

(D) it can be

(E) h o S = 0 fo

Volumetric glasto maintain its

below are way

(A) direct. ab

(B} relative Cl



(D) 'b' corrects for the free volume and 'at for tne intermoleculiarrepulsion between molecules.

.(E) none of the above

9. LiviAg tissues are very sensitive to any changes in the composi-

tion of the fluids that bathe them. Thus, the maintenan'ce of analmost constant pH in the blood is necessary and is achieved bythe many buffers present in that body fluid. Listed below,areseveral of these buffers. choose the one(s) which are not active

in the blood.

(A) proteins

(B) hemoglobin

(C) chlorides

(D) phosphates


Whichof the following elements is not a component of Wood's

metal?

(A) Bismuth (D) Titanium

(B) Lead

(e) Tin

(E) Cadmium

All of the following statements about llS are true except for:

(A) it is a measure of the energy dispersal.

(NJ the natural tendency is fQr it to increase;

(e) it is not a state function.

(D) it can be defined both thermodynamically and statistichlly.

(E) tl.S= 0 for a reversible process.

Volumetric glassware needs to be calibrated periodically in order

to maintain its precision, and accuracy. All of the methods lis.ted

below are ways of calibrating this glassware except for:

(Al direct. absolute calibration

(B) relative calibration

139



(C) complex calibration

(D) calibration by comparison


143. The nucleophilic aromatic aubati tution that can occur on a benzenering is affected by the substituent group(s) present , Which one

of the following statements correctly describes such a substituent

group and its effects.

(A) -eN, electron withdrawing, deatabi llz.es carbaniori

(B) -eOOR, electron releasing. activates the ring

(e) ~N02, stabilizes carbanion, acti vates the ring

(D) -R, des tabifiz.es carbanion , electron withdrawing

(E)' -CRO, deactivates the ring, destabilizes carbanion

144. The strongly repulsive interaction that takes place when an C\

particle closely approaches a gold nucleus is best' explained by:

(A) Dalton's theory. (D) Gauss's law.

(B) Marsden's rule. (E) Coulomb's law.

(e) Thomson's model.

145. All of the following equations are Maxwell's relations, with one

exception. Indicate the letter of the equation that does not desi~-

nate a correct Maxwell reation.

(A) (8TI8V)s = -(8P/8S)V

(B) (8P/8:T)V'" (dS/8V)T

(e) (3V/8T)p=-(8SI8P)" T

(D)

(E)

(8T / dP ) S = (8V / as ) P

(8 S /c)P)v = -(d T laV)p

146. For a sodium ion selective electrode all of the following statementsare true except:

(A) the boundary potential depends upon the activities of botb

sodium and hydrogen ions.

14;0

(E) the electroo

(e) the potentia

(D) the selectiv:

exchange Si

(E) the sodium

fusion potel

What is the right

(A) ts22s22p63g2

(E) ls22s22p6 3s:

(e) 1s22823s 22p6

The Clapeyron' e(

condensed phase,

applies to phase

(A) twe condens

(B) twocondens

(C) a liquid pha

(D) a gas phase

(E) none of the

Of the many chen

sary requirement

Whi(!h one of the

!'eaction to be USE

CA) The reaction

(B) The equilibn

(C) The reaction

equation.

(D) The reaction

is readily ob



(B) the electrode is specific for sodium ions.

(C) the potential is largely a function of the sodium ion activity.

(D) the selectivity of the glass electrode is related to the cation-

exchange selectivity of the glass surface.

(E) the sodium ions can penetrate the gel and influence the dif-

f,usion potential.

What·is the right configuration of an element with 24 electrons?

(A) Is22sz2p63s23p63d6

(B) ls22s22p63s23p64s2 3d.4

(C) lS22s23s2.2p63 p64s14ps

(D) 1~2s22p63~3p64s13d5

(E) ls22s23if2p63p64s23d4

The Clapeyron equation applies to a phase change involving only

condensed phases. However, the Clausius-Claypeyron equation

applies to phase transitions between:

(A) two condensed phases at different temperatures only.

(8) two condensed phases at different pressures only.

(C) a liquid phase and a gas phase.

(D) a gas phase and any condensed phase.


.3. Of the many chemical reactions known. only a few meet the neces-

sary requirements in order to be used in trdtation processes.

Which one of the requirements listed below is not necessary for a

reaction to be used in ritrtmetrie analysis?

(A) The reaction can have no side reactions ,

(EI) The equtlibri um constant of the reaction must be very large.

(C) The reaction should proceed according to a definite chemical

equation.

(D) The reaction should proceed very slowly so that the endpoint

is readily observable.

141



(E) Someinstrumental method should be available to tell the an-

alyst when to stop the addition of titrant.

150. In laboratory work. when small quantities of hydrogen are re-qulred , the following method is most often used to prepare it:

(A) the reaction of certain acid solutions Withmetals .

. (B) the liquidation and subseq uent distillation 'of air.

(C) the pyrolization of specific inorganic compounds.

(D) the passing of steam over hot coke.

(E) the reaction of metallic oxides with water.

THE G

AMINAl i

1. D

2 '. E

3 . A

4 . C

5. E

6 . E

7 . E

8 . E

9. D

10. E

11. B

1 2 . D

1 3 . A

H. B

1 5 . 0

16. D

17., B

1 8 . A

19. D

1 4 2



THE GRADUATE REGORD

XAMINATI 'ON CHEM IS TRY TE ST

· 1 MODEL TEST II IANSWERS

l. D 20. B 39. A

2 . E 21 . C 40. C _,

3. A 2 2 . D 41 - E

4. , C 23. E 42. A

5. E 24. A 43 . E

6. E 25 . C 4 4 . D

7. E 26. B 45 . C

8. E 27 . C 4 6 . E

9. D 28 . D 47. C

10. E 29. D 48 . E

1 1 . B 30. ·B 49. B

12. D 31. B 50•. B

13. A 32. E 51. E

14•. B 33. C 52. .: 6

15. D 34. B 53. B

16. D 35. B 54. A

1 7 . B 36. E 55. B

1 8 . A 37. B 56. C

19. D 38. D 57. B

143



58. B 89. D 120. A THE·GJ59. A .90. A 121. A

60. D 91. D 122. A

61. B 92. e 123. D

~

62. A 93. E 124. B

63. E 94. e 125. E

64. E 95. D 126. E

65. c 96. D 127. A

66. D 97. D 128. A DETAil67. A 98. D 129. D

68. e 99. e 130. B

69,. D 100. J 3 131. e

70. B 101. D 132. c7 1 . E 102. e 133. E

72. D 103. E 134. B1. (D)

73. A 104. E 135. A For an ideal soh

74. E 105. E 136. B

75. A 106. B 137. e

76. B 107. C 138. eL IS

77. B 108. D 139. e mi

78. B 109. c 140. D and lIG .

79. E 110. D 141. e m l

80. D 111. A 142. e

81. A 112. D 143. C

82. E 113. D 144. E

83. B 114. B 145. E 2 . (E)

Aromatic

84. A 115. B 146. B substitution

85. c 116. C 147. Dreaction of t

conditions. For

86. B 117. E 148. D all unsubstituted

87. D 118. B 149. D

88. e 119. D 150. A

gre chemistry3

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