CHEM%1310% Sample%Final%Exam% 1.%Antimony,%Sb,%has%two%stable%isotopes.%Given%that%43.8%%of%natural%antimony%is%

CHEM%1310%
Sample%Final%Exam%
1.%Antimony,%Sb,%has%two%stable%isotopes.%Given%that%43.8%%of%natural%antimony%is%
123Sb%with%the%experimentally%determined%mass%122.904%amu,%what%is%the%other%
stable%isotope?%
%
%
%
A)%120Sb%
%
B)%121Sb%
%
C)%122Sb%
%
D)%123Sb%
%
E)%124Sb%
%
2.%%What%is%the%chemical%formula%for%the%compound%containing%the%iron(III)%cation%
and%the%sulfate%anion?%
%
%
A)%Fe3SO4%
%
B)%FeS%
%
C)%Fe3(SO4)2%
%
D)%Fe2(SO4)3%
%
E)%Fe2S3%
%
3.%%A%given%isotope%contains%92%protons,%146%neutrons,%and%86%electrons.%%What%is%the%
chemical%symbol%for%this%isotope?%
%
6+
%
A)% 238
92 U %
%
B)% 146
92 U %
178
%
C)% 86 Rn %
6+
%€
D)% 238
86 Rn %
%€
E)% 146 U 6+ %
%€
4.%%A%laboratory%analysis%of%an%unknown%solid%determined%the%following%mass%
€
percent%composition:%
€
%
Ca%=%54.09%%
%
H%=%2.72%%
%
O%=%43.19%%
%
What%is%the%empirical%formula%for%the%solid?%
%
%
A)%Ca(OH)2%
%
B)%Ca27O22H%
%
C)%CaOH%
%
D)%Ca0.337O0.675H0.668%
%
E)%Ca4(OH)8%
%
%
%
CHEM%1310%
Sample%Final%Exam%
%
5.%What%is%the%formula%of%the%organic%molecule%below?%
%
%
%
%
A)%C3H6O3%
%
B)%C3H2O3%
%
C)%CH2O%
%
D)%C3H3O6%
%
E)%CHO2%
%
%
6.%%What%is%the%solid%produced%when%K3PO4%reacts%with%Ca(NO3)2?%
%
%
A)%KNO3%
%
B)%Ca3(PO4)2%
%
C)%Ca2+%
%
D)%NO3\%
%
E)%K%
%
%
7.%%How%many%moles%of%carbon%are%there%in%650.5%grams%of%glucose,%C6H12O6?%
%
%
A)%2.17%x%1024%
%
B)%3.61%
%
C)%0.277%
%
D)%21.7%
%
E)%1.30%x%1025%
%
8.%Five%liters%(5.00\L)%of%an%aqueous%solution%is%prepared%by%complete%dissolution%of%
40.00%g%of%FeCl2%.%What%is%the%chloride%ion%(Cl%\)%concentration%of%this%solution?%The%
molar%mass%of%FeCl2%is%126.75%g/mol.%
%
%
A)%0.0631%M"
%
B)%0.0315%M"
%
C)%0.0876%M"
%
E)%0.0438%M"
%
E)%0.126%M"
CHEM%1310%
Sample%Final%Exam%
9.%%How%much%C2H2%can%be%produced%when%100.%g%of%H2O%reacts%with%100.g%of%CaC2%
according%to%the%reaction%below?%
CaC2(s)%+%2H2O(l)%%%%Ca(OH)2(aq)%+%C2H2(g)%
%
%
A)%72.25%g%
%
B)%40.62%g%
%
C)%144.5%g%
%
D)%31.63%g%
%
E)%112.9%g%
%
10.%%If%the%percent%yield%of%the%reaction%is%74.2%%when%24.0%g%of%NaHCO3%is%heated,%
then%how%much%Na2CO3%is%formed?%
Molar%masses:%%NaHCO3%=%84.01%g/mol;%Na2CO3%=%105.99%g/mol;%CO2%=%44.01%g/mol;%
H2O%=%18.01%g/mol%
%
%
A)%15.1%g%
%
B)%11.2%g%
%
C)%22.3%g%
%
D)%26.4%g%
%
E)%30.3%g%
%
11.%What%is%the%partial%pressure%of%CO%in%a%container%that%holds%5.0%moles%CO(g),%3.0%
moles%of%N2(g),%and%1.0%mole%of%H2(g)%and%has%a%total%pressure%of%1.05%atm?%
%
%
%
A)%0.42%atm%
%
B)%0.53%atm%
%
C)%0.58%atm%
%
D)%0.47%atm%
%
E)%There%is%not%enough%information%to%answer%this%question.%
%
12.%An%ideal%gas%differs%from%a%real%gas%in%that%the%molecules%of%an%ideal%gas_________.%
%
%
A)%have%an%average%molecular%mass.%
%
B)%have%no%kinetic%energy.%
%
C)%have%a%molecular%weight%of%zero.%
%
D)%have%no%attraction%for%one%another.%
%
E)%take%up%a%significant%amount%of%volume%in%comparison%to%the%volume%of%the%
%
sample.%
CHEM%1310%
Sample%Final%Exam%
13.%The%graph%below%represents%the%gases%He,%Ar,%N2,%and%CH4%all%at%the%same%
temperature.%%Which%statement%regarding%this%graph%is%true?%
%
%
A)%Curve%3%represents%N2.%
B)%Curve%1%represents%N2%
C)%Curve%4%represents%Ar.%
D)%Curve%2%represents%He.%
E)%Curve%3%represents%CH4.%
%
%
14.%A%newly%discovered%substance%in%the%gas%phase%has%density%of%2.39%g/L%at%25.0oC%
and%0.941%atm.%%What%is%the%molar%mass%of%the%substance?%
%
%
A)%16.1%g/mol%
%
B)%62.1%g/mol%
%
C)%5.21%g/mol%
%
D)%0.0919%g/mol%
%
E)%This%problem%cannot%be%solved%without%the%volume%of%sample.%
%
%
15.%What%mass%of%P4(s)%is%required%to%completely%consume%25.0%L%of%H2(g)%at%27.0oC%
and%0.976%atm%in%the%presence%of%excess%oxygen?%The%molar%mass%of%P4%is%%%%%%%%%%%%%%
123.88%g/mol.%%The%molar%mass%of%H2%is%2.02%g/mol.%
%
P4(s)%+%6H2(g)%+%8O2(g)%%%%4H3PO4(s)%
%
%
A)%0.202%g%
%
B)%20.5%g%
%
C)%1.21%g%
%
D)%123%g%
%
E)%246%g%
%
%
%
%
CHEM%1310%
Sample%Final%Exam%
16.%How%many%unpaired%electrons%are%in%a%ground%state%vanadium%(V)%atom?%
%
A)%0%%%%%%%%%%%
%
B)%1%%%%%%%%%%%
%
C)%3%%%%%%%%%%%
%
D)%4%%%%%%%%%%%
%
E)%5%
%
17.%Which%of%the%following%has%the%largest%atomic%or%ionic%radius?%
%
%
A)%S2\%%%%%
%
B)%Cl%%%%%%
%
C)%Cl\%
%
D)%K+%%%%%%
E)%S%
%
18.%Which%set%of%quantum%numbers%could%correspond%to%a%4d\orbital?%
%
%
A)%
n%=%4,%l%=%4,%ml%=%+3%%
%
B)%
n%=%4,%l%=%2,%ml%=%+4%%
%
n%=%4,%l%=%3,%ml%=%−3%%
C)%
%
D)%
n%=%4,%l%=%2,%ml%=%+1%%
%
%
%
19.%For%a%hydrogen%atom,%which%transition%correlates%to%the%longest%wavelength%of%
light%absorbed?%
%
%
A)%n%=%1%to%n%=%2%
%
B)%n%=%3%to%n%=%4%
%
C)%n%=%1%to%n%=%3%
%
D)%n%=%2%to%n%=%5%
%
E)%n%=%2%to%n%=%3%
%
20.%%A%0.500%Joule%laser%pulse%with%780.0%nm%wavelength%contains%how%many%
photons?%
%
%
A)%1.96%x%1018%photons%
%
B)%2.55%x%10\19%photons%
%
C)%9.67%x%1038%photons%
%
D)%1.96%x%1027%photons%
%
E)%1.27%x%10\19%photons%
%
%
%
%
CHEM%1310%
Sample%Final%Exam%
21.%How many lone pairs of electrons are found on the central atom in the Lewis
structure of the compound ICl3?
A) 2
B) 3
C) 4
D) 8
E) 11
22. The%hybrid%orbitals%used%in%carbons%2%and%4,%respectively,%in%the%molecule%below%
are:%
%
%
%
A)%
B)%
C)%
D)%
E)%
sp3%and%sp%%
sp2%and%sp%%
sp3%and%sp3%%
sp2%and%s2%%
spd"and%sp%%
%
%
%
23.%Which%bond%is%the%most%polar?%
%
%
A)%C—H%%
%
B)%C—C%
%
C)%C—S%
%
D)%C—O%
%
E)%C—N%
%
24.%What%is%the%electron%group%arrangement%(electron%geometry)%of%AsF3?%
%
A)%tetrahedral%
B)%trigonal%planar%
C)%trigonal%pyramidal%
D)%bent%(V\shaped%or%angular)%
%
E)%trigonal%bipyramidal%
%
%
CHEM%1310%
Sample%Final%Exam%
%
25.%Which%molecule%can%form%intermolecular%hydrogen%bonds%(with%other%molecules%
of%itself)?%%
%
%
A)%NH2CH2COOH%%%%%
%
B)%SiH4%%%%%%
%
C)%CH3COCH3%%%%%
%
D)%CH2F2%%
%
E)%CH3Cl%
%
%
26.%What%is%a%p\type%semi\conductor?%
%
A)%
One%with%excess%electrons%in%the%valence%band%(valence%electron%rich).%%
B)%
One%with%excess%electrons%in%the%conduction%band%(conduction%electron%rich).%%
C)%
One%with%a%less\than\full%valence%band%(valence%electron%deficient).%
D)%
One%with%a%less\than\full%conduction%band%(conduction%electron%deficient).%%
E)%
One%with%electrons%positively%in%the%conduction%band%(conduction%positive%electrons).%%
%
%
27.%Which%statement%regarding%the%image%is%true?%
%
%
%
A)%It%is%a%body%centered%cubic%unit%cell,%and%there%are%9%atoms%per%cell.%
B)%It%is%a%face%centered%cubic%unit%cell,%and%there%are%2%atoms%per%cell.%
C)%It%is%a%simple%cubic%unit%cell,%and%there%is%one%atom%per%cell.%
D)%It%is%a%body%centered%cubic%unit%cell,%and%there%are%2%atoms%per%cell.%
E)%It%is%a%face%centered%cubic%unit%cell,%and%there%are%two%atoms%per%cell.%
%
%
%
%
%
%
%
28.%Rank%the%boiling%points%from%highest%to%lowest%for:%
CH3OH,%CH3CH3,%CH2O%
%
%
A)%CH3OH%>%CH3CH3%>%CH2O%
%
B)%CH2O%>%CH3OH%>%CH3CH3%
%
C)%CH3CH3%>%CH3OH%>%CH2O%
%
D)%CH3OH%>%CH2O%>%CH3CH3%
%
E)%CH2O%>%CH3CH3%>%CH3OH%
CHEM%1310%
Sample%Final%Exam%
%
29.%When some TNT detonates, the volume of gas increases from 10.0 L to 90.0 L at a
constant pressure of 1.00 atm. Additionally, 90 kJ of energy is released as heat. What is
ΔE for this process? ( 1 L•atm = 101.325 J)
%
%
A)%%\98.1%kJ%%%%%%
%
B)%%−81.9%kJ%%%%%%
%
C)%%−8.1%%kJ%%%%%%
%
D)%%+81.9%kJ%%%%%%
%
E)%%+98.1 kJ%
%
30.%%You%hold%a%gram%of%aluminum%in%one%hand%and%a%gram%of%copper%in%the%other;%
each%started%at%the%same%temperature.%To/from%which%metal%will%more%heat%have%
been%transferred%when%both%have%reached%body%temperature?%Given%Cs,Cu=%0.387%
J/g°C,%dCu=%8.93%g/cm3,%Cs,Al=%0.900%J/g°C,%and%dAl=%2.70%g/cm3.%
%
A)%Copper,%because%it’s%specific%heat%capacity%is%lower%
B)%Copper,%because%it’s%density%is%higher%
C)%Aluminum,%because%it’s%specific%heat%capacity%is%higher%
D)%Aluminum,%because%it’s%density%is%lower%
E)%Copper%and%aluminum%will%reach%body%temperature%at%the%same%time%
%
%
31.%Which%statement%is%true?%
%
%
A)%In%an%endothermic%reaction,%the%energy%of%the%products%is%less%than%that%of%% %
%
%%%%%%the%reactants.%
%
B)%There%is%no%temperature%change%associated%with%the%conversion%of%ice%to%%
%
%%%%%%liquid%water.%
%
C)%Freezing%is%an%endothermic%process.%
%
D)%The%change%in%enthalpy%is%equal%to%q%at%constant%volume.%
%
E)%None%of%these%statements%is%true.%
%
32.%%Which%statement%best%explains%why%water%freezes%only%at%or%below%0oC%at%
atmospheric%pressure.%
%
%
A)%Freezing%is%an%endothermic%process%with%an%increase%in%entropy.%
%
B)%Freezing%is%an%exothermic%process%with%decrease%in%entropy.%
%
C)%The%sign%of%ΔG%for%the%process%is%always%positive.%
%
D)%Freezing%is%an%endothermic%process%with%a%decrease%in%entropy.%
%
E)%Freezing%is%an%exothermic%process%with%an%increase%in%entropy.%
CHEM%1310%
Sample%Final%Exam%
33.%Given:%
%
1. NH3(g)%+%HBr(g)%%NH4Br(s)%
%
2. N2(g)%+%3%H2(g)%%2%NH3(g)% %
%
3. N2(g)%+4%H2(g)%+%Br2(l)%2NH4Br(s)%%
%
%
%
∆H°rxn%=%\188.32%kJ%
∆H°rxn%=%\92.22%kJ%
∆H°rxn%=%\541.66%kJ%
%
Which%steps%are%necessary%to%calculate%the%∆Hrxn%for%this%reaction:%
%
%
H2(g)%+%Br2(l)%%2%HBr(g)%
%
I. Reverse%reaction%1.%
II. Halve%reaction%3.%
III. Double%reaction%1.%
IV. Reverse%reaction%2.%
%
A. I%&%IV%only%
B. II%&%III%only%
C. I%&%III%only%
D. I,%III,%&%IV%only%
E. All%of%these%steps%are%necessary.%
%
%
34. For which reaction or process is the change in entropy greater than zero?
A) NH3(g)%+%HBr(g)%%NH4Br(s)%% %
Β) N2(g)%+%3H2(g)%%2NH3(g)%
%
C) N2(g)%+%4H2(g)%+%Br2(l)%%2NH4Br(s)%
%
D)%H2O(s)%%H2O(g)%
%
E)%Na+(aq)%+%Cl\(aq)%%NaCl(s)%
!
!
35.%Which%of%the%statements%below%is%not%a%direct%consequence%of%a%law%of%
thermodynamics?%
%
%
A)%Entropy%of%the%universe%(system%plus%surroundings)%increases.%
%
B)%Spontaneous%reactions%are%fast.%
%
C)%Total%energy%is%conserved.%
%
D)%The%entropy%of%a%crystalline%solid%approaches%zero%at%0%Kelvin.%
%
E)%All%of%these%are%consequences%of%the%laws%of%thermodynamics.%
%
CHEM%1310%
Sample%Final%Exam%
36.%%Calculate%the%normal%boiling%point%of%CH3CH2OH,%given%the%following%
information:%
%
%
%
∆H°vap%%
%
43.5%kJ/mol%
%
%
∆H°fus%%%
%
4.60%kJ/mol%
%
%
∆H°f% %
%
\278%kJ/mol%
%
%
∆S°vap% %
%
124%J/mol·K%
%
%
∆S°fus% %
31.0%J/mol·K%
%
Molecular%weight% 46.1%g/mol%
%
%
%
%
A)%
159%K%
%
B)%
2240%K%
%
C)%
1.40e3%K%
%
D)%
351%K%
%
E)%
0.351%K%
%
%
37.%%Calculate%ΔGo%at%45.0oC%for%a%reaction%for%which%ΔHo%=%\293%kJ%and%%
ΔSo%=%\69.5%J/K.%
%
%
A)%\271000%kJ%
%
B)%\290%kJ%
%
C)%21800%kJ%
%
D)%\271%kJ%
%
E)%2830%kJ%
%
38.%The rate law for a reaction is: Rate = k[A]2[B]. What happens to the rate if both
concentrations are doubled?
A) No change
B) Rate increases by a factor of 4
C) Rate increases by a factor of 2
D) Rate increases by a factor of 8.
E) Not enough information
39.%The rate law for a particular reaction is Rate = k[A][B]. If the initial concentration of B is
increased from 0.1 M to 0.3 M (while the concentration of A is held constant), the initial rate will
increase by which of the following factors?
A)
B)
C)
D)
E)
2
27
4
6
3
%
%
CHEM%1310%
Sample%Final%Exam%
40. A eneral reaction written as 2A + 2B
C + 2D is studied and yields the following data.
[A]0
[B]0
Initial Δ[C]/Δt
0.100 M
0.200 M
0.100 M
0.100 M
0.100 M
0.200 M
4.00 × 10–5 mol/L • s
4.00 × 10–5 mol/L • s
8.00 × 10–5 mol/L • s
What are the proper units for the rate constant for the reaction?
1/s
M/s
1/M·s
1/M3·s
1/M2·s
%
%
41.%The rate constant, k, for a chemical reaction is dependent on
A) the concentration of the reactant.
B) the concentration of the product.
C) the temperature.
D) enthalpy.
E) none of these
%
%
42.%%A%1.00%atm%sample%of%H2S%is%allowed%to%decompose%at%1405%K%until%equilibrium%is%
achieved.%%At%equilibrium,%the%partial%pressure%of%S2%is%0.0370%atm.%%What%is%the%value%of%K%for%
this%reaction?%
2H2S(g)% %S2(g)%+%2H2(g)%
%
%
A)%2.36x10\4%
%
B)%2.96x10\3%
%
C)%1.42x10\3%
%
D)%4.24x103%
%
E)%7.04x102%
%
%
%
%
%
%
%
%
%
%
%
%
A)
B)
C)
D)
E)
CHEM%1310%
Sample%Final%Exam%
%43.%%Select%the%equilibrium%expression%for%the%reaction:%
%
P4(s)%+%3KOH(aq)%+%3%H2O(l)% %%PH3(aq)%+%3KH2PO2%(aq)%
%
ANS:%E%
A) K =
1
[P4 ][H 2O]3
[KOH]3
B) K =
[PH 3 ][KH 2PO 2 ]3
%
C) K =
[PH 3 ][KH 2PO 2 ]3
[P4 ][KOH]3 [H 2O]3 %
[PH 3 ][KH 2PO 2 ]3
D) K =
[KOH]3 [H 2O]3
[PH 3 ][KH 2PO 2 ]3
E) K =
[KOH]3
%
%
44. An increase in total pressure (at constant temperature) for the following reaction causes:
€
A(g) + B(g)
C(g) + heat
A) increase in the number of moles of A
B) decrease in the number of moles of A
C) no change in the number of moles of A
D) an undetermined effect on the number of moles of A
45. Calculate the [H+] in a 0.020 M solution of HCN, Ka = 6.2 × 10–10.
A) 1.0 × 10–7 M
B) 3.5 × 10–6 M
C) 1.6 × 10–5 M
D) 2.5 × 10–5 M
E) none of these
!
!
%
%
%
%
%
%
%
CHEM%1310%
Sample%Final%Exam%
46.% The%value%of%K%for%the%reaction%N2O4(g)% %2NO2(g)%at%a%given%temperature%is%%0.211.%
If%the%equilibrium%partial%pressure%of%NO2%at%the%same%temperature%is%0.0172%bar,%
then%what%is%the%equilibrium%concentration%of%N2O4?%
%
%
A)%0.0815%
%
B)%0.00664%
%
C)%0.00140%
%
D)%6.24×10–5%
%
E)%0.0602%
%
%
47.%%The%galvanic%cell%shown%below%uses%the%half\cells%Mg2+/Mg%and%Zn2+/Zn,%and%a%
salt%bridge%containing%KCl(aq).%The%voltmeter%gives%a%positive%voltage%reading.%%
Which%statement%correctly%identifies%the%anode%and%cathode%compartments%and%the%
reactions%that%occur%in%them?%
%
%
%
Mg2+(aq)%+%2e\%%%Mg(s)%% %
Eo%=%\2.37%
%
%
%
Zn2+(aq)%+%2e\%%%Zn%(s)%
%
Eo%=%%\0.76%V%
%
%
A)%A%and%E%represent%the%cathode:%Zn2+(aq)%+%2e\%%%Zn%(s)%
B)%B%and%F%represent%the%cathode:%Mg2+(aq)%+%2e\%%%Mg(s)%
C)%A%and%E%represent%the%anode:%Mg2+(aq)%+%2e\%%Mg(s)%
D)%B%and%F%represent%the%anode:%%Zn(s)%%Zn2+(aq)%+%2e\%
E)%B%and%F%represent%the%cathode:%Zn2+(aq)%+%2e\%%%Zn%(s)%
%
%
%
%
%
%
48.%What%is%the%oxidation%state%of%N%in%Sn(NO3)4?%
%
%
A)%\3%
%
B)%+2%
%
C)%+3%
%
D)%+4%
%
E)%+5%
%
%
CHEM%1310%
Sample%Final%Exam%
49.%%Which%reaction%corresponds%to%the%cell%diagram?%
%
Pt(s)%|%H2(g)%|%H+(aq)%||%Ag+(aq)%|%Ag(s)%
%
%
A)%H2(g)%+%2Ag+(aq)%%%2H+(aq)%+%2Ag(s)%
%
B)%2H+(aq)%+%Pt(s)%+%2Ag(s)%%%%H2(g)%+%2Ag+(aq)%
%
C)%2H+(aq)%+%Ag(s)%%%%H2(g)%+%Ag+(aq)%
%
D)%Pt(s)%+%H2(g)%+%2Ag+(aq)%%%2H+(aq)%+%2Ag(s)%
%
E)%H2(g)%+%Ag+(aq)%%%2H+(aq)%+%Ag(s)%
%
%
50.%%What%is%the%standard%cell%potential%(Eocell)%when%a%galvanic%cell%is%constructed%
using%the%following%half\reactions?%
%
%
%
Au3+%+%3e\%%%Au(s)% %
Eo%=%+1.50%V%
+
\
%
%
Cu %+%e %%Cu(s)%
%
Eo%=%+0.52%V%
%
%
%
A)%+0.52V%
%
B)%+0.98%V%
%
C)%+2.02%V%
%
D)%\0.98%V%
%
E)%\2.02%V%
%