2208-6114
10 pages
M08/4/CHEMI/HP2/ENG/TZ2/XX
Thursday 8 May 2008 (afternoon)
CHEMISTRY
HIGHER lEvEl
PaPER 2
INSTRUCTIONS TO CANDIDATES
•
Write your session number in the boxes above.
•
Do not open this examination paper until instructed to do so.
•
Section A: answer all of Section A in the spaces provided.
•
Section B: answer two questions from Section B. Write your answers on answer sheets. Write
your session number on each answer sheet, and attach them to this examination
paper and your cover sheet using the tag provided.
•
At the end of the examination, indicate the numbers of the questions answered in the candidate
box on your cover sheet and indicate the number of sheets used in the appropriate box on your
cover sheet.
2 hours 15 minutes
Candidate session number
0
0
© International Baccalaureate Organization 2008
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Section a
Answer all the questions in the spaces provided.
1.
Hydrogenandnitrogen(II)oxidereacttogetherexothermicallyasfollows.
2H (g) 2NO(g)
2H O(g) N (g)
2
2
2
+
→
+
Therateofthisreactionwasinvestigatedinaseriesofexperimentscarriedoutatthesame
temperature,theresultsofwhichareshowninthetablebelow.
Experiment
Initial
[H (g)]
2
/
moldm
−3
Initial[NO(g)]/
moldm
−3
Initialrateofreaction/
moldm s
−
−
3
1
1
2.0
×
−
10
3
4.0
×
−
10
3
4.0
×
−
10
3
2
4.0
×
−
10
3
4.0
×
−
10
3
8.0
×
−
10
3
3
6.0
×
−
10
3
4.0
×
−
10
3
4
2.0
×
−
10
3
2.0
×
−
10
3
1.0
×
−
10
3
5
2.0
×
−
10
3
1.0
×
−
10
3
(a) ExplainhowtheresultsfromExperiments1and2canbeusedtodeducethattheorderof
reactionwithrespecttohydrogenis1.
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[1]
(b) Deducetheorderofreactionwithrespecttonitrogen(II)oxide,givingareasonforyour
answer.
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[2]
(c) Useyouranswersfromparts(a)and(b)todeducetherateexpressionforthereaction.
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[1]
(d) CompletethetableabovebycalculatingtherateofreactionforeachofExperiments
3and5(writeyouranswersinthetable).
[2]
(This question continues on the following page)
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(Question 1 continued)
(e) UsetheresultsfromExperiment1todeterminethevalueof,andtheunitsfor,therate
constant,k,forthereaction.
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[2]
(f) Suggestamechanismforthereactionthatisconsistentwiththerateexpression.
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[2]
(g) Thereactionisfasterinthepresenceofaheterogeneouscatalyst.Explainthemeaningof
thetermheterogeneousasappliedtoacatalyst.Drawalabelledenthalpyleveldiagram
thatshowstheeffectofthecatalyst.
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[3]
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2.
(a) A 25.0
cm
3
sample of an aqueous solution of barium hydroxide, of concentration
0.146mol
dm
−3
wasexactlyneutralizedby28.7
cm
3
ofaqueousnitricacid,according
tothefollowingequation.
Ba(OH) (aq) 2HNO (aq)
Ba(NO ) (aq) 2H O(l)
2
3
3 2
2
+
→
+
Calculatetheconcentration(inmol
dm
−3
)ofthenitricacid.
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[3]
(b) Asolutioncontaining0.142molaqueousnitricacidwasaddedtoasolutioncontaining
0.107molbariumhydroxide.Calculatetheamount(inmol)ofbariumnitrateformed.
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[1]
(c) A 0.010 mol sample of the barium nitrate formed was heated until it had completely
decomposedaccordingtothefollowingequation.
2Ba(NO ) (s)
2BaO(s) 4NO (g) O (g)
3 2
2
2
→
+
+
Use the ideal gas equation to calculate the total volume, in
cm
3
, of gaseous products
obtainedat387Kand
1 12 10
5
. ×
Pa.
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[3]
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3.
Values of first ionization energy for the elements are shown in Table 7 of the Data Booklet.
(a) Define the term first ionization energy and write an equation to illustrate it, using
magnesiumasanexample.
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[3]
(b) Explain why the first ionization energy of aluminium is lower than that of magnesium.
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[2]
(c) Explain why the third ionization energy of magnesium is much higher than its first
ionizationenergy.
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[2]
(d) Use the Aufbau principle to deduce the full electron configuration of cobalt. Identify the
sub-level from which an electron is removed when the first ionization energy of cobalt
ismeasured.
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[2]
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4.
(a) Using information from Table 16 of the Data Booklet, write an equation for the
dissociation of chloroethanoic acid, and calculate the pH value of a 0.200 mol
dm
−3
solutionofchloroethanoicacidat298K.
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[5]
(b) TheapproximatepHvaluesoffourequimolaraqueoussaltsolutionsareshowninthe
followingtable.
Solution
A
B
C
D
pH
2
6
7
9
Thesolutionsarelistedbelow.Matcheachofthesolutionswiththeletter(A,B,CorD)
bywritingtheletternexttotheappropriatesolution.
potassiumbromide . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
potassiumethanoate . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
iron(II)chloride. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
iron(III)chloride . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
[2]
(c) Giveareasonforeachofyourchoicesinpart(b).
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[4]
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Section b
Answer two questions. Write your answers on the answer sheets provided. Write your session number
on each answer sheet, and attach them to this examination paper and your cover sheet using the tag
provided.
5.
(a) Define the term standard enthalpy of formation,andwriteanequationtoillustrateit,
usingmethanolasyourexample.
[4]
(b) Onereactionusedinthemanufactureofmethanolisshownbelow.
CO (g) 3H (g)
CH OH (g) H O(g)
2
2
3
2
+
→
+
Define the term average bond enthalpy. Using values from Table 10 of the Data Booklet,
calculatetheenthalpychangeforthisreaction.
[5]
(c) One industrial method of manufacturing ethanoic acid uses methanol as a feedstock in the
followingexothermicreaction.
CH OH (l) CO(g)
CH COOH (l)
3
3
+
The standard enthalpy of formation of CO (g) is –111 kJ
mol
−1
.Usinginformationfrom
Table 11 of the Data Booklet, calculate the enthalpy change for the reaction above.
[2]
(d) Typical conditions used for the reaction in part (c) are 450K and 30atm. Use Le
Chatelier’sprincipletopredictandexplaintheeffectonthepositionofequilibriumof,
separately,increasingeachofthesevalues.
[4]
(e) Statewhatismeantbythesymbol
∆
S
Ö
.Predict,withareason,thesignof
∆
S
Ö
forthe
reactioninpart(c).
[2]
(f) Methanolcanbemadefrom“synthesisgas”,producedbythefollowingreaction.
CH (g) H O(g)
3H (g) CO(g)
4
2
2
+
→
+
Forthisreaction,
∆
H
Ö
= +210 kJ
and
∆
S
Ö
= +
−
216
1
J K
.
Usethesevaluestoexplainwhythisreactionisnotspontaneousat298K.Calculatethe
temperatureatwhichitbecomesspontaneous.
[4]
(g) Areactionthatcanbeusedtopreparemethanolisshowninthefollowingequation.
CH Br NaOH
CH OH NaBr
3
3
+
→
+
Givethenameofthemechanismofthisreactionandshowthemechanism,usingcurly
arrowstorepresentthemovementofelectronpairs.
[4]
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6.
(a) TheVSEPRtheorycanbeusedtopredictthedistributionofelectronpairsandtheshapes
andbondanglesofmanymoleculesandions.Showhowthistheorycanbeusedto
explainwhyammoniahasatetrahedraldistributionofelectronpairs,atrigonalpyramidal
shapeandabondangleof107°.
[3]
(b) ApplytheprinciplesoftheVSEPRtheorytoeachofthefollowingspecies,ineachcase
predictingtheshapeoftheelectronpairdistribution,theshapeoftheactualspeciesand
thebondangle(s).
(i) F
2
O
(ii)
F O
ICl
2
4
−
[3]
[3]
(c) Thecompoundchloroethene,
CH =CH Cl
2
−
,canbeusedtoillustrateseveraltermsused
inthetheoryofbonding.Usingthiscompoundastheexample,explainwhatismeantby
eachofthefollowing.
(i) Lewisstructure
[1]
(ii) Sigmaandpibonds
[4]
(iii) Hybridization
[2]
(d) Thecarbon-chlorinebondlengthinchloroetheneis0.169nm.Useinformationfrom
Table 9 of the Data Booklet to explain how delocalization of electrons can occur in this
moleculeandsuggestavalueforitscarbon-carbonbondlength.
[4]
(e) Arrangethefollowingcompoundsinorderofincreasingboilingpoint(startingwiththe
lowestboilingpoint)andexplainyourchoicebyreferencetotheintermolecularforces
involved.
[5]
bromoethene
chloroethene
ethene
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7.
(a) Aluminiumandoxygencombinetogethertoformacompoundthathasahighmelting
pointandisagoodconductorofelectricitywhenmolten.Writeanequationtorepresent
thereactionandexplain,intermsofitsbondingandstructure,whythecompoundhas
theseproperties.
[4]
(b) Aluminiumandchlorinecombinetogethertoformacompound
Al Cl
2
6
thathasalow
meltingpointandisapoorconductorofelectricitywhenmolten.Explain,intermsofits
bondingandstructure,whyithastheseproperties.
[3]
(c) Describe the two different ways in which current flows during the electrolysis of molten
aluminiumoxide.Writeanequationshowingtheformationofeachoftheproducts.
[4]
(d) Samplesofaluminiumoxideandaluminiumchlorideareadded,withstirring,toseparate
beakers of pure water. Suggest the pH value of the liquid in each beaker after the stirring,
givingareasonforyourchoice.Writeanequationforanyreactionoccurring.
[5]
(e) Ahalf-cellismadeusinganaluminiumrodandanaqueoussolutionofaluminiumsulfate.
State two conditions that must apply if this half-cell is used to measure the standard
electrodepotentialofaluminium.
[2]
(f) The cell described in part (e) is connected to a silver half-cell, both under standard
conditions. Using information from Table 15 of the Data Booklet, deduce the overall
equationforthereactionthatoccurs,andcalculatethecellpotential.
[3]
(g) Whenwaterreactswithzincionsitactsasaligandintheformationofthecomplexion
[Zn (H O) ]
2
4
2+
.Explainwhatismeantbythetermligand.Explainwhysolutionscontaining
thiscomplexionarecolourlessbutthosecontaining
[Fe(H O) ]
2
6
3+
arecoloured.
[4]
0910
2208-6114
–10–
M08/4/CHEMI/HP2/ENG/TZ2/XX
8.
(a) Explainwhythe
1
HNMR
spectrum of butane shows two peaks with areas in the ratio 3:2. [2]
(b) Describethestructuralfeatureresponsibleforopticalisomerism.Outlinehowoptical
isomerscanbedistinguished.
[3]
(c) Alcohols can be oxidized by refluxing with hot acidified potassium dichromate(VI).
Statethecolourchangeoccurringwhenthiscompoundactsasanoxidizingagentandthe
oxidationnumberofthechromiumcompoundformed.
[2]
(d) Therearefourstructuralisomersofthealcoholwiththeformula
C H OH
4
9
.Thesealcohols
canbedistinguishedusingtheinformationreferredtoinparts(a)to(c).Thefollowing
tablegivesfurtherinformationaboutthesefouralcohols.
Alcohol Number of peaks in
1
HNMR
spectrum Opticalisomers
Finalorganicoxidationproductwith
acidified potassium dichromate(VI)
A
5
no
carboxylicacid
B
5
yes
ketone
C
4
no
carboxylicacid
D
2
no
nooxidationoccurs
DeducethestructuralformulaofeachofthealcoholsAtoD.
[4]
(e) ForalcoholB,drawtwostructurestorepresenttheopticalisomers,showingclearlythe
relationshipbetweenthem.Writeanequationfortheoxidationofoneoftheoptical
isomersofB,using[O]torepresenttheoxidizingagentandshowingthestructureofthe
organicproduct.
[3]
(f) AlcoholsAandCcanbeoxidizedtodifferentproductstothosenamedin(d)usingthe
sameoxidizingagentasinpart(c).Statethetypeofcompoundformedintheseoxidations
anddescribetheconditionsusedtoobtainthistypeofcompound.
[2]
(g) Three alkenes are formed by the dehydration of alcohols A to D. Draw the structures of
these alkenes.
[3]
(h) There are three possible compounds with the molecular formula
C H O
3
8
. Two of
these compounds E and F have infrared spectra that show absorption in the regions
of 1000–1300
cm
−1
and 3230–3550
cm
−1
. Use this information, and table 18 in the
Data Booklet, to deduce the structures of E and F. Explain how you could distinguish
betweenEandF.
[6]
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