XII - ISC BOARD - Rao IIT Board Paper... · 2015. 3. 23. · rao iit academy/ isc - board...
Transcript of XII - ISC BOARD - Rao IIT Board Paper... · 2015. 3. 23. · rao iit academy/ isc - board...
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PART IQuestion 1:(a)(i) positive , lesser(ii) efficient , 74(iii) decreases , common-ion effect(iv) Cannizzaro , no hydrogen (v) paramagnetic , dimagnetic(b)(i) (2) –0.372°C(ii) (3) 1155(iii) (2) Secondary Alcohol(iv) (4) Octahedral and sp3d3
(v) (1) +3 and + 4(c)(i) As temperature increases, concentration of H+ and OH– increases and hence pH value decreases.
At 298 K.14H OH 10
for neutral solution pH = 7and at high temperature pH will be less than 7.
(ii) 3 2Fe e Fe
for 1 mole of 3 ,Fe 1 mole of e is required
for 3 moles of 3 ,Fe 3 moles of e are required
3 3 3 96500e F C
Q I t
3 96500 2 t
3 965002 3600
t
40.2t hrs
XII - ISC BOARDDate: 20.03.2015 CHEMISTRY - SOLUTIONS
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(iii) Mixture containing potassium cyanate and ammonium sulphate on heating gives ammonium cyanate whichfurther gives urea
4 2 4 4 2 4urea
2 ( ) 2KCNO NH SO NH CNO N H CO
(iv) Yes(v) 3 2 3 Strong AcidWeak Acid
CH COONa H O CH COOH NaOH
3 2 3CH COO Na H O CH COOH Na OH 1
3 2 3CH COO H O CH COOH OH
OH are left in the solution
Sodium acetate on hydrolysis gives basic solution.
(d) (i) ; ii (iii) iv vd c b e a
PART II
SECTION AQuestion 2:(a)(i) 2 0.5w g
1 100w g1
1 18 .M g mol
0 0.24 0.24fT C
22
1
1000 1000 1.86 0.5 38.75 /0.24 100
f
f
k wM g mol
T w
Calculated (theoritical) mol mass of 39 35.5KCl
174.5 g mol
Calculated molar mass 74.5 1.92Theobserved molar mass 38.75
i
1.92i
KCl K Cl
Initial 1 0 0Equillibrium 1-
KCl K Cl
total number of moles after dissociation = 1
= 1
1 or 11
i i
1.92 1 0.92 degree of dissociation = 0.92
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(ii) Given:mass of sugar = 1.71 gmolar mass = 342 gvolume of solution = 500 mltemperature = 300 KFormula used
number of moles mass of sugarmolar mass
number of moles of soluteMolarity =volume of the solution in litres
Osmotic pressure CRT
Solution:
number of moles = 1.71342
0.005
0.005 1000Molarity C500
= 0.01 MOsmotic Pressure = CRT 0.01 0.083 300
0.249 bar
(iii) Given
Mass of solute = 20.70 g w
Mass of solvent = 32 g (w1)
0.25bT C
11.72 .bK K kg mol
To find = M2 (molecular mass of organic compound)
Formula 22
1
1000 b
b
K wMw T
21000 1.72 0.70
32 0.25M
2 150.5M g
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(b)(i)
Order Molecularity 1. Order of a reaction is an
experimental quantity. It can be zero and even a fr action.
Molecularity of a reaction is number of species (atoms, ions or molecules) taking part in elementary reaction. It cannot be zero or non integer
2. Order is applicable to e lementary as well as complex reactions.
Molecularity is applicable only for elementary reactions.
3. For complex reaction, order is given by slowest step.
Molecularity of the slowest step is equal to the order of over all reaction.
(ii) Given : Following is a 1st order reaction.
1/ 2t half life of a reaction = 120 min
To Find :Time required to complete 90% of the reaction.Solution:Let the reaction constant be KInitial concentration [R0]Now calculating constant K
1/ 2
0.693Kt
0.693120
K
10.0058 minK
Now time required to complete 90% of the reaction
Final concentration 0 00.9R R
00.1 R
Now,
2.303 log0.1
o
o
RK
t R
2.303 1log
0.0058 0.1t
2.303
0.0058t
397.06 mint time required to complete 90% of reaction = 397 .06 min.
(c) Crystal structure of Cu metal is FCC or CCP[Face centered cubic or cubic closed packed]
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Question 3:(a)(i) Given :
Crystal structure of Cr = BCCEdge length (a) = 287 pmTo findAtomic radius r
Density
Solution:For BCC crystal system
Edge length (a) 4
3r
34
ar
0.433 287 pm
124.27r pmNow density of a crystal :
3A
zMa N
Wherenumber of atom in BCC unit cell 2z
M = Molar mass of 52.99Cr g
33 287a pm
312287 10 m
310287 10 cm
23 32.37 10 cm
236.022 10AN atoms
3DensityA
zMa N
23 232 52.99
2.37 10 6.022 10
105.9814.27
Density of crystal = 7.42 g/cm3
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(ii) NaCl show metal excess defect due to anionic vacancies. When crystals of NaCl are heated in an atmosphere
of sodium vapour, the sodium atoms are deposited on the surface of the crystal. The Cl ions diffuse to thesurface of the crystal and combine with Na atoms to give NaCl. This happens by loss of electrons by sodiumatoms to form Na+ ions. The released electrons diffuse into the crystal and occupy anionic sites. As a resultcrystal now has excess Na+ ions. The anionic sites occupied by unpaired electrons are called F–centres. Theyimpart yellow colour to the crystals of NaCl. The colour results by excitation of these electrons when theyabsorb energy from visible light falling on the crystal.
(iii) 2( ) 2 33 2g g gN H NH
K (equilibrium constant) = 6.0 × 10–2 1mol L
Temperature (T) = 715 K
12 0.25H mol L
13 0.06NH mol L
2 ?N
23
32 2
NHK
N H
23
2 32
NHN
K H
2
32
0.06
6.0 10 0.25
20.0036
6.0 10 0.015625
12 3.84N mol L
(iv) 2 16.2 10H mol L 1410H OH
Now putting the value of H
14
210
6.2 10OH
13 11.61 10OH mol L (v) Le–Chatelier’s principle : The principle states that if an external stress is applied to a reacting system at
equilibrium, the system will adjust itself in such a way that the effect of the stress is reduced.
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(b)(i) NaCl crystallises in FCC lattice
(ii) Each Na+ ion is surrounded by six Cl ions and each Cl ion is surrounded by six Na ions.(iii) Number of Cl ions = 4
Number of Na ions 4
(iv) In the NaCl crystal, Cl ions occupy all the FCC positions and Na+ ions occupy the octahedral voids.(c)(i) Increase in temperature – forward reaction
Decrease in temperature – backward reaction(ii) Increase in pressure – forward reaction
Decrease in pressure – backward reaction(iii) Increase in conc. of [N2O4] – forward reaction
Decrease in conc. of [N2O4] – backward reaction(iv) Removal of NO2 causes decrease in [NO2] – forward reactionQuestion 4:
(a) 4 1 11.65 10K cm
3
0 1 2 1
0 1 2 1
349.1
40.9H
CH COO
cm mol
cm mol
0.01 .C M
(i)4
1 2 12
1000 1000 1.65 10 16.510
K cm molC
1 2 116.5 cm mol
(ii) 3 349.1 40.9 390.0H CH COO
16.5 0.0423390
0.0423
(iii)2 2(16.5) 0.01
( ) 390 (390 16.5)CK
51.86 10K
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(b)
(i) 2 2Mg Cu Mg Cu
2 3
4210 1010
MgQ
Cu
2n
010
0.0592 logcell cellE E Qn
100.05922.71 log 10
2
2.71 0.0296
2.68cellE V
(ii) In pure water2 2
4spK Ba SO
9 21.5 10 S
91.5 10S
1015 10
53.87 10S M
in 0.1 M 22BaCl Ba 0.1x
Cl x
22K Ba Clsp
9 21.5 10 0.1x x
9 21.5 10 0.1 is very smallx x
2 81.5 10x
81.5 10x
41.224 10x M
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(c)
(i) 4 4NH OH NH OH
4 4NH Cl NH Cl
33Fe 3OH Fe OH
22Ca 2OH Ca OH
sp3 2K Fe OH is very less compared to K Ca OHsp hence 3Fe OH will be precipitated
and 2Ca OH remains in solution.
(ii) 22H S 2H S when strong acid is added HCl H Cl . Due to common ion effect,
concentration of H+ is suppressed. Therefore dissociation of 2H S suppressed.
SECTION B
Question 5:(a) IUPAC Name
(i) 3 2 34 2Cr NH H O Cl Tetra ammine diaqua chromium (III) chloride
(ii) 2 3 44Pt Cl NH PtCl Tetraamminedichloro platinum (IV) tetrachloro platinate (II)
(b) 3
6Fe CN
hybridisation = d2sp3
magnetic property = paramagnetic(c)
(i) 2 2
3 4 3 45 5Co NH Br SO Co NH Br SO
1
3 4 3 45 5Co NH SO Br Co NH SO Br
Both are ionisation isomers.
3 4 2 45 red violet ppt ofCo NH Br SO BaCl BaSO
3 4 35 red ppt ofCo NH SO Br AgNO AgBr
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(ii) 2 2Co(en) Cl
Co Co
Cl ClCl Cl
enen
en en
+ +
Cis form
Non super imposable mirror image structure
Question 6:(a)
(i) 2 2 22 2 2NaOH F F O NaF H O
(ii) 24 2 2 2 22 6 5 2 8 5MnO H H O Mn H O O
(iii) 2 4 2 2 22H SO H S H O SO S
(b) 4XeF
Xe
F
FF
F
Hybridisation = 3 2sp dGeometry = square planar
Question 7:(a) Silver :
Argentite or silver glance 2Ag SLeaching Process:Steps:
2 22Ag S 4 NaCN 2 Na Ag CN Na S
2AgCl + 2 NaCN Na Ag CN NaCl
2 2 2 4Na S 2O Na SO
2 2 2 42Ag S + 4 NaCN + 2O 2 Na Ag CN + Na SO
22 4ppt
2 Na Ag CN + Zn 2 Ag + Na Zn CN
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(b)(i) Due to small size of transition metal atoms or their cations and high effective nuclear charge, they have
a high positive charge density on them. This high positive charge density makes the atoms or cations toattract the lone pairs of e– from the ligands.
The transition metal cation or atoms have vacant d-orbital in which they can accomodate the lone pairs
of e– donated by ligands and thus can form L M coordinate bonds.(ii) Paramagnetic character increases with the increase in the number of unpaired electrons. The larger is the
number of unpaired e– in central atom or ion greater is the paramagnetic character.
Hence from Sc to Mn number of unpaired e– increases and then from Fe to Zn decreases. Hence paramagneticcharacter also increases from Sc to Mn and then decreases from Fe to Zn.
SECTION CQuestion 8:(a)(i) Glycerol to formic acid
HO OHOH
3H– C – OHFormic
acid
Pd(I) CatalystH O2 2
Glycerol
O
(ii) Chlorobenzene to phenolCl OH
+ OH–
Chlorobenzene Phenol
NaOHpressure, H+
(iii) Diethyl ether to ethanol
3 2 2 3 2 5 2 5Diethyl ether Ethanol
CH CH O CH CH HI C H OH C H I
(iv) Phenol to anilineOH NH2
+ NH3
Phenol Aniline
ZnCl /2
High pressure + H2O
(b)
(i) 3 2 2 3 2Ethanol Iodoform
CH CH OH 4I 6 NaOH CHI HCOONa 5 NaI 5H O
(ii) Chlorobenzene is heated with sodium metal in presence of dry ether gives diphenyl compound.
+ 2Na2
Cl
dryether + 2 NaCl
Chlorobenzene Diphenyl Compound
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(c) Identifying compounds :
CH COCH3 3conc. HNO3
SOCl2
(O)CH C OH3
– – CH – C – Cl3
ONH3 CH – C – NH3 2
O
LiAlH4
CH CH NH3 2 2HNO2CH COCl3 C H OH2 5C H – O – C –CH2 5 3
O
O
(A) (B) C
(D)(E)(F)
Question 9:(a)(i) Reimer – Tiemann reaction :
OH ONa OH
+ CHCl3
Phenol
NaOH, 340 K –H O2
CHCl2 CH(OH)22 NaOH
ONa
CHO
– H O2
dil. HCl– NaCl
OH
CHO
Hydroxybenzaldehyde
(ii) Rosemund Reaction :
CH – C – Cl + H3 2 CH – C – H + HCl3
O OPd , BaSO4
Boiling xyleneAcetyl chloride Acetaldehyde
(iii) Hoffmann’s degradation reaction :
CH – C – NH3 2 + Br + 4NaOH2 CH NH + 2 NaBr + Na CO + 2H O3 2 2 3 2
O
Acetamide Methylamine
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(b)(i) Ethylamine and diethylamine
Ethylamine reacts with Nitrous acid in cold condition to form unstable diazonium salt and which decomposesto give alcohol with liberation of N2 gas.
2 5 2 2 2 5 2 2C H NH + NaNO + 2HCl C H N Cl NaCl + 2H O +
2 5 2 2 5 2C H N Cl H O C H OH + HCl N diethylamine reacting with Nitrous acid give yellow oily N–Nitrosoamines
22 5 2 5 2 5 2
N nitroso diethylamineC H NH C H HO N = O C H N N = ONaNO
HCl
(ii) Acetaldehyde and benzaldehyde
Acetaldehyde reacts as reducing agent which reduces Fehling solution. The aldehyde gets oxidized tocarboxylate ion and Cu2+ is reduced to Cuprous oxide
23 3 2
Carboxylateion
Acetaldehyde
O|
CH C H + 2Cu 5OH CH C = O Cu O||O
Benzaldehyde
CHO(aromatic aldehyde) are not oxidised by Fehling solution.
(c)(i) Compounds in ascending order of their basic strength:
diethylether < Aniline < Methylamine < ethylamineIn aliphatic amines, due to presence of electron donating alkyl group, electron density on nitrogen increases.Hence lone pair is easily available for protonation.In aniline the lone pair of nitrogen is in conjugation with benzene and less available for protonation henceaniline is less basic than aliphatic amine and ethers are inert in nature due to stable C O C bond .
(ii) (a) Polyester :Monomer used :Ethylene Glycol 2 2OH CH CH OH
Dimethyl terephthalate H C – O – C3 C – O – CH3
O OType of Polymerization : Condensation polymerization.
(b) Bakelite :Monomer used :Phenol :
OH
Formaldehyde – HCOOH
Type of Polymerization : Condensation polymerization.
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Question 10:
(a) 3 2 2A CH CH NH
3 2 2 2 3 2 2 2(B)(A)
CH CH NH HNO CH CH OH N H O
3 2 3 2(C)
Controlled
(B)CH CH OH (O) CH CHO H O
3 3 2 3 3 2(D)(C)
CH CHO 2[Ag(NH ) ] + 3OH CH COOH 2Ag 4NH 2H O
CH COOH + HO – CH – CH3 2 3 CH – COO – C H + H O3 2 5 2Con. H SO2 4
dil. H SO2 4
(E)Ethyl acetate
CH – CHO – NH3 3 CH – CH – OH3 CH – CH = NH3
NH2
Acetaldamine(C)
(b)
(i)Cold
3 2 2 2 3 2 2 2Ethylamine
CH CH NH HNO CH CH OH N H O
72 2
2 43 2 3 2
K Cr Odil. H SO ,CH CH OH (O) CH COOH H O
CH – COOH + NH3 3 CH – C – O NH3 – +
4
O
CH – C – O NH Br + 2KOH 3 2 – +
4 +
O CH – NH + 2KBr + 2H O + CO3 2 2 2
Methylamine
(ii) When globular proteins undergo coagulation or precipitation to give fibrous proteins, due to coagulation thenative shape of protein is destroyed and biological activity is lost. That is why coagulated proteins so formedare called denaturated proteins.During denaturation, secondary and tertiary structures are destroyed but primary structure remains intact.
(iii)
Adenine (A) Guanine (G)
NH2
N
N
N
N
O
N
N
N
NH N2
Thymine (T)
O
N
N
CH3
O
Cytosine (C)
NH2
N
NO
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(c)
(i)
NH2 N2Cl
+ HNO + HCl2273
278 k
+ –
+ 2 H2O
(ii) CH – CO – Cl + HO – C H3 2 5 CH – COO – C H3 2 5 + HClPyridine
(iii)3 2 6 4 2
O||
6 H C H 4 NH (CH ) N 6H O