Pre University Board 2008 P.U.C Physics, Chemistry, Maths
Karnataka second CHEMISTRY June 2008 Kan & ENG version is in Pdf Format Check tat beneath.
Code No. 34
Total No. of Questions : 39 ] [ Total No. of Printed Pages : 15
June, 2008
( Kannada and English Versions )
Time : 3 Hours 15 Minutes ] [ Max. Marks : 90
( Kannada Version )
ii) - A, B, C ddo D 0>
' * 77 -0 CO y C*, C*, 6
_D
iii) - A do Sx4r 0X@ oo oddod 10 odrto, - B do od@ 2 oddod 20 odrto, - C do
0x, 5 odrtod 40 odrto )ri - D do D 1 10
odrt> D 2 44 od, 5 odrtod 10
2 CO y ct 6
odrtdod d
_D
iv) rt ddo o d;rt>0R ddo ,oeddrart>dR ddoo.
- A
co y <=i <=i _o
ii) oo sy d oo d3d6Y do-n>0R ddoedo. 4 od oddodrf. 10 x 1 = 10
y y oi _o
1. Qo ne,Y-o dod eSrS,<o SdeA,o de ,dd
2. 3d rra Aob, eo,d Jdo ,oA.
3. o ea<do, eXdrado doo.
CO ct
4. ea<z ( NH 3 ) ,o<dooA ddo, rao ,>do doo.
5. ,j0OeO doo, ( Spontaneous process ) &Sz 0o!e& ert
_D
6. ,dod dod, d, ( Dispersed phase ) /d)o ?
7. odo ( Ethylamine ) <,&, Wdo, ( Nitrous acid ) doart ,o<ert oa>rt J (d/rtod aod ,oA.
>J _o ct
8. Xrd ( Polysaccharide ) 0O de ?
9. Sodribd <X,@ ( Drying oil ) odo OT d}ob, X&S.
10. rtAea ( Glycine ) Ozope<do d(doo doo.
- B
i) <zd)d) 0o oA.
ii) d,<>oo do 0ddo oXrt>bt oadod.
10 X 2 = 20
11. o-poaoo ded) Xeooo AXrt ( Cr 2 O 3 ) dXrX. b, 0 ons.dj X.doart doA.
ct co 6 <A
12. d,< rtodsado,d) ( H 2 SO 4 ) aors wdodoart oa,a<doaddaA sen
dr,o d ? dd Doeddraddo doO.
_0 c
13. ,od,dora ( d-y ) dort>o ,do/> (dooddo, o&od/dod. dd1! 0ddo sadrart>o doO.
ct
14. K 4 [ Fe ( CN ) 6 ] d darad dOadosaO ddd/rao ,oZ6 ( EAN ) (dodo, dodoaoO.
15. dddo drtrd da,a<doad 3/do<d>odd dert a<doaodd) P23 x 10 - 2 s-1 wAdd, 3/do<do d'andoo ( Half-life ) ddo, d@ sad
16. x> A d)rt>o d< sart dor< doaKwrtda ( Strong and weak electrolytes ) ort :
i) H 2 S
ii) CH 3 COONa
iii) KNO 3
iv) NH 4 OH
17. wdr doo dadr dadrartdod (d/ddadd 0ddo drtdo doO.
18. dor< doaaKnn ( Weak electrolytes ) Lod adOS/ddra aidododdo ,od\e&&.
19. deaod) aoedodofioa e d,< ddo,. do ado.
20. daos5" ao2>ra ( Racemic mixture ) 0oddeo ? odo dd} X&S.
21. aoeo e* wA ert d0dF,oa0 ?
22. Xdo, dddF} 0odeo ? 3,<o<o dra, cEoad ,aoeddrado
co r\) ct ZS t> t
doO.
- C
I. X> fld)rt>, <zdd 0-3 drtrt O : 2x5=10
23. a) Xedoaod dPioo dXdoel ( K 2Cr 2O 7 ) Qod
a dOr ado. dd@ ,oopd ,aoeddrart>R doo. 4
b) X>A ,oooXrt>o eO,d ,draoAeoJ(o addo ,O :
Cl 0 doo
Pt ( NH -1 Cl,
Br 2 . 1
Pt ( NH 3 ) 4 Br 2 J Ci 2 d0S0- " Pt ( NH 3 ) 4 Ci 2
24. a) 0d d d.rad o aoao dO,d ,odFd 0 doodo<o (i)
aO (?> co v *
d do (ii) dddFra do srt (iii) S&j d doort>< dood ooad ort>o ado. 3 b) eoo 0ddo dertrtg 2
4 -
25. a) ,o<ert o ropd wddd [ Fe ( CN )6 ] d, wsd doOo ooeo rtora drt>o ado. 4 b) dddrad dddd 2,ed a<do ,o. 1
CO y O Ct
II. d>Ad)rt>, </d)d3dd dodo drt$n Oft : 3 x 5 = 15
26. a) do6oe* ( Cumene ) >Q0 p,od rt0o d0. 3
b) s* wdo,d) pci 5 oan aoaddA Sen dFod ? do
a3,3<oad ,&oeddrado do0. 2
ct
27. a) oea X%e0e* S/oo 3,/ .asdO d0. 3 b) sFods* 3,(0 0oddeo ? dd ooad ,&oeddrado doO. 2
28. a) a-rioe,* >iidd*F d3 do doO. 2
b) d<0d* ,>t dotd ( Baeyers Strain theory ) ( Postulates ) rt>0 000. 3
ot
29. a) d)|)F doad d30}doart d0. 2
b) <d oOed- rad Or d0. 2
c) Sde3<deaeddra ( Dehydrohalogenation ) 3000, d <eA,od 50 d ( Reagent ) (/>d)do ? 1
iii. x> Ad)n>, /d)o dodo dnn tp : 3 x 5 = 15
30. a) ddo drtF ooad Sxoo dert aosodd ,oeddrado aa. 4
b) /as* ,drt > ,{6odd0R dz. 1
aa aodY 660 Pa $d dodDaoQD ( Lowering of vapour pressure ). 50C 3ad, eO aa 12260 Pa
DO</ raD dodDSDO. 3
CO CO <=i
b) saDdeoQ, &d de Cb ( Body centered cubic unit cell )
drart > ,oZ.dD d, aS.
6 t u
32. a) a1 < ( Brownian movement ) 0ode ? ert
oiariD.rf ?
,a/, dOaD dd ea nra<a d<>eA
6 -> cp oi
0dd e ribo& eD da,adrt>o d art O.
y 6 co 6 ct-ot3 n
33. a) 0-1 M NH 4 OH D. 0-15 M NH 4 Cl a,drart >0 D5,daAdD &,d pOH o d@ aS.
( NH 4 OH (eaa %pda>od = 1-8 X 10 - 5 ) 4
b) WD ( Lewis acid ) 0o de ? 1
34. a) 298 K (D aoD da,a<D>d SjDD , daod) K
' co y cp cp p
2
2
b)
3
dd 1-06 x 10 5 wAd, ad
3. aa}<D
_o _o
CO CO
( A G o ) d@ aS.
b) os3j,a<D>d e 0ode ? osa,,a<D>d eD
ar
0ddb d<DDd DD
3
_0 c
- D
35. a.) raD dd,d a o ( molecular orbital theory ) d a<D,
n>D, ( Assumptions ) adDO.
4
b) {Pd PD ? oD rao Sp, 0iJ
doe ? 2
c) Xedjo 3/ooOr PO. 2
d) 0-001 M HNO 3 a,raY [ H + ] 00 [ OH - ] Or X@ aS.
2
36. a) X>A rt>bR : 2
i)
ii) oa O}ado
b) Poa>w 4xo rtr 3,<o 0odeo ? oo ad}oOR Xs. 2
c) Li 2 raoP 36 oj X\oOr doO art - o eo X@ aS, o,a@0eo ribra ( Magnetic property ) &&. 3
d) {ade S/dd S;/ Pa6,OR PO. 3
D 2
V. X> Ad)rt>P /)ad 0rfo JO : 2x5=10
37. a) &iaad(ao p-edeiaadR dertadop ert J</O,oartoJrf ? 3
b) 4/Ddl' OeXO PO. 2
38. dPia<Do d d,djei dD. dPia<Do dodra S/dd 3x</dertd doed dD dO}adDd0 eO,d d,ertd0 dO. 5
39. d,d/rad dPiaDo ddDel daxdrad0 deA& d," deao ,<1 a,dradY-Dd d," deao ,djel dO}adDd0 dodb&aDod d,ertY X>Ad)rt>D :
i) w Sxdd oa,a<Dad ,DeddradD adDO.
ii) d," deaDo ,/!" ,d/ d,d6oa&D0
iii) d,<>ertdY d<>eAd ,d /d)D ?
iv) s,dd o.d wribd ara d adad}<De ? 2+1 + 1 + 1
' ZJ t co rs
( English Version )
Instructions : i) The question paper has four Parts.
ii) Parts A, B, C and D are common to all the candidates.
iii) Part A carries 10 marks. Each question carries one mark. Part B carries 20 marks. Each question carries two marks. Part C carries 40 marks. Each question carries five marks. In Part D D 1 carries 10 marks and D 2 carries
10 marks. Each question of D 2 carries five marks.
iv) Write balanced chemical equations and draw diagrams wherever necessary.
PART - A
Note : i) Answer all the 10 questions.
ii) Questions have to be answered in one word or in one sentence each. Each question carries one mark.
10 x 1 = 10
1. Name the metal used in the desilverization of lead by Parkes process.
2. Name the transition metal in 3d series which shows maximum oxidation state.
3. Write Arrhenius equation.
4. Write the formula of conjugate base of NH 3 .
5. How does entropy of universe vary in a spontaneous process ?
6. What is the dispersed phase present in milk ?
7. Name the gas liberated when ethylamine reacts with nitrous acid.
8. What is a polysaccharide ?
9. Give an example for a drying oil.
10. Write the Zwitterion structure of Glycine.
Note : i) Answer any ten questions.
ii) Each question carries two marks. 10 x 2 = 20
i) H 2 S
ii) CH 3 COONa
iii) KNO 3
iv) NH 4 OH.
17. Write any two differences between ideal and non-ideal solutions.
18. Derive Ostwalds dilution law for weak electrolytes.
19. Explain why methylamine is a stronger base than ammonia.
20. What is a racemic mixture ? Give one example.
21. How do you convert methane to ethane ?
22. What is Clemmensens reduction ? Write its general equation.
I. Answer any two of the following questions : 2 x 5 = 10
23. a.) Explain the manufacture of potassium dichromate ( K 2 Cr 2 O 7 ) from chromite. Write the equations involved. 4
b) Name the type of isomerism exhibited by the following pair : 1
Cl and
Br 2 .
Pt NH Cl
24. a) Explain the reactions taking place in the extraction of cast iron
at (i) zone of combustion, (ii) zone of reduction, (iii) zone of
slag formation of blast furnace. 3
b) Write two uses of Helium. 2
25. a.) Explain the formation, geometry and magnetic property of
4 -
[ Fe ( CN ) 6 ] on the basis of valence bond theory. 4
b) Name the noble gas that does not occur in air. 1
II. Answer any three of the following questions : 3 x 5 = 15
26. a) How is phenol manufactured by cumene process ? 3 b) How does acetic acid react with PCl 5 ? Write the equation. 2
27. a.) Explain the mechanism of chlorination of benzene. 3
b) What is carbylamine reaction ? Write the chemical equation
involved. 2
28. a) Write the Haworth structure of a-glucose. 2 b) Write the postulates of Baeyers Strain theory. 3
29. a) Explain Wurtz reaction with an example. 2
b) Explain refining of oil. 2
c) Name the reagent used for dehydrohalogenation reaction. 1
30. a) Derive an expression for the velocity constant of a first order reaction. 4
b) Define radius ratio in an ionic crystal.
1
31. a.) 18-2 g of urea is dissolved in 100 g of water at 50C. The lowering of vapour pressure produced is 660 Pa. The vapour pressure of pure water at 50C is 12260 Pa. Calculate the molecular weight. 3
b) Calculate the number of particles present in a body centered cubic unit cell. 2
32. a.) What is Brownian movement ? How is it caused ?
2
b) Explain the application of common ion effect and principles of solubility product in the precipitation of second group Basic radicals. 3
33. a) A buffer solution contains 0-1 M NH 4 OH and 0-15 M NH 4 Cl.
Calculate the pOH of the buffer solution.
4
(
)
Dissociation constant of NH . OH = 1-8 x 10 5
b) What is a Lewis acid ? 1
34. a) The value of equilibrium constant Kp for a reaction is found to
be 1-06 x 10 5 at 298 K. Calculate A G o of the reaction at the same temperature. 2
b) What is electrochemical series ? Mention any two applications of electrochemical series. 3
IV. Answer any one of the following : 1 x 10 = 10
35. a) Write any four assumptions of molecular orbital theory. 4
b) What is the biological importance of Insulin ? How many amino acid units are present per molecule in Insulin ? 2
c) Explain Kolbes reaction. 2
d) Calculate the [ H + ] and [ OH - ] in 0-001 M HNO 3 solution.
2
36. a) Define the following terms : 2
i) Dialysis
ii) Tyndall effect.
b) What is a Pseudo first order reaction ? Give one example. 2
c) Write the energy level diagram for the formation of Li 2 molecule. What is its bond order ? Predict its magnetic property. 3
d) Explain the mechanism of Cannizzaros reaction. 3
V. Answer any two of the following : 2 x 5 = 10
37. a) How is p-bromoacetanilide prepared from acetanilide in the
laboratory ? 3
b) Explain Biuret test. 2
38. Describe an experiment to study the effect of temperature on the rate of the reaction between potassium persulphate and potassium iodide. 5
39. For the estimation of ferrous ammonium sulphate using standard potassium dichromate solution
i) write chemical equation for the reaction involved.
ii) give the equivalent mass of ferrous ammonium sulphate.
iii) name the indicator used.
iv) what is the colour change at the end point ? 2 + 1 + 1 + 1
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