Pre University Board 2010 P.U.C Physics, Chemistry, Maths - exam paper
Code No. 34
Total No. of Questions : 39 ]
Total No. of Printed Pages : 16 ]
March, 2010
( Kannada and English Versions )
Time : 3 Hours 15 Minutes ] [ Max. Marks : 90
( Kannada Version )
: i)
ii) - A, B, C d0t D 0> d,4rt>0 d>,aFrt>
' * 77 -0 cn y c c o*
_D
iii) - A 0 d,4 odX, 00 oXdot 10 odrt>, - B 0
d odX@ 2 oXdot 20 oXrt>,
odX, 5 oXrt>ot 40 oXrt> - D 0 D , 10
6 co 1 *
oXrt D 2 mrtd d,4 odX, 5 odn>ot 10 odrt$d0td.
2 co y ct TfT -0
iv) nt6>d0d, odrod d0t ,&0eXdrart>0 d00.
C 0
- A
0> 10 d,4jn>0j t ob.
: i) ii)
co y ct _o
drtrt od ddd od dd tdn>0t d0ed0. d, d;4rt) od od>d0td. 10 x 1 = 10
y y -e
1. Zn 2 + z </d a yeid rt0rad teoj&td ?
2. aedd tofi <0 aed} >dd< /d 4,ed >< p4ed}
3. o dooodo<o O,d>rt 600C Jio d<oo TO,3<oad
co aO ot, cp rs co
3/o<o ,aoeddrao wd oO.
4. oo &&d a,rtdo pH = 1 do >dra 25C 3(o >Arf.
6 ~y ot ~ ZJ co rococo
5. oo 3/o<o rto}>od 2. d ao ?
6. X,d (ca</) aedo ort$,o d* d<>eA,odo. ydra da.
7. d>A ,aoeddra o3, 3j, ( B ) oo. ,O&.
CO > sJ ci ' ' c
9. 0 yb,n >o wo&dfi 'di)edoOS' Orasdo ,O&.
10. CH 3 N CH 3 d IUPAC ,doR WdoO.
CH
- B
ii) <>oo o 0do odrt>oct oado3rf.
11. odo.roy wd,, d}rt ,ooa 0 on.dj* dezd.oo a. 0 oTO.dj*
6 co6 oOkct co6
X\o , ><oao dodorOs wdo d&r, oo
12. ,oo oo ndd}oart aOb.
13. ,<305 w4 ,es<3o Xed oo 4Pidb<oo dXoel d>rt> aorarfoart ert roJrf ? ,aoeXdra Xs.
14. sd r oXe," dd doO.
15. oo raoj {aoeo ,/ortJobR 3e0,o esd arort 3$b.
16. des' Ji, 0odeo ? oo 0}<o des' Ji, o3,eo ?
6 rs 6 oi
17. s N 1 oo s N 2 3//> a,n> oa </4dd 0do 63D6,rt>OR xs.
18. 25C oo dd,d<oaX &<o<o 5ooX 3 d}<oo 100 kJ wAd,
co ZS _o _o co
e 3dS w dd,d<oaX 3,<o<o ,ob 3 b odoXo d3.
co cp cp ct -o
19. bebo Xed &X Xe do doO. w ;,X,do doo </>a ,ooe ,oZ6 0o ?
20. ,orar ,oZ6oor rozdab. oo & ,orar ,oZ6rt>o 0o ?
21. i) ddcj wa ,deX\ Xo a<ooo ad&b.
ii) wr odra 0odeo ?
22. M 1 | M 1 + || M 2 + | M 2 o oo ndas* Xe oJrf. Xe oo fX 3,<o oo Xe dorto doO.
- C
I. <d/>dad 0do JO& : 2 x 5 = 10
23. a) ' aaao ea/o. ert sapodo ? 3
b) SodXdo a<dooR oo ad}doart aO. 2
24. a) ,o<d>e&X o SjotoJOr efi&, Xoeaoo /a ,oXdra o J {aaoeido wyado aO. 3
_D c
b) -aj,e oJ -aS aaao e aort aora na$oo ert
,J.eS,o3a d ? 2
y t -o
25. a) deeo oX@ dyaj a< djdoart aO. 3
b) naora (,o<Ar) 0odeo ? aoe naraM oo ad} Xs. 2
II. X> Ad)n>, <d/>dad odo JO : 3x5=15
26. a) doea ,de 3/d/Jo adO. 3
b) ||h,,d(jrart>odeo ?
1
c) sade-wdn wd@e" sdrtaA o&od/raod 3;<do<do
, aoeXdrao aron>oan doO. 1
27. a) Xe 0ode ? Xe ,>Jdo OX, a>3. 2
e) co co u
b) wd doo oeoS" wdo,rt> adeX weo sadra dOft. 2
c) o 0ode ? 1
28. a) x> a dad}rt>o en d/doo 0o ,oeXdradoart
ot
d Oft :
i) a-Sdea? <, wdO saars* wdd eaoo <d ra doo wO@ad oradaA
ii) 3leo de5aF wA 4 b) 4g)en> djiQw aXeXdra 0ode ? 1
29. a) X> A dn> O ert J/O,oo ?
i) e<DR oa0ao
ii) satraps* wdd o wdes? |<0ao 4
b) o nXe," raod) 5 raad rtoortO oad 0oo JeO,co oo da,aDX a/ooo Xa. 1
III. X> Ad)rt>0 /d)ad odo jOft : 3x5=15
30. a) & && X o6 n d doJOo 5aoraadO oda
do<X dOft. 3
b) 4 woeo*n> ao6JoOi 20 >od ,Jd ,0/1 oa,dra do<X aftart 0Oi ,Jo endrartorf ?
(,Jo> ,d/ d6oa& = 3286) 2
31. a) oo 3,d/4rtF S/dodoo 20% Adoo 5 ,Xod
n5X>o. S/dodoo 60% 04Dj odo
3noX>o,d)o 0OD d@ aS. 3
b) 4s|j{e4* 0OdeD ? oo ad}dooR Xs. 2
32. a) L, 4JedJa aaQo oo oaadoad S/dodo S/d/driF
doosdood aa4o adOft. 2
b) ,aoeddra4 o ddoO. ,aoeddra4o 4deftft oo S/dodo 3)d/ aJdoo ert ? 2
c) a, 0odeo ? 1
33. a) ,a4/, d/ 4O}a4o 4oJ aeJa rtora JJ.rto, 4d>eAft
6 -c cp d <=i
0d rtoo& 4,3a,ao edo oa,Sdc*rt> J OoaXdoo adOft. 3
.> 6 co 6 -> t,
b) da.za.aft :
ii) {a<d 2
34. a) 4,4o 3/d/4rtF S/dodo 4ert adoJaod eddrado aaft. 3
b) 25C y aeO wa J4 238 ao.aoe. dad&da0, 100 na,o j&Xe, (raoJd = 342) oo S. nap aeO<, ddftftart oiartod wa J Xdoy d, aS. 2
_0 tr
1 X 10 = 10
35. a) i) Sc 3 + (d d/rai ,0Z6 = 21)
Cr 3 + (dd/rai ,oZ6 = 24) , d)n> </>rt
aX? 2
1
3
b) X<,co ooaod ert ?
c) i) pH = 57 do o 3&,X 3zO,ro>rt ,eS<o &lel
n> ,3d3 XooSO.
_0 CO _D c
(5* K q = 1-8 X 10 - 5 )
3
ii) 0Ole&R Zn).
1
36. a) i) iKOs6" dPI&o eraoQrt ert
0o ,aoeXdraoart aO. 2
_D
ii) |i*ao Xra O,ro>rt eXr
,O&. 1
0 a,Q,m&, > o3 0d /3rt>o
CO >&5> cp y ct
o oe" raoa _ .o d 0d5
,aoeXdraoan ao. 2
n 0odn>0 ?
dDO.
b) i) ii)
c) i)
S
1
2
ii) aod) 25C 3(0, 0125 wd, 001 M s
pH XoiSO.
2
D
2
V. X> Ad)rt> <zd3d> 0do JO : 2x5=10
37. a) laadpaod p-ee&iaadra Or enaood J</O,o aa o arfO& 3
b) Selert >Or Xorao&soo oo OeXR Xs. OeX\o ,deo ? 2
38. 4Pia<oo ddjei oJ 4Pia<oo <>ra,)rart> raora S/oo
S,/en oed Jo Oraaoo JeO, aO. 5
39. oo raaoed nara,dO d,? eaoo d/l ra da5oO pia&oo raoel a ra o eA& Xorao&soo aa Or arfO& dY raoo oa,a<oaX Sjoo ,aoeXdrao Xs. 5
( English Version )
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. What type of magnetic behaviour is shown by Zn 2 + ion ?
2. Name the noble gas which is not adsorbed by coconut shell charcoal in Dewars charcoal adsorption method.
3. Write the equation for the chemical reaction taking place at 600C in the extraction of iron by blast furnace.
4. The hydrogen electrode is dipped in a solution of pH = 1 at 25C. What is the potential of the electrode ?
5. Temperature coefficient of a reaction is 2. What does it mean ?
6. Alum is used in the clarification of the muddy water. Give reason.
7. Name the end product ( B ) of the following reaction :
( CH 3 COO , 2 Ca dlstillati" - A N 2 - B
8. Write the structural formula of proline.
9. Name an electromeric effect which involves partial displacement of electrons.
10. Give the IUPAC name of
CH 3 N CH 3
CH 3
Note : i) Answer any ten questions.
ii) Each question carries two marks. 10 x 2 = 20
11. Draw Ellingham diagram for the formation of mercuric oxide. With the help of Ellingham diagram, suggest a method for the reduction of mercuric oxide.
12. Explain linkage isomerism with an example.
13. How does concentrated sulphuric acid react with a mixture of sodium chloride and potassium dichromate crystals ? Give the equation.
14. Write Haworths structure for sucrose.
15. Mention the conditions for a molecule to show geometrical isomerism.
16. Define iodine value. What is the significance of iodine value of an oil ?
17. Give any two differences between S N 1 and S N 2 mechanisms.
18. The standard free energy change of a chemical reaction is 100 kJ at 25C. Calculate the equilibrium constant of the chemical reaction at the same temperature.
19. Sketch the unit cell structure of caesium chloride. What is the coordination number of each ion in the crystal ?
20. Define the term Gold number. What are the Gold numbers of gelatin and starch ?
21. i) State Raoults law of relative lowering of vapour pressure. ii) What is an ideal solution ?
22. A galvanic cell is represented as M 1 | M 1 + || M 2 + | M 2 .
Write the half-cell reactions and cell reaction for the above cell.
I. Answer any two of the following questions : 2 x 5 = 10
23. a) How is ammonia manufactured by Habers process ? 3 b) Explain with an example Nernsts distribution law. 2
24. a) With the help of valence bond theory, explain the hybridisation
and geometrical shape of cuprammonium ion. 3
b) How is a mixture of noble gases isolated from air by Ramsay and Rayleigh method ? 2
25. a) Explain, with a diagram, electron gas theory of metallic bond. 3 b) What is a ligand ? Give an example of a bidentate ligand. 2
II. Answer any three of the following questions : 3 x 5 = 15
26. a.) Explain the mechanism of sulphonation of benzene. 3
b) What are triglycerides ? 1
c) Write chemical equation with conditions for the formation of alkane nitriles from haloalkanes. 1
27. a) What is angle strain ? Calculate the angle strain in cyclopentane.
2
b) Giving reason, explain the relative acidity of ethanoic acid and methanoic acid. 2
c) What is a peptide bond ? 1
28. a) Explain with equations how to convert
i) aldehyde containing no a-hydrogen to a mixture of sodium salt of the carboxylic acid and alcohol
ii) ketone into hydrocarbon. 4 b) What is denaturation of proteins ? 1
29. a) How are the following prepared ?
i) Ethanol from methanol
ii) Carboxylic acid from alkane nitrile. 4
b) Give a chemical reaction to show that a molecule of glucose contains five hydroxyl groups. 1
III. Answer any three of the following questions : 3 x 5 = 15
30. a) With a neat diagram, explain the construction and working of
standard hydrogen electrode. 3
b) Calculate the mass of zinc metal deposited from zinc sulphate solution by passing a current of 4 amperes for 20 minutes.
( Equivalent mass of zinc = 32-86 ) 2
31. a) A first order reaction takes 5 seconds for 20% completion.
Calculate the time required for 60% completion of the reaction.
3
b) What is peptization ? Give one example. 2
32. a.) Explain Ostwalds isolation method for the determination of the
order of a reaction. 2
b) Write Gibbs equation. How do you predict the feasibility of a reaction using Gibbs equation ? 2
c) What are Lewis bases ? 1
33. a) Explain the application of common ion effect and principles of
solubility product in the precipitation of second group basic radicals. 3
b) Define :
i) Osmotic pressure
ii) Space lattice. 2
34. a) Derive an expression for the velocity constant of a first order
reaction. 3
b) Calculate the lowering of vapour pressure caused by addition of 100 g of sucrose ( molecular mass = 342 ) to 1 kg of water if the vapour pressure of water at 25C is 23-8 mm of mercury. 2
PART - D D 1
1 x 10 = 10
35. a) i) Among Sc 3 + ( Atomic number = 21 )
and
Cr 3 + ( Atomic number = 24 ) , which ion is coloured and
why ?
2
ii) Write the electronic configuration of oxygen molecule. 1
b) How is phenol isolated from coal tar ?
3
c) i) What is the ratio of concentration of sodium acetate to acetic acid while preparing a buffer solution of pH = 5-7 ?
3
(
)
K of acetic acid is 1-8 x 10 5
ii) Define the term entropy.
1
36. a.) i) Explain with equation how concentrated sulphuric acid reacts with potassium bromide. 2
ii) Name the flux used in the extraction of iron from haematite. 1
b) i) Explain with equation of Hoffmanns bromamide reaction. 2
ii) How many n electrons are present in the delocalised electron cloud in a benzene molecule ? 1
c) i) Write any two merits of Arrhenius theory of electrolytic
dissociation. 2
ii) Calculate the pH of a 0-01 M solution of acetic acid if the degree of dissociation at 25C is 0-125. 2
V. Answer any two of the following : 2 x 5 = 10
37. a) Explain the laboratory method of preparation of
p-bromoacetanilide from acetanilide. 3
b) Give a test to detect ketoses. What is the name of the test ? 2
38. Describe an experiment to show the effect of temperature on the rate of a reaction between potassium persulphate and potassium iodide.
5
39. Describe the experiment to determine the mass of ferrous ammonium sulphate crystals present in one dm 3 of its solution by using standard potassium dichromate solution. Give the equation for the reaction involved. 5
|
Attachment: |
| Earning: Approval pending. |
