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10 CHEMISTRY TODAY | JANUARY '06

Q h M S ) C B S E ) f D P M T ) A F M C ) f v M M C ) (EAMCET) (WB-JEE) ( B H U ) ( C M C )

2006 Medical Entrance Exam

{ U P C P M T )

fCET Karnataka]

Practice Test Paper

(Manipal PMT)

( J I P M E R ) (MP PMT) ( M G I M S ) ( P M P T B i h a r ) (PMT H a r y a n a ) ( K e r a l a PMT ) ( R a j . P M T j f T N P C E E )

1. Iodised table salt contains 7.6 x IO-5 g of KI per gram of NaCl. The concentration in ppm of KI is (a) 76 (b) 152

2. The heat of combustion of ethane, hydrogen and graphite are -33.0, - 68.5, - 9 4 K cal/mole, the heat of formation of ethane would be

(a) -188 K cal/mole (b) -383.5 K cal/mole (c) -350.5 K cal/mole (d) +53.5 K cal/mole.

3. A compound A'reacts in the following ways.

BaC12 (aq)^

X(aq)

yellow precipitate

NaOH (aq) brown precipitate

white ppt.

I

3 (aq)

\

colourless solution The compound X is likely to be

(a) Pb(N03)2 (b) CaCr04

(c) Ag2S04 (d) AgN03. 4. Holmes signal makes use of a mixture of (a) calcium carbide and calcium chloride (b) calcium carbide and sodium phosphide (c) calcium carbide and calcium phosphide (d) calcium chloride and sodium phosphide.

5. The oxyacid of phosphorus that has some reducing property is

(a) H3P04 (b) HP03

6. Portland cement contains the following amount of CaO.

(a) 5-15% (b) 20-35%

7. The ether that undergoes electrophilic substitution reaction is

(a) CH3OC2H5

(b) C6H5OCH3

(d) C2H5OC2H5.

8. Predict the final product B in the sequence of reaction.

3 0 % H , S 04

CH = CH „ 4> A > B

H g S 04 N a O H

(b) CH3COOH

(d) C H3- C H - C H2- C H O OH

(a) CH3COONa (c) CH3CHO

9. An organic compound with the formula C6H! 206

forms 20% a yellow crystalline solid when treated with phenylhydrazine and gives a mixture of sorbitol and mannitol when reduced with sodium. Which among the following could be the compound?

(a) fructose (b) glucose (c) mannose (d) sucrose.

10. Caprolactum polymerises to give (a) terylene (b) teflon (c) glyptal (d) nylon-6.

11. The SN1 mechanism for the hydrolysis of an alkyl halide to an alcohol involves the formation of (a) carbanion (b) carbocation (c) free radical

(d) pentavalent carbon in the transition state.

12. The relationship between standard reduction potential of cell and equilibrium constant is shown by (a) E°, _{cell '} " log Kc (b) / ^ — - l o g / Q .

0.059

,,, r-o _ 'og

( d ) £ cell

13. Colourless solutions of the following four salts are placed separately in four different test tubes and a strip of copper is dipped in each one of these. Which solution will turn blue?

(a) KN03 (b) AgN03

14. Concentrated H2S04 has a density of 1.98 gm/ml and is 98% H2S04 by weight. Its normality is

(a) 2 N (b) 19.8 N

15. Which of the following reactions occur at the cathode during the charging of lead storage battery?

(a) Pb2+ + 2e~ Pb (b) Pb2+ + S042" PbS04

(d) PbS04 + 2H20 -> Pb02 + 4H+ + S042" + 2e~

16. The number of dative bonds in sulphuric acid molecule is

(a) 0 (b) 1 (c) 2 (d) 4.

17. The correct sequence of decrease in the bond angle of the following hydrides is

(a) NH3 > PH3 > AsH3 > SbH3 ( b ) N H3 > A S H3 > P H3 > S b H3

( d ) P H3 > N H3 > A S H3 > S b H3.

18. Which of the following reactions is not exothermic?

(a) C(„ + 02 t e )- > C 02 t e )

(b) CW + 2 SW. - » C S2 W

19. The favourable conditions for Haber's process are (a) low temperature and low pressure

(b) low temperature and high pressure (c) high temperature and low pressure (d) high temperature and high pressure.

20. A graph plotted between logKvs 1/7"for calculating activation energv is shown by

t

log K

(a)

1/7" • 1 IT •

t

log K (C)

t

log K

(d)

1/7" • 1/7" •

21. The oxidation number of Fe in compound 46

[ F e ( H20 )5N 0 ] S 04 js

(a) +2 (b) - 2 (c) 0 (d) +1.

22. The equivalent weight of sodium thiosulphate (Na2S203-5H20) in the reaction

2Na2S203 + I2 -> 2NaI + Na2S406 is (a) 248 (b) 124 (c) 596 (d) 62.

23. 'Mischmetal' is an

(a) alloy of rare earth elements with Fe and traces of S, C, Ca and Al

(b) alloy of rare earth elements with Cu and traces of S, C, Ca and Al

(d) alloy of transition elements with Ca and traces of S, C, Ca and Al.

24. In the reaction,

[A] ^Br,/P ^{* [ S ]} [C] ^{- H B r .} -co.

( C5H1 0O2) contains an (No geo.

[D]

(alkene)

(E) and (F) are

asymmetric isomerism) carbon

ozonolysis > ^ ^ [yr]

(positive (negative S c h i f f s test) S c h i f f s test)

O II (a) HCHO and CH3 - C - C2H5

O II (b) HCHO and CH3 - C - CH3

C H

(d) none of these.

25. The amount of NH3 and NH4C1 required to prepare a buffer solution of pH = 9, when

(pKh for NH3 = 4.7, log2 = 0.30) (a) 0.2 mol/lit and 0.4 mol/lit

(b) 0.4 mol/lit and 0.2 mol/lit (c) 0.2 mol/lit and 0.2 mol/lit (d) 0.2 mol/lit and 0.02 mol/lit.

26. Ka for ascorbic acid (HASC) is 5 * 10~5. Then the value of [H+] in an aqueous solution in which the concentration of ASC~ ions is 0.02 (M) will be (a) 5 x 10~7 (b) 5 x IO"9

CHEMISTRY TODAY | DECEMBER '05 47

27. The increasing order of thermal stability for oxyhalide anion/the salts of CIO", C102", C103", C104" is as follows.

(a) CIO < ClOY < C103- < C104 -(b) c i o - > c i o2- > d o , - > c i o4 -(c) CIO" > C104- < C102 < CIO3-(d) C104" > C102- > CIO- >

CIO3-28. Which of the following will displace Br, from an aqueous solution containing bromide ions?

(a) Cl2 (b) I3

-(c) I2 (d) Cl".

29. Ionic solids with Schottky defects contain in their structure

(a) equal number of cationic and anionic vacancies (b) anionic vacancies and interstitial ions

(d) cationic vacancies and interstitial cations.

30. Which one of the following pairs of atoms or ions will have identical ground state electronic configuration?

(a) Li+ and He" (b) Cl" and Ar (c) Na and K (d) F+ and Ne.

31. A compound is treated with NaNH2 to give sodium salt. Identify the compound.

(a) C2H, (b) C6H6

32. Chlorobenzene reacts with Mg in dry ether to give a compound (/I) which further reacts with ethanol to yield

(a) phenol (b) benzene (c) ethyl benzene (d) phenyl ether.

33. Benzene reacts with n-propyl chloride in the presence of anhydrous A1C13 to give

(a) 3-propyl-l-chlorobenzene (b) /7-propyl benzene

34. At 90°C, pure water has [H+] = IO"6. What will be the value of Kw at 90°C?

(a) IO"12 (b) IO"11

35. A solution of potassium bromide is treated with each of the following. Which one will liberate bromine?

(a) hydrogen iodide (b) sulphur dioxide (c) chlorine (d) iodine.

36. If a 0.1 molar solution of glucose (mol. wt. = 180) and a 0.1 molar solution of urea (mol. wt. 60) are placed on the two sides of a semipermeable membrane to equal heights, then it will be correct to say that

(a) there will be no net movement of solutions across the membrane

(b) glucose will flow across the membrane into urea solution

(d) water will flow from urea solution into glucose solution.

37. The reaction of toluene with chlorine in presence of ferric chloride gives mainly

(a) «-chlorotoluene (b) benzyl chloride (c) o- and p- chlorotoluene

(d) benzoyl chloride.

38. A solution containing ammonium chloride and sodium nitrite on boiling produces

(a) ammonia (b) nitric oxide (c) nitrogen (d) nitrous oxide.

39. In the manufacture of bromine from sea water, the mother liquor containing bromides is treated with (a) carbon dioxide (b) chlorine

40. When chlorine is passed over dry slaked lime at room temperature, the main reaction product is (a) Ca(C102)2 (b) CaCl2

41. In a molecule of carbon tetrachloride the four C - Cl bonds are directed towards the corners of a (a) square (b) tetrahedron

42. Cu2+ and Ag+ are both present in the same solution.

To precipitate one of the two ions and leave the other in solution, we shall add

(a) HCl (fl?) (b) NH4N03 (aq)

43. The root mean square speeds at S.T.P. of molecules H2, N2, 02 and HBr are in the order of

(a) N2 > 02 > HBr > H2

(b) 02 > N2 > H2 > HBr (c) HBr > 02 > N2 > H2

(d) H2 > N2 > 02 > HBr.

44. Which one of the following carboxylic acids will have lowest acidic strength?

(a) BrCH,COOH (b) CH3COOH (c) CHjCHCICOOH (d) ClCH2COOH.

45. The hydrolysis of PC13 produces (a) (H3P03 + HCl) (b) (PH3 + HCIO) (c) (H3P03 + HCIO) (d) (H3P04 + HCl).

46. Calcium carbonate decomposes on heating according to the equation : CaC03 = CaO + C02. At S.T.P. the volume of C 02 obtained by thermal decomposition of 50 g of CaC03 will be

(a) 22.4 litres (b) 44 litres (c) 11.2 litres (d) 1 litre.

47. 12.5 ml of a gaseous hydrocarbon were mixed with 100 ml of oxygen and exploded. After cooling the residual gas occupied 68.75 ml. The volume was further reduced by 50 ml by passing the gases in KOH solution and the remaining gas was oxygen. The molecular formula of the hydrocarbon is

(a) C2H6 (b) C4H8

48. Two containers A and B contain the same gas. If the pressure, volume and absolute temperature of gas in A are two times as compared to those in B and if density of gas in A is d, then density of gas in B is (a) d/2 (b) d

(c) 2d (d) 4d.

49. XC + THN03 C 02 + N 02 + H20. The value of X and Y to balance this equation is

(a) X=4, Y= 3 (b) X= 3, 7 = 4 (c) X=4, 7 = 1 (d) X = 1, Y = 4.

50. The compound which gives the most stable carbonium ion on dehydration is

(a) 2-methyl-l-propanol (b) 2-methyl-2-propanol

SOLUTIONS 1. (a) : 7.6 x 10'5 g in one gram

= 7.6 x 10~5 x 106 = 76 ppm.

2 ( g )' AH = - 3 3 . 0 Kcal/mol

2. (c) : C2H6 w + - 02 (g) -> 2C02 + 3HzO ... (i) H2(g) + 2I 02(g)- H²0 ;

AH = -68.5 Kcal/mol c (.«) + °2^(g) c o2 fe)

AH = - 9 4 Kcal/mol

Heat of formation of ethane is given by

... (ii) ... (iii) 2C _(.V) 3H20 (,,) —» C2H6 (g), AH, = ?

The above equation can be obtained by multiplying equation (ii) by 3 and equation (iii) by 2, and then subtracting (i) from the resultant equation (iv).

[H2 fe) - 01 2 to H20 ; AH = -68.5] x 3 [C w + 02 to - » CP2 to ; = -94] x 2 2C (,, + 3H' (s) T J n2 (g)2 + 3 - 0 1 J 21 w2 <g) 2 (s) 3H20 (x) + 2CO:

AH = -383.5 Kcal/mol

2 (g) ... (iv) 3H20 + 2COz —> C2H g + — 02; AH= +33 Kcal/mol 2C w + 3H2 w -> C2H6^y, AW" = -350.5 Kcal/mol.

3. (d) : Reaction with KI and NaOH indicate that cation is Ag+.

i.e. Ag+ + KI —> Agl + K+ yellow ppt.

Ag+ + NaOH AgOH + Na+ brown

Reaction with BaCl2 indicate that anion is either S042^ or N03" as white ppt. may be formed due to BaS04 or AgCl. However, AgCl is soluble in NH3 and not BaS04, so X is AgN03.

4. (c)

5. (c): Oxyacid in which P is in low valent oxidation state can act as reducing agent.

Oxidation state of P in H3P04 = +5 Oxidation state of P in HP03 = +5 Oxidation state of P in H3P03 = +3 Oxidation state of P in H4P207 = +5

As oxidation state of P in H3P03 is +3, hence it can be oxidised to +5, thus shows some reducing behaviour.

6. (c) : Composition of Portland cement is CaO - 60%, Si02 - 22.5%, A1203 - 7.5%, MgO - 2.5%, Fe203 - 2.0%, K20 - 1.5%, S 03- 1.0%, Na20 - 1.5%.

% SiO-, Essentially,

% AI2O3

% CaO

• = 2.5 to 4.0

% SiO, + %A1,0, + %Fe,0, - = 1.9 to 2.1

4 8

7. (c) : Aromatic ring undergoes electrophilic substitution reaction due to rich Jt-electron cloud in the ring.

CHEMISTRY TODAY | DECEMBER '05 47

8. ( D ) : C H = C H ^{3 0 % H}*S (S CH,CHO HgSQ4

9. ( a ) : CH,OH C = o I I (CHOH)3

CH2OH fructose

C H , - C H - C H , C H O

O H B (aldol)

C H = N N H CSH5

C = N N H Q H ,

( C H O H )3

CH2OH

fructose osazone (yellow)

C HI 2O H

> H - C - O H + H O - C - H CH2OH

[H]

( C H O H )3

CH2OH sorbitol

10. (d)

11. (b) : S^N1 mechanism.

(CHOH)3

CH2OH mannitol

> R+ + X~ > RQH+X"

(carbocation) 12. (b) : AG = -nFE

Cell reaction at equilibrium has AG = 0.

This means, nFE = 0 or, E = 0.

Consider a reaction,

Zn + Cu2+ ^ Zn2+ + Cu, .-. K = [Zn2+] [Cu2+] As only ions are present in solution, then

E-E° + 3 L] o g I C O

ce" nF g c [Zn2+]

eeU nF [Zn2+] nF [Cu2+] RT, ,„ 2.303/?7\

£0ce.i = — log. K = — log10 K nF nF

£ ° c e „ = ^ l o g , o ^ ( a t 2 9 8 K ) n

Also, nFE° = RT logeK or, -AG° = RT logeK.

13. (b) : Cu + 2AgN03 Cu(N03)2 + 2Ag colourless green

As, Ag is below the Cu in electrochemical series, hence

it is reduced to Ag. Cu is oxidised to Cu:" ion.

98 g H,S04

14. (c) : 98% H2S04 by weight means = 1 0 0 g w a t e r

Volume of solution = 100 100 N,

d 1.98

g eq. of H2SQ4 98

"2S°4 volume of solution 49x100 1.98x1000 JVH2so4 = 19.8 x 2 = 39.6

15. (d)

O H

16. (a) : 0 = S = 0

OH I

17. (a) : This is due to decreased bond-bond repulsions as electronegativity of X decreases.

18. (b) : All combustion reactions are exothermic.

19. (b) : Formation of NH3 proceeds with decreasing of moles of products, hence pressure decreases. It is an exothermic reaction. According to Le-Chatelier principle, to counter the physical changes during reactions, high pressure and low temperature is required. However, at very low temperature rates of reaction decreases considerably, hence reaction is carried out at optimum temperature at the expense of yield.

20. (a) : In K = A + j or, 2.303 log K = A + j log K vs — is linear with a positive slope. 1

21. (a) : Oxidation number of Fe in compound [Fe(H20)5N0]S04 will be as follows

-x + (0 x 5) + (0 x 1) + 1 x (-2) = 0

=> x = +2.

Hence, oxidation state of Fe in compound [Fe(H20)5N0]S04 will be +2.

22. (a) : The molecular weight of hydrated sodium thiosulphate (Na2S203-5H20) is 248.

From reaction, 2Na2S203 + I2 2NaI + Na2S406

it is clear, that change in oxidation number = 5 - 4 = 1 mol. wt.

Now, E (Na2S203) = c h a n g e i n 0.N

248 248 5 - 4 1 = 248.

CHEMISTRY TODAY | DECEMBER '05 47

23. (a) : 'Mischmetal' is an alloy of rare earth elements with iron and traces of S, C, Ca and AI. It is used to improve the workability of steel.

24. (b) : The reaction is

C I S CO + HCHO <°ZON°'YSIS C H 3> C = CH2

X CH, 2

CH3

(F) ^(E) - c o2

(D) CH,

CH C = CH.COOH 4 ^HBr Br ( Q

C H3 V I

> C H . C H C O O H CH,

J (S)

CH. ^>CH.CH2COOH (A)

O Hence (E) and (F) are HCHO and CH3 - C - CH3. 25. (a) : Let the concentration of NH4CI (salt)

= x mol/lit .'. Concentration of NH3 (base) = 0.6 - x

[salt]

[base]

x For alkaline buffer, pOH = pKh + log]0

5 = 4.7 + log|0 * => 0.3 = log]0

(0.6- x)

=> logl0 2 = log,0 ——^ => 2 = — ^ 0.6-x 0.6 -x

=> x = 0.4

.-. Concentration of [NH3] = 0.2 mol/lit.

and concentration of [NH4C1] = 0.4 mol/lit.

-14

0 . 6 - x

A' 1x10"

26. (b) : Kh =

Ka 5x10"

Hydrolysis reaction, ASC~

At equilibrium (0.02 - x)

= 0.02

Now by applying the formula,

= 2x10"

HA + OH-x

K,=- 2x10"

=-0.02 =-0.02 =-0.02

=> x2 = 2 x IO"10 x 0.02 = 2 x IO"10 x 2 x io-2

=i» x2 = 4 x IO"12 => x = 2 x 10"6

=> [OH-] = 2 x 10-6. ... [ H +] = l i l i ^ - = 5xlO-9.

2x10"

[Since, [H+] x [OH"] = 1 x IO"14].

27. (a) : As, the thermal stability of both the acids and their salts increases with the increasing order of oxidation

5 0

state of halogen or with the increase of the number ol oxygen atoms.

So, the correct order of thermal stability for oxyhalide anions CIO , C102- C103", C104~ is as

cio- < cio²- < cio³- < C10⁴ .

28. (a) : Cl2 + 2 B r 2CL + Br2

29. (a) : Such a defect which involves a cation and anion valency in the crystal lattice is called Schottky defect.

30. (b) : Both having the same number of electrons.

i.e., 18 electrons.

31. (a) : Because, acidic hydrogens are present in acetylene.

32. (b) : C6H5C1 + Mg d r y e t h e r > C6H5MgCl (A) C2H5OH + C6H5MgCl C6H6 + Mg

33. (d)

(benzene)

A1C1,

+ CH3CH,CH2C1 ^

OC2HS

a

^CHC H - C H , ^I³³ + HCl

34. (a) : As [H+][OH"] = Kw

But, [H+] = [OH-] = 10"6

[10 6][10-6] = IO1 2 =

35. (c) : Because, chlorine is more electronegative than bromine. Therefore, it can replace bromine in KBr.

2KBr + Cl2 2KC1 + Br2

36. (a) : Such solutions are said to be isotonic.

38. (c) : NH4C1 + NaN02 N2 + NaCl + 2HzO 39. (b) : 2KBr + Cl2 2KCI + Br2

40. (c) : Ca(OH)2 + CI2 CaOCI2 + H20

41. (b) : In carbon tetrachloride covalent bonding involves sp3 hybridisation. So C - Cl bonds are directed towards four corners of a tetrahedron.

CHEMISTRY TODAY | DECEMBER '05 47

42. (a): Silver will be precipitated in 1 st group as silver chloride on addition of HCI.

43. (d): Because, the root mean square speed is inversely proportional to the square root of molecular weight.

44. (b): Presence of halogen in the alkyl chain enhances the acidic strength by increasing the ionisation of carboxylic group due to inductive effect.

45. (a) : Hydrolysis o f P C l³

-PC1, + 3HOH H³P0³ + 3HC1.

46. (c) : CaC0³ = CaO + CO,

(40 + 12 + 48) g 22.4 litres at STP v 100 g CaC0³ produces 22.4 litres C0² at STP

.'. 50 g CaC0³ will produce 11.2 litres C 0² at S.T.P.

47. (c) : Volume of hydrocarbon taken = 12.5 ml Volume of oxygen taken = 100 ml

Volume of C0² produced = 50 ml

Volume of oxygen left = (68.75 - 50.00) ml = 18.75 ml Volume of 0² reacted with hydrocarbon

= (100 - 18.75) = 81.25 ml

Let the f o r m u l a of the h y d r o c a r b o n be C^X¥L^Y C H , + x O , - > X C 0²+ ^ H²0

1 vol vol x vol

12.5 m l 12.5| x + ^ | m l 1 2 . 5 * ml

5 0 „

Here, 12.5.x = 50 115

Again, 12.5| x + ^ ( = 81.25

12.5| 4 + ^ | = 81.25 = 10

Therefore, formula of the hydrocarbon = C4HI 0. 48. (b) : PA = 2PB, d^A = d, TA = 2TB, VA = 2VB, d^B = ? As, we know that —P P ^j— = ——

d,7] a2T2

2 PR . - J j L

dATA dBTB

d^H = d.

d x 2 Tb dBTB

49. (d) : By trial and error method, we can get x = 1 and y = 4.

50. (b)

W l - f c G -

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