1. PAPER – I
61. 17g of hydrogen peroxide is present in 1120 ml of solution. This solution is called
(A) 5 volume solution (B) 10 volume solution
(C) 15 volume solution (D) 16 volume solution
62. The density of a gas at 27°C and 1 atm is d. Pressure remaining constant, at which of the
following temperature will its density become 0.75d.
(A) 20°C (B) 30°C
(C) 36°C (D) 127°C
63. Radioactivity of radioactive element remains 1/10 of the original radioactivity after 2.303
seconds. The half life period (in seconds) is
(A) 2.303 (B) 0.693
(C) 0.2303 (D) 0.0693
64. Assuming complete dissociation predict which of the following will have pH = 12.
(A) 500 ml 0.005 M NaOH (B) 1000 ml 0.005 M Ca(OH)2
(C) 100 ml 0.05 M Ca(OH)2 (D) 50 ml 0.05 M NaOH
65. The percentage of metal in its oxide is 60. The percentage of bromine in metal bromide
(oxidation state of metal remains the same) will be
(A) ~ 87 (B) ~ 97
(C) ~ 77 (D) ~ 80
66. Which of the following will be most reactive towards the nucleophilic substitution.
(A)
Br
(B)
OTs
(C)
OH
(D)
OSO2CF3
67. 50g of CaCO3 when treated with 60 ml of 20 N HCl at 300 K and 4 atm produces
(A) 22 g CO2 (B) 44g CO2
(C) 11g CO2 (D) 88 g CO2
68. A certain weak acid has a dissociation constant of 10–5
. The equilibrium constant for its
reaction with a strong base is
(A) 10–9
(B) 10+14
(C) 109
(D) 10–5
69. The species with maximum magnetic moment is
(A) K4[Ni(CN)6] (B) K4[Fe(CN)6]
(C) K3[Co(CN)6] (D) [Cu(NH3)4]SO4
70. Acetophenone on reaction with p -nitroperbenzoic acid gives
(A) phenyl propionate (B) phenyl acetate
(C) methyl benzoate (D) benzophenone

2. 71. OH
is
,
A
4
LiAlH
.
2
TsCl
.
1


 

(A)
OLi
(B)
(C) (D)
Cl
72.
C N
C
H3
Ph OH
are
products
The
.
oducts
Pr
O
H
PCl
3
5


 

(A) PhCOOH, CH3NH2 (B) CH3COOH, PhNH2
(C) 2PhCOOH (D) None of these
73. L1 and L2 are the lattice energies of NaF and CsF respectively and IC1 and IC2 are the ionic
characters of NaF and CsF respectively. Then
(A) IC1  IC2 & L1  L2 (B) IC1  IC2 and L2  L1
(C) IC1  IC2 & L2  L1 (D) IC1  IC2 & L2  L1
74. A compound of vanadium has a magnetic moment of 8 B.M. Hence the vanadium ion is
(A) V2+
(B) V+
(C) V4+
(D) V3+
75. In which of the following solutions AgBr will be maximum soluble?
(A) 10–3
M NaBr (B) 10–3
M NH4OH
(C) Pure water (D) 10–3
M HBr
76. Copper can be deposited from acidified CuSO4 and alkaline CuCN. If 5 amp current is
passed for 5 min through both the solutions separately, which of the following is correct.
(A) The amount of Cu deposited from acidic CuSO4 solution will be higher.
(B) The amount of Cu deposited from alkaline CuCN solution will be higher.
(C) The same amount of Cu will be deposited in both the cases.
(D) It cannot be predicted.
77. The chemical reaction 2O3  3O2 proceeds as follows
O3 O2 + O (fast)
O + O3  2O2 (slow)
The rate law expression for 2O3  3O2 reaction should be [K is rate constant]
(A) Rate = K[O3]2
(B) Rate = K[O3]2
[O2]–1
(C) Rate = K[O3][O2] (D) None of these
78. When CO2 dissolves in water the following equilibrium is established;
CO2 + 2H2O H3O+
+ HCO3
–
For this equilibrium Kc is 3.8  10–6
and pH = 6 at the same temperature. So
]
CO
[
]
HCO
[
2
3

at that
temperature is
(A) 3.8  10–12
(B) 3.8
(C) 6.7  10–2
(D) 13.4
79. Hydrated proton can exist in water as
(A) H3O+
(B) H5O2
+

3. (C) H9O4
+
(D) All of these
80. What will be the product of the following reaction
CH3—CH=CH2 + IN3  ?
(A)
C
H3
CH
CH2N2
I
(B)
C
H3
CH
CH2I
N3
(C)
R
HC CH2
N
I
(D) None
81. Dehydrohalogenation of the following in increasing order
C
H3 X C
H3 CH3
X
C
H3 CH3
CH3
X
I III
II
(A) I  II  III (B) III  II  I
(C) I = II  III (D) III  I = II
82.
OH
CH
NaBH
2
2
B 

 

O
O
O
A
4
LiAlH


 

in the above reaction A and B are
(A)
O
O
O
in both cases (B)
in both cases
OH
OH
OH
(C)
OH
OH
OH
O
O
O
, (D) Formation of A and B is not possible.
83. An organic compound of molecular formula C4H6(A), forms precipitate with ammonical
cuprous chloride. A has an isomer B, one mole of which reacts with one mole of Br2 to form
1,4 - dibromo-2-butene. A and B are
(A) CH3—CH2—C  CH and CH2 = CH—CH=CH2
(B) CH3—CC—CH3 and CH3—CH=C=CH2

4. (C)
H2C
H2C
C=CH2
H2C
H2C
CH
CH
and
(D) H2C
CH
CH2
CH
C
H3 C C CH3 and
84. Coupling with diazonium salts of the following takes place in the order of
O
-
OH NH2 NH3
+
I II III IV
(A) IV  II  III  I (B) IV  III  II  I
(C) II  IV  I  III (D) I  II  III  IV
85. The product X of the following reaction is
O
,
X
HI C
100


 



(A)
O
+
I
-
(B) O
I
(C)
CH2
CH2
I
CH2
CH2
I
(D) I – CH2 – CH2 – I
86. What will be the final product 'B' of the following reaction?


 



 NaOH
O
||
3
3
5
6 CH
C
CH
CHO
H
C A



 

OH
NaOCl
B
(A)
H5C6
CH
CH2
COCH3
OH
(B) C6H5 – CH = CH – COCH3
(C) C6H5CH = CH – COONa (D) C6H5COOH
87. Find the final product Z of the following reaction
Δ
,
EtOH
KCN
SO
H
HNO
FeCl
Cl
Y
X
4
2
3
3
2

 


 


 

(A)
CN
NO2
(B)
CN
NO2

5. (C)
Cl
CN
(D)
Cl
CN
88.
O
CH2
The ether when treated with HI produces.
CH2I CH2OH I OH
I III IV
II
(A) I and II (B) I and IV
(C) I, II and III (D) All the four
89. Which one is the most stable complex, if the equilibrium constants are
(A) 1.0  10–12
(B) 1.0  10–10
(C) 1.0  10–8
(D) 1.0  10–6
90. The basic character of hydrides of the VB group elements decreases in the order
(A) NH3  PH3 AsH3  SbH3 (B) SbH3  PH3  AsH3  NH3
(C) NH3  SbH3  PH3  AsH3 (D) SbH3  AsH3  PH3  NH3

6. Answers
61. A
. 62. D 63. B 64. B
65. A 66. D 67. A
68. C 69. D 70. B
71. C 72. A 73. D
74. D 75. B 76. B
77. B 78. B 79. D
80. B 81. B 82. C
83. A 84. A 85. C
86. C 87. D 88. B
89. A 90. A
Hints & Solutions
61. Weight of H2O2 in 1 ml =
1120
17
Moles of H2O2 in 1 ml =
34
1
1120
17

Moles of O2 liberated =
2
1
34
1
1120
17


Volume of O2 liberated = 22400
2
1
34
1
1120
17


 = 5 ml
62. PM = dRT or d 
T
1
273
27
273
T
d
75
.
0
d
T
T
d
d 2
1
2
2
1





T2 = 127°C
63.
t
0
2
/
1 A
A
log
t
303
.
2
t
693
.
0

Putting the values we get
t1/2 = 0.693
64. pH = 12, pOH = 2  [OH–
] = 10–2
M
65. % of M in MxOy =
y
16
xM
100
xM


= 60  xM = 24y
% M in MxBr2y = 100
y
160
y
24
y
24
100
y
160
xM
xM





 13
 % of bromine in MxBr2y  87
66. 3
CF
||
O
O
||
S
O 


is the best leaving group as it is the weakest base
67. Equivalents of CaCO3 =
100
2
50 
= 1

7. Equivalent of HCl =
1000
20
60
= 1.2
 Equivalent of CO2 = 1, moles of CO2 = 0.5 (n-factor = 2)
 mass of CO2 = 22g
Ka
68. HA + OH–
A–
+ H2O
Kh
Kh = 5
14
a
w
10
10
K
K


 = 10–9
Ka = Kh
–1
= 109
69. Because it has maximum no. of unpaired electrons.
70.
C O
C
H3
Ph
+
PhO2N
C O
O
-
O
C
Ph
C
H3
O
-
O
O
C
Ph
O2N
O
H3C
C
O
Ph
O
71.
OH OTs




H



 
TsCl
+
74. We know magnetic moment of )
2
n
(
n  B.M. V3+
is ‘d2
’ system. So it's magnetic moment is
8 B.M.
75. Solubility of AgBr is maximum in NH4OH due to soluble complex [Ag(NH3)2]Br formation
76. Cu2+
+ 2e  Cu (from CuSO4)
Cu+
+ e  Cu (from CuCN)
So if same amount of charge is passed through both the solution alkaline CuCN will deposit
more Cu.
77. The slow r.d.s gives rate = K[O][O3]
and Kc =
]
O
[
]
O
][
O
[
3
2
or [O] =
]
O
[
]
O
[
K
2
3
c
from this Rate =
]
O
[
]
O
[
K
]
O
[
]
O
][
O
[
K
K
2
2
3
2
3
3
c



= 1
2
2
3 ]
O
[
]
O
[
K 
 [K is overall rate constant]
78. Kc
]
CO
[
]
HCO
][
O
H
[
2
3
3




8. [H3O+
] = 10–6
Since pH = 6
or 6
6
2
3
3
c
10
10
8
.
3
]
CO
[
]
HCO
[
]
O
H
[
K






 = 3.8
79. H+
+ H2O  H3O+
H+
+ 2H2O  H5O2
+
H+
+ 4H2O  H9O4
+
H5O2
+
and H9O4
+
can exist in solid state also
80. IN3 I+
+ 
3
N
81. 1°  2°  3°
82. LiAlH4 reduces keto, aldehyde and even cyclic ester, NaBH4 also reduces keto and aldehyde
but not ester
83. A has acidic H hence CH3CH2C CH
B reacts with one mole of Br2 by 1,4 addition hence CH2=CH—CH=CH2
86. C6H5CHO+CH3COCH3 

 
NaOH
C6H5—CH=CH—COCH3
reaction
Haloform
NaOCl
OH 

C6H5CH = CH – COCH3 + NaCl + CHCl3
87. Cl Cl
NO2


X 

Y
89. Stability constant of a complex ion is the reciprocal of its equilibrium / dissociation constant.
Smaller the value of equilibrium constant, greater will be the stability of that complex.
90. The basic character of hydrides decreases down the group.