Q41. Given below are two statements: Statement I : Nitration of benzene involves the following step - [Figure]
Statement II : Use of Lewis base promotes the electrophilic substitution of benzene. In the light of the above statements, choose the most appropriate answer from the options given below :
(1) Statement I is correct but Statement II is incorrect(2)
(2) Statement I is incorrect but Statement II is correct
(3) Both Statement I and Statement II are correct
(4) Both Statement I and Statement II are incorrect

Q41. The quantity of silver deposited when one coulomb charge is passed through $\mathrm { AgNO } _ { 3 }$ solution :
(1) $1 g$ of silver
(2) 1 electrochemical equivalent of silver
(3) 1 chemical equivalent of silver
(4) 0.1 g atom of silver

Q41. Given below are two statements: Statement I : Gallium is used in the manufacturing of thermometers. Statement II : A thermometer containing gallium is useful for measuring the freezing point ( 256 K ) of brine solution. In the light of the above statements, choose the correct answer from the options given below :
(1) Both Statement I and Statement II are true
(2) Statement I is false but Statement II is true
(3) Both Statement I and Statement II are false
(4) Statement I is true but Statement II is false

Q41. Given below are two statements : Statement I : $\quad \mathrm { PF } _ { 5 }$ and $\mathrm { BrF } _ { 5 }$ both exhibit $\mathrm { sp } ^ { 3 } \mathrm {~d}$ hybridisation. Statement II : Both $\mathrm { SF } _ { 6 }$ and $\left[ \mathrm { Co } \left( \mathrm { NH } _ { 3 } \right) _ { 6 } \right] ^ { 3 + }$ exhibit $\mathrm { sp } ^ { 3 } \mathrm {~d} ^ { 2 }$ hybridisation. In the light of the above statements, choose the correct answer from the options given below :
(1) Statement I is true but Statement II is false
(2) Statement I is false but Statement II is true
(3) Both Statement I and Statement II are true
(4) Both Statement I and Statement II are false
Q42. List - I List - II Reaction Type of redox reaction
(A) $\mathrm { TiCl } _ { 4 }$ (I) $\mathrm { e } ^ { 2 } , \mathrm { t } _ { 2 } ^ { 0 }$
Match List - I with List - II.
(B) $\left[ \mathrm { FeO } _ { 4 } \right] ^ { 2 - }$ (II) $e ^ { 4 } , t _ { 2 } ^ { 3 }$ (III) $e ^ { 0 } , t _ { 2 } ^ { 0 }$ (IV) $\mathrm { e } ^ { 2 } , \mathrm { t } _ { 2 } ^ { 3 }$
(C) $\left[ \mathrm { FeCl } _ { 4 } \right] ^ { - }$
(D) $\left[ \mathrm { CoCl } _ { 4 } \right] ^ { 2 - }$
Choose the correct answer from the options given below :
(1) (A)-(III), (B)-(IV), (C)-(II), (D)-(I)
(2) (A)-(IV), (B)-(III), (C)-(I), (D)-(II)
(3) (A)-(III), (B)-(I), (C)-(IV), (D)-(II)
(4) (A)-(I), (B)-(III), (C)-(IV), (D)-(II)
Q43. [Figure]
(I) [Figure]
(II) [Figure]
(III) [Figure]
(IV)
The correct arrangement for decreasing order of electrophilic substitution for above compounds is :
(1) (III) $>$ (I) $>$ (II) $>$ (IV)
(2) (IV) $>$ (I) $>$ (II) $>$ (III)
(3) (III) $>$ (IV) $>$ (II) $>$ (I)
(4) (II) $>$ (IV) $>$ (III) $>$ (I)

41. (4) & 42. (3) & 43. (4) & 44. (2) \hline 49. (2) & 50. (1) & 51. (5) & 52. (6) \hline 57. (0) & 58. (5) & 59. (591) & 60. (5) \hline 65. (1) & 66. (2) & 67. (2) & 68. (2) \hline 73. (3) & 74. (4) & 75. (4) & 76. (3) \hline 81. (36) & 82. (103) & 83. (5) & 84. (16) \hline 89. (569) & 90. (17) & & \hline \end{tabular}
\begin{tabular}{|l|l|l|l|} \hline 5. (2) & $6 . ( 4 )$ & 7. (2) & 8. (2) \hline 13. (3) & 14. (4) & 15. (2) & 16. (4) \hline 21. (3) & 22. (15) & 23. (7) & 24. (16) \hline 29. (6) & 30. (156) & 31. (3) & 32. (3) \hline 37. (4) & 38. (1) & 39. (3) & 40. (2) \hline 45. (2) & 46. (1) & 47. (4) & 48. (1) \hline

Q41. The reaction; $\frac { 1 } { 2 } \mathrm { H } _ { 2 ( \mathrm {~g} ) } + \mathrm { AgCl } _ { ( \mathrm { s } ) } \rightarrow \mathrm { H } _ { ( \mathrm { aq } ) } ^ { + } + \mathrm { Cl } _ { ( \mathrm { aq } ) } ^ { - } + \mathrm { Ag } _ { ( \mathrm { s } ) }$ occurs in which of the following galvanic cell :
(1) $\mathrm { Ag } \left| \mathrm { AgCl } _ { \text {(s) } } \right| \mathrm { KCl } _ { \text {(soln.) } } \left| \mathrm { AgNO } _ { 3 \text { (aq.) } } \right| \mathrm { Ag }$
(2) $\mathrm { Pt } \left| \mathrm { H } _ { 2 ( \mathrm {~g} ) } \right| \mathrm { HCl } _ { \text {(soln.) } } \left| \mathrm { AgCl } _ { ( \mathrm { s } ) } \right| \mathrm { Ag }$
(3) $\mathrm { Pt } \left| \mathrm { H } _ { 2 ( \mathrm {~g} ) } \right| \mathrm { KCl } _ { ( \text {soln. } ) } \left| \mathrm { AgCl } _ { ( s ) } \right| \mathrm { Ag }$
(4) $\mathrm { Pt } \left| \mathrm { H } _ { 2 ( \mathrm {~g} ) } \right| \mathrm { HCl } _ { ( \text {soln. } ) } \left| \mathrm { AgNO } _ { 3 ( \mathrm { aq } ) } \right| \mathrm { Ag }$

Q41. Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R). Assertion (A) : Both rhombic and monoclinic sulphur exist as $\mathrm { S } _ { 8 }$ while oxygen exists as $\mathrm { O } _ { 2 }$. Reason (R) : Oxygen forms $\mathrm { p } \pi - \mathrm { p } \pi$ multiple bonds with itself and other elements having small size and high electronegativity like $\mathbf { C } , \mathbf { N }$, which is not possible for sulphur. In the light of the above statements, choose the most appropriate answer from the options given below :
(1) (A) is correct but (R) is not correct
(2) (A) is not correct but (R) is correct
(3) Both (A) and (R) are correct and (R) is the
(4) Both (A) and (R) are correct but (R) is not the correct explanation of (A) correct explanation of (A)

Q41. Match List I with List II

	List - I (Cell)		List - II (Use/Property/Reaction)
A.	Leclanche cell	I.	Converts energy of combustion into electrical energy
B.	Ni - Cd cell	II.	Does not involve any ion in solution and is used in hearing aids
C.	Fuel cell	III.	Rechargeable
D.	Mercury cell	IV.	Reaction at anode $\mathrm { Zn } \rightarrow \mathrm { Zn } ^ { 2 + } + 2 \mathrm { e } ^ { - }$

Choose the correct answer from the options given below:
(1) A-II, B-III, C-IV, D-I
(2) A-I, B-II, C-III, D-IV
(3) A-III, B-I, C-IV, D-II
(4) A-IV, B-III, C-I, D-II

Q42. What will be the decreasing order of basic strength of the following conjugate bases? ${ } ^ { - } \mathrm { OH } , \mathrm { R } \overline { \mathrm { O } } , \mathrm { CH } _ { 3 } \mathrm { CO } \overline { \mathrm { O } } , \mathrm { C } \overline { \mathrm { I } }$
(1) $\mathrm { RO } > { } ^ { - } \mathrm { OH } > \mathrm { CH } _ { 3 } \mathrm { CO } \overline { \mathrm { O } } > \mathrm { CI }$
(2) $\mathrm { C } \overline { \mathrm { l } } > \mathrm { R } \overline { \mathrm { O } } > { } ^ { - } \mathrm { OH } > \mathrm { CH } _ { 3 } \mathrm { CO } \overline { \mathrm { O } }$
(3) ${ } ^ { - } \mathrm { OH } > \mathrm { R } \overline { \mathrm { O } } > \mathrm { CH } _ { 3 } \mathrm { CO } \overline { \mathrm { O } } > \mathrm { C } \overline { 1 }$
(4) $\mathrm { C } \overline { \mathrm { I } } > { } ^ { - } \mathrm { OH } > \mathrm { R } \overline { \mathrm { O } } > \mathrm { CH } _ { 3 } \mathrm { CO } \overline { \mathrm { O } }$

Q42. For a strong electrolyte, a plot of molar conductivity against (concentration) ${ } ^ { 1 / 2 }$ is a straight line, with a negative slope, the correct unit for the slope is
(1) $\mathrm { Scm } ^ { 2 } \mathrm {~mol} ^ { - 3 / 2 } \mathrm {~L} ^ { - 1 / 2 }$
(2) $\mathrm { Scm } ^ { 2 } \mathrm {~mol} ^ { - 3 / 2 } \mathrm {~L} ^ { 1 / 2 }$
(3) $\mathrm { Scm } ^ { 2 } \mathrm {~mol} ^ { - 3 / 2 } \mathrm {~L}$
(4) $\mathrm { Scm } ^ { 2 } \mathrm {~mol} ^ { - 1 } \mathrm {~L} ^ { 1 / 2 }$

Q42. The reaction at cathode in the cells commonly used in clocks involves.
(1) reduction of Mn from + 7 to + 2
(2) reduction of Mn from + 4 to + 3
(3) oxidation of Mn from + 3 to + 4
(4) oxidation of Mn from +2 to +7

Q42. For the electro chemical cell If $\mathrm { E } _ { \left( \mathrm { M } ^ { 2 + } / \mathrm { M } \right) } ^ { 0 } = 0.46 \mathrm {~V}$ and $\mathrm { E } _ { \left( \mathrm { x } / \mathrm { X } ^ { 2 - } \right) } ^ { 0 } = 0.34 \mathrm {~V}$. Which of the following is correct?
(1) $\mathrm { M } + \mathrm { X } \rightarrow \mathrm { M } ^ { 2 + } + \mathrm { X } ^ { 2 - }$ is a spontaneous reaction
(2) $\mathrm { E } _ { \text {cell } } = 0.80 \mathrm {~V}$
(3) $\mathrm { E } _ { \text {cell } } = - 0.80 \mathrm {~V}$
(4) $\mathrm { M } ^ { 2 + } + \mathrm { X } ^ { 2 - } \rightarrow \mathrm { M } + \mathrm { X }$ is a spontaneous reaction

Q42. A conductivity cell with two electrodes (dark side) are half filled with infinitely dilute aqueous solution of a weak electrolyte. If volume is doubled by adding more water at constant temperature, the molar conductivity of the cell will - [Figure]
(1) decrease sharply
(2) increase sharply
(3) remain same or can not be measured accurately
(4) depend upon type of electrolyte

Q42. In the given compound, the number of $2 ^ { \circ }$ carbon atom $/ \mathrm { s }$ is $\_\_\_\_$ . [Figure]
(1) Four
(2) Two
(3) One
(4) Three

Q42. For a reaction $\mathrm { A } \xrightarrow { \mathrm { K } _ { 1 } } \mathrm {~B} \xrightarrow { \mathrm {~K} _ { 2 } } \mathrm { C }$ If the rate of formation of $B$ is set to be zero then the concentration of $B$ is given by :
(1) $\left( \mathrm { K } _ { 1 } + \mathrm { K } _ { 2 } \right) [ \mathrm { A } ]$
(2) $\left( \mathrm { K } _ { 1 } / \mathrm { K } _ { 2 } \right) [ \mathrm { A } ]$
(3) $\left( \mathrm { K } _ { 1 } - \mathrm { K } _ { 2 } \right) [ \mathrm { A } ]$
(4) $\mathrm { K } _ { 1 } \mathrm {~K} _ { 2 } [ \mathrm {~A} ]$

Q42. On reaction of Lead Sulphide with dilute nitric acid which of the following is not formed?
(1) Nitric oxide
(2) Nitrous oxide
(3) Lead nitrate
(4) Sulphur

Q42. Give below are two statements: Statement I : The higher oxidation states are more stable down the group among transition elements unlike p-block elements. Statement II : Copper can not liberate hydrogen from weak acids. In the light of the above statements, choose the correct answer from the options given below :
(1) Both Statement I and Statement II are true
(2) Statement I is false but Statement II is true
(3) Both Statement I and Statement II are false
(4) Statement I is true but Statement II is false

Q43.

		List - I		List - II
\cline { 2 - 5 }	A.	$\mathrm { K } _ { 2 } \left[ \mathrm { Ni } ( \mathrm { CN } ) _ { 4 } \right]$	I.	$\mathrm { sp } ^ { 3 }$
\cline { 2 - 5 } Match List I with List II	B.	$\left[ \mathrm { Ni } ( \mathrm { CO } ) _ { 4 } \right]$	II.	$\mathrm { sp } ^ { 3 } \mathrm {~d} ^ { 2 }$
\cline { 2 - 5 }	C.	$\left[ \mathrm { Co } \left( \mathrm { NH } _ { 3 } \right) _ { 6 } \right] \mathrm { Cl } _ { 3 }$	III.	$\mathrm { dsp } ^ { 2 }$
\cline { 2 - 5 }	D.	$\mathrm { Na } _ { 3 } \left[ \mathrm { CoF } _ { 6 } \right]$	IV.	$\mathrm { d } ^ { 2 } \mathrm { sp } ^ { 3 }$
\cline { 2 - 5 }
\cline { 2 - 5 }

Choose the correct answer from the options given below:
(1) A-III, B-I, C-IV, D-II
(2) A-III, B-I, C-II, D-IV
(3) A-I, B-III, C-II, D-IV
(4) A-III, B-II, C-IV, D-I

Q43. The element which shows only one oxidation state other than its elemental form is :
(1) Cobalt
(2) Titanium
(3) Nickel
(4) Scandium

Q43. Fuel cell, using hydrogen and oxygen as fuels, A. has been used in spaceship B. has as efficiency of $40 \%$ to produce electricity C . uses aluminum as catalysts D . is eco-friendry E . is actually a type of Galvanic cell only Choose the correct answer from the options given below:
(1) A, B, D, E only
(2) A, D, E only
(3) A, B, D only
(4) A, B, C only

Q43. Molar ionic conductivities of divalent cation and anion are $57 \mathrm {~S} \mathrm {~cm} ^ { 2 } \mathrm {~mol} ^ { - 1 }$ and $73 \mathrm {~S} \mathrm {~cm} ^ { 2 } \mathrm {~mol} ^ { - 1 }$ respectively. The molar conductivity of solution of an electrolyte with the above cation and anion will be :
(1) $187 \mathrm {~S} \mathrm {~cm} ^ { 2 } \mathrm {~mol} ^ { - 1 }$
(2) $260 \mathrm {~S} \mathrm {~cm} ^ { 2 } \mathrm {~mol} ^ { - 1 }$
(3) $130 \mathrm {~S} \mathrm {~cm} ^ { 2 } \mathrm {~mol} ^ { - 1 }$
(4) $65 \mathrm {~S} \mathrm {~cm} ^ { 2 } \mathrm {~mol} ^ { - 1 }$

Q43. The number of ions from the following that have the ability to liberate hydrogen from a dilute acid is $\_\_\_\_$。 $\mathrm { Ti } ^ { 2 + } , \mathrm { Cr } ^ { 2 + }$ and $\mathrm { V } ^ { 2 + }$
(1) 2
(2) 3
(3) 1
(4) 0

Q43. The number of element from the following that do not belong to lanthanoids is $\mathrm { Eu } , \mathrm { Cm } , \mathrm { Er } , \mathrm { Tb } , \mathrm { Yb }$ and Lu
(1) 3
(2) 4
(3) 1
(4) 5

Q43. Iron (III) catalyses the reaction between iodide and persulphate ions, in which A . $\mathrm { Fe } ^ { 3 + }$ oxidises the iodide ion B. $\mathrm { Fe } ^ { 3 + }$ oxidises the persulphate ion $\mathrm { C } . \mathrm { Fe } ^ { 2 + }$ reduces the iodide ion $\mathrm { D } . \mathrm { Fe } ^ { 2 + }$ reduces the persulphate ion Choose the most appropriate answer from the options given below:
(1) B only
(2) A only
(3) B and C only
(4) A and D only

Q43. Identify the incorrect statements about group 15 elements : (A) Dinitrogen is a diatomic gas which acts like an inert gas at room temperature. (B) The common oxidation states of these elements are $- 3 , + 3$ and + 5 . (C) Nitrogen has unique ability to form $\mathrm { p } \pi - \mathrm { p } \pi$ multiple bonds. (D) The stability of + 5 oxidation states increases down the group. (E) Nitrogen shows a maximum covalency of 6 . Choose the correct answer from the options given below :
(1) (A), (C), (E) only
(2) (B), (D), (E) only
(3) (D) and (E) only
(4) (A), (B), (D) only

Q43. $0.05 \mathrm { MCuSO } _ { 4 }$ when treated with $0.01 \mathrm { MK } _ { 2 } \mathrm { Cr } _ { 2 } \mathrm { O } _ { 7 }$ gives green colour solution of $\mathrm { Cu } _ { 2 } \mathrm { Cr } _ { 2 } \mathrm { O } _ { 7 }$. The two [Figure] [0pt] solutions are separated as shown below : [SPM : Semi Permeable Membrane] Due to osmosis :
(1) Molarity of $\mathrm { CuSO } _ { 4 }$ solution is lowered.
(2) Molarity of $\mathrm { K } _ { 2 } \mathrm { Cr } _ { 2 } \mathrm { O } _ { 7 }$ solution is lowered.
(3) Green colour formation observed on side Y.
(4) Green colour formation observed on side X .