Chemistry Practice MCQs

1. When \(V_2O_5\) reacts with base and acid, X and Y are formed respectively. X and Y are:

1. \(X = VO^{3-}_4 ,~~~Y = VO^{+} _2\)
2. \(X = VO^{3-}_4 ,~~~Y = VO^{+}_4 \)
3. \(X = VO^{+}_4 ,~~~Y = VO^{3-}_4 \)
4. \(X = VO^{2+} ,~~~Y = V_2O_{3} \)

2. The pair in the actinide series that can have the highest oxidation state is:
1. Np, Pu
2. U, Am
3. U, Cm
4. Am, Cm

3. The correct IUPAC nomenclature of \(\mathrm{[NiCl_2(PPh_3)_2] }\) is:

1.	Bischloridobis(triphenylphosphine)nickel(II)
2.	Dichloridobis(triphenylphosphine)nickel(II)
3.	Dichloridodi(triphenylphosphine)nickel(II)
4.	Bischloridodi(triphenylphosphine)nickel(II)

4. For the dissolution of a solid in a liquid, choose the incorrect statement:

1.	If the dissolution is endothermic, the solubility should increase with rise in temperature.
2.	If the dissolution is exothermic, the solubility should decrease with rise in temperature.
3.	Pressure affects the solubility of solids in liquids such that on increasing pressure, the solubility of solids in liquids increases.
4.	Solute dissolves in a solvent if the intermolecular interactions are similar in the two.

5. Choose the incorrect statement from the following:

1.	Standard boiling point of a liquid is slightly lower than the normal boiling point.
2.	Boiling does not occur when liquid is heated in a closed vessel.
3.	The SI unit of coefficient of viscosity is kg m^-1s^-1.
4.	When the attractive forces between molecules of a liquid is large, the surface tension is low.

6. Match List I with List II

List I	List II
Graph	Law
I.	A. Boyle's law
II.	B. Avogadro's law
III.	C. Charle's law
IV.	D. Gay-Lussac's law

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

7. 3 moles of helium gas at 1 bar is compressed reversibly and isothermally at 400 K to 10 bar pressure. The work done (in J) on the system is: (Given: \(R= 8.314 ~J K^{-1}~ mol^{-1}\) )

1.	\(2.29 \times 10^4 \)	2.	\(2.29 \times 10^{-4} \)
3.	\(-2.29 \times 10^4 \)	4.	\(-2.29 \times 10^{-4} \)

8. Which of the following is an incorrect statement?

1.	Molar heat capacity is an intensive property.
2.	\(\Delta S > 0 \) for an isolated system \((\Delta U = 0 )\)
3.	A bomb calorimeter is used to measure the heat absorbed at a constant volume.
4.	Pressure, volume and work done on the system are state functions.

9. Correct statement for the given reaction is:
\(\mathrm{Cr}_2 \mathrm{O}_7{ }^{2-}(a q)+\mathrm{SO}_3{ }^{2-}(a q) \rightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{SO}_4{ }^{2-}(a q)\)
1. Generally \(SO_4^{2-}\) is not a reducing agent.
2. \(Cr^{3+} \) can be further reduced in this reaction.
3. Oxidation by \(SO_3^{2-} \) gives \(Cr^{3+} \)
4. In \(Cr_2O^{2-}_7 \) oxidation state of Cr is not +6.

10. The method that is not used for the coagulation of lyophobic sols is:
1. Bredig's Arc method
2. Electrophoresis
3. Addition of flocculating ion
4. Persistent dialysis

11. For a first-order reaction, the relationship between the time required for 99% completion of the reaction \((t_{0.99}) \) and the time required for completion of 90% of the reaction \((t_{0.90}) \) is:
1. \(t_{0.90} = 10 t_{0.99}\)
2. \(t_{0.90} = 2 t_{0.99} \)
3. \(t_{0.99} = 10 t_{0.90} \)
4. \(t_{0.99} = 2 t_{0.90} \)

12. The solubility of \(Sr(OH)_2 \) at 298 K is 20 g/L of solution. The pH of this solution will be:

(Given: molar mass of Sr = 88 g/mol; log 40 =1.60 ; and log 122 = 2.086)
1. 13.51
2. 0.48
3. 10.22
4. 11.25

13. What is the resulting pH when 50 mL of a 0.1 M solution of \(\mathrm{CH_3COOH }\) is mixed with 25 mL of 0.1 M NaOH?
(Given: \(\text K_a\) of \(\mathrm{CH_3COOH = 1.77 \times 10^{-5} ; }\)
\(\text {log}~ 1.77 = 0.248\))
1. 9.25
2. 4.75
3. 4.01
4. 9.18

14. Incorrect statement about a mercury cell is:

1.	Zinc- Hg amalgam acts as anode.
2.	Paste of HgO and C acts as cathode.
3.	Paste of KOH and ZnO is used as electrolyte.
4.	Cell potential is 2.50 V and it keeps on decreasing with the life of the cell.

15. Litmus solution, when shaken with charcoal, becomes colorless. Incorrect statement about adsorption from the solution phase is:

1.	Extent of adsorption depends on the concentration of the solute in the solution.
2.	Extent of adsorption increases with the increase of the surface area of the adsorbent.
3.	Extent of adsorption decreases with the decrease in temperature.
4.	Extent of adsorption depends on the nature of the adsorbent and the adsorbate.

16. Select the correct option for the structure of iproniazid:
1.

2.

3.

4.

17. The correct cyclic structure of β-D-fructofuranose is:

1.		2.
3.		4.

18. For the following ions, choose the correct statement:

1. III is the most stable in aqueous phase
2. I is the most stable in the aqueous phase
3. III is the smallest in size
4. II is the most stable in the aqueous phase

19. In the following reaction, "A" is:

1. Cu
2. Pd
3. Cu (I)
4. Sn

20. For the given organic reaction, 'A' is:

1.		2.
3.		4.

21. In the given organic reaction, A is:

1. NaOH
2. NaOCI
3. NaCI
4. CI₂

22. The product 'A' in the given organic reaction is:

1.		2.
3.		4.

23.

Among the following, the most reactive compound towards S_N1 reactions is:

1.
2.
3.
4.

24. Select the correct option for the following structure of picric acid:

1.		2.
3.		4.

25. Which of the following compounds is aromatic?

1.		2.
3.		4.

26. In the Carius method, which of the following elements is not analyzed quantitatively?
1. Nitrogen
2. Sulphur
3. Halogen
4. Phosphorus

27. What is the nature of Lassaigne's extract?
1. Neutral
2. Mild acidic
3. Strong acidic
4. Basic

28. The incorrect statement among the following is:

1.	Temperature at which a real gas obeys ideal gas laws over an appreciable range of pressure is called Boyle temperature.
2.	Compressibility factor is defined as the ratio of the molar volume of the gas had it been ideal to the actual molar volume of the gas.
3.	Critical temperature of a gas is the temperature above which it cannot be liquefied no matter how high the pressure is.
4.	Critical pressure is the minimum pressure required to liquefy a gas at its critical temperature.

29. On the basis of the Maxwell-Boltzmann distribution of molecular speed, identify the incorrect statement in the following:

1.	At the same temperature, N₂molecules move faster than the Cl₂molecules.
2.	The maximum in the Maxwell-Boltzmann curve represents the most probable speed.
3.	The average speed of CO₂molecules is more than CH₄ molecules.
4.	At a particular temperature, the individual speed of the molecules keeps changing but the distribution of speed remains the same.

30. Match the following reactions in Column-I to the correct enthalpy associated with them given in Column-II:

	Column-I		Column-II
A.	\(\small{C_6H_6(l)+\frac{15}{2}O_2\rightarrow6CO_2(g)+3H_2O(l)}\)	I.	\(\Delta_{\text{lattice}}H^\circ\)
B.	\(NaCl(s)\rightarrow Na^+(g)+Cl^-(g) \)	II.	\(\Delta_{\text{hyd}}H^\circ\)
C.	\(AB(s)\rightarrow A^+(aq)+B^-(aq) \)	III.	\(\Delta_\text cH^\circ \)
D.	\(\small{A^+(g)+B^-(g)\rightarrow A^+(aq)+B^-(aq)}\)	IV.	\(\Delta_{\text{sol}}H^\circ \)

Choose the correct option from the following:
1. A - (III); B - (I); C - (IV); D - (II)
2. A - (III); B - (I); C - (II); D - (IV)
3. A - (II); B - (I); C - (IV); D - (III)
4. A - (III); B - (II); C - (I); D - (IV)

31. Choose the incorrect statement from the following :

1.	In a reversible process, the system and surroundings are always in equilibrium with each other.
2.	Work done in free expansion > 0.
3.	For adiabatic change, \(\Delta q \) = 0 .
4.	For a process carried at constant pressure,\(\Delta H = q_p \)

32. For the reaction,
\(N_2(g)+3H_2(g)\rightleftharpoons2NH_3(g)+22.2~\text{kcal} \)
What will be the effect of increasing temperature and pressure on the equilibrium?

A.	.Higher temperature shifts equilibrium in the reverse direction.
B.	Lower pressure shifts equilibrium backward.
C.	Higher temperature shifts equilibrium forward.
D.	Higher pressure shifts equilibrium backward.

Choose the correct pair of statements from the above:
1. C, D
2. A, B
3. A, D
4. B, C

33. The standard Gibbs free energy for the following reaction is:
\(Fe^{2+} (aq)+Ag^+(aq) \rightarrow Fe^{3+}(aq)+Ag(s)\)
Given: \(\small(E^o_{Ag^+/Ag} = 0.80 V; E^o_{Fe^{3+}/Fe^{2+}} = 0.77 V; E^o_{Fe^{2+}/Fe} = 0.44 V )\ \).

1.	- 2.895 kJ/mol	2.	- 2.895 J/mol
3.	- 239.287 kJ/mol	4.	239.287 kJ/mol

34. The molar conductance of a solution, given its conductivity (0.248 S m^-1) and concentration (0.2 mol m^-3) is:
1. 0.124 S cm² mol^-1
2. 1.24 S m²mol^-1
3. 124 S cm² mol^-1
4. 124 S m² mol^-1

35. For a reaction, A + B \({\rightarrow}\) products, the rate is double when the concentration of B is halved (keeping [A] constant), while the rate is halved when the concentration of A is halved (keeping [B] constant). The overall order of the reaction is:

1.	1	2.	0.5
3.	0	4.	2

36. Consider the following graphs:

a.		b.
c.		d.

Among the above, the incorrect graph of a first-order reaction of R → P is:
1. a
2. b
3. c
4. d

37. The process of removing ions (or molecules) from a sol by diffusion through a permeable membrane is called:

1. Ultrafiltration
2. Dialysis
3. Electrophoresis
4. Osmosis

38. When NaCl solution is added to a solution of AgNO₃, the AgCl sol produced is:

1.	Negatively charged due to the adsorption of NO₃^-ions.
2.	Negatively charged due to the adsorption of Cl^-ions.
3.	Positively charged due to the adsorption of H⁺ions.
4.	Positively charged due to the adsorption of Ag⁺ions.

39. In face-centered cubic (fcc) structure, each sphere is in contact with ________ spheres.
1. 6
2. 8
3. 12
4. 4

40. A 50-watt bulb emits monochromatic yellow light of a wavelength of 0.60 μm. The number of photons emitted per second by the bulb is:
1. 2.3 × 10²⁰
2. 1.1 × 10¹⁹
3. 1.8 × 10¹⁹
4. 1.5 × 10²⁰

41. At atmospheric pressure ice crystallizes in the X form, however, it condenses to Y form at a lower temperature. X and Y are:
1. X = cubic, Y = hexagonal
2. X = cubic, Y = cubic
3. X = hexagonal, Y = hexagonal
4. X = hexagonal, Y = cubic

42. Water gas and producer gas are respectively:
1. CO + H₂ and CO + N₂
2. CO₂ + H₂ and CO + N₂
3. CO + H₂ and CO₂+ N₂
4. CO₂ + H₂ and CO₂ + N₂

43. At elevated temperatures (~1000 K), sulphur exists as:
1. S₈
2. S
3. S₂
4. S₆

44. Which one of the following halides exhibits the least covalent character?

1.	\( \text{SbCl}_5\)	2.	\(\text{SnCl}_2 \)
3.	\( \text{SnCl}_4\)	4.	\( \text{PbCl}_4\)

45. The following fluoride is not known:
1. CrF₆
2 MnF₆
3. MnF₄
4. CrF₅

46. Which of the following is NOT a property of interstitial compounds?

1.	Retains metallic conductivity.
2.	Very hard.
3.	High melting point, lower than those of pure metals.
4.	Chemically inert.

47. The correct electronic configuration of Ytterbium (Yb ,atomic no- 70) is:
1. [Xe]4\(\)f¹²5d²6s²
2. [Xe]4f¹⁴5d²6s⁰
3. [Xe]4f¹⁴5d¹6s¹
4. [Xe]4f¹⁴5d⁰6s²

48. The correct increasing order of ligands based on their effect on the splitting of d orbitals is:
1. edta^4-< NH₃ <CN^-< en
2. en < edta^4-< NH₃<CN^-
3. edta^4-< NH₃< en <CN^-
4. en < NH₃ < edta^4- < CN^-

49. The splitting of the d-orbital in a tetrahedral crystal field is:

1.	(2/5)\(\Delta_t\) above barycentre and (3/5/)\(\Delta_t\) below barycentre.
2.	(2/5)\(\Delta_0\) above barycentre and (3/5/)\(\Delta_0\) below barycentre.
3.	(2/5)\(\Delta_t\) below barycentre and (3/5)\(\Delta_t\) above barycentre.
4.	(2/5)\(\Delta_0\) below barycentre and (3/5/)\(\Delta_0\) above barycentre.

50. Select the correct option for the increasing order of ease of S_N1 reaction by the following compounds, on treatment with aq. KOH:

A.
B.
C.
D.

Choose the correct answer from the options given below:

1.	C < D < A < B	2.	B < C < A < D
3.	C < B < D < A	4.	D < C < B < A

51. Identify the reaction that produces the correct major products under the given condition.

1.
2.
3.
4.

52. Given the following compounds A to E:

A.		B.
C.		D.
E.

Select the correct option for the increasing order of acidic strength for the compounds given above:
1. C < B < A < D < E
2. A < C < B < E < D
3. C < A < B < D < E
4. B < A < C < E < D

53. Among the following types of detergents, non-biodegradable detergents are:
1. Anionic and linear
2. Cationic and linear
3. Non-ionic and linear
4. Non-ionic and branched

54. Which among the following is an aromatic compound?

1.		2.
3.		4.

55. An element 'X' having density of 9.0 gcm^-3has a face-centered cubic structure with a cell edge of 300 pm. The number of unit cells present in 270 g of the element are:
1. 4.44 × 10²⁴
2. 1.11 × 10²⁴
3. 2.22 × 10²⁴
4. 2.7 × 10²³

56.

The osmotic pressure of the solution formed by mixing 25 ml of 0.1 M MgCl₂ and 25 ml of 0.1 M Urea at 300 K will be:
(R=0.0821 lit atm K^-1mol^-1)

1.	2.463 atm	2.	1.231 atm
3.	4.926 atm	4.	369 atm

57.

For metal \('M',~E^o_3 \) for \(M^{+7}/M \) will be:
1. 0.59 V
2. 2.07 V
3. 0.44 V
4. -0.59 V

58. The magnetic moment for a divalent ion in an aqueous solution having atomic number 25 is:
1. 4.89 BM
2. 5.92 BM
3. 3.87 BM
4. 2.84 BM

59. Identify the transition metal ions from the given list that exhibit no color in their aqueous solution:
Sc³⁺; Ti³⁺; Ti⁴⁺; Ni²⁺; Zn²⁺; Mn²⁺
Choose the correct answer from the options given below:
1. Sc³⁺; Ti³⁺; Zn²⁺
2. Sc³⁺; Ti⁴⁺; Zn²⁺
3. Ni²⁺; Zn²⁺; Mn²⁺
4. Ti⁴⁺; Ni²⁺; Zn²⁺

60.

A.	\((C_6H_5)_3\dot{C} \)
B.	\((CH_3)_2\dot{C}H \)
C.	\((C_6H_5)_2\dot{C}~CH_3 \)
D.	\(C_6H_5\dot{C}(CH_3)_2 \)

For the free radical given above, correct option for decreasing order of stability is:
1. A > C > D > B
2. A > B > C > D
3. B > A > C > D
4. B > D > A > C

61. Among the following, a disaccharide is:
1. Fructose
2. Maltose
3. Cellulose
4. Amylopectin

62. Which of the following diseases is caused by a deficiency of Vitamin \(\mathrm{B_2}\)?

1.	Beri-Beri	2.	Cheilosis
3.	Pernicious anaemia	4.	Convulsions

63. In the following reaction \(Z\xrightarrow[\text{Reagent}]{\text{Tollen's}}RCH_2CH_2COO^\ominus, \) Identify \('Z'\):

1.
2.
3.
4.

64. Which of the following carboxylic acids is the most acidic?
1. Butanoic acid
2. 2-Chlorobutanoic acid
3. 3-Chlorobutanoic acid
4. 4-Chlorobutanoic acid

65. Among the following, the amine that is most basic is:

1.
2.
3.
4.

66. Shape-selective catalysis depends upon the:
1. Pore structure of the catalyst only.
2. Size of the reactant only.
3. Size of the product only.
4. Size of both reactant and product and pore structure of the catalyst.

67. The correct statement regarding lithium is:

1.	It forms Li₂O when burnt in O₂
2.	It has lower melting and boiling point than other alkali metals.
3.	It's compound shows ionic character.
4.	Lithium is much softer than other alkali metals.

68. In the Castner-Kellner process, the solution of 'A' is electrolyzed using a cathode of metal 'B' and anode of element 'X'. Identify 'A', 'B', and 'X' respectively:
1. NaCl, Mercury, Carbon
2. NaOH, Zinc, Carbon
3. NaCl, Zinc, Carbon
4. NaOH, Mercury, Zinc

69. At 300K, \(\Delta rG \) and \(\Delta rG^\circ \) are - 12.8 KJ mol^-1 and -11.5 KJ mol^-1 respectively for the following reaction:
\(A(g) + B(g) \rightleftharpoons C(l) + D(aq)\)
If the reaction is at equilibrium, then the equilibrium constant K will be:
1.\(-2.0 \times 10^0\)
2. \(1.0 \times 10^2\)
3. \(1.0 \times 10^{-2}\)
4. \(1.69 \times 10^0\)

70. The enthalpy of combustion of four allotropic forms of element 'X' are given as:

Allotropic forms	\(\Delta_\text{comb}H^\circ\)(kJ/mol)
A.	-270.3
B.	-189.1
C.	-390.5
D.	-465.0

The most stable allotropic form of element 'X' is:
1. A
2. B
3. C
4. D

71. The pH of 10^-6 M H₂SO₄ will be:
1. 5.69
2. 5.60
3. 6.0
4. 6.32

72. What is the solubility of BaSO₄in 10^-3 M H₂SO₄ solution ?
(Given: K_sp for BaSO₄= 1.1 × 10^-10)

1.	1.1 × 10^–13M	2.	1.1 × 10^–7 M
3.	5.5 × 10^–7 M	4.	5.5 × 10^–8 M

73. Arrange the following molecules in the correct decreasing order of boiling points
H₂ ; D₂ ; H₂O ; H₂O₂ ; D₂O
Choose the correct answer from the options given below:

1.	H₂O₂> D₂O > H₂O > D₂> H₂
2.	D₂O > H₂O₂> H₂O > D₂> H₂
3.	H₂O₂ > H₂O > D₂O > H₂ > D₂
4.	H₂O > H₂O₂> D₂O > H₂ > D₂

74. Which of the following molecules does not contain a coordinate bond?

1.	N₂O	2.	KNC
3.	CO	4.	HNO₂

75. ICl₃ dimerizes in order to:
1. Reduce the number of lone pairs of electrons
2. Increase the number of bonds
3. Form coordinate bonds
4. Reduce lone pair-lone pair repulsion

76. The molecule having \(p\pi -d\pi \) bond is:
1. H₂CO₃
2. HNO₃
3. H₃PO₄
4. HOCl

77. Incorrect statement about ozone is:

1.	Pure ozone is a pale blue gas, dark blue liquid, and violet-black solid.
2.	Ozone acts as a powerful oxidising agent.
3.	The two oxygen-oxygen bond lengths in the ozone molecule are identical.
4.	Ozone is not an allotropic form of oxygen.

78. The IUPAC name of coordination compound having formula [Cr(NH₃)₃(H₂O)₃]Cl₃ is:
1. Triamminetriaquachromium (III) chloride
2. Triamminetriaquachromium (III) trichloride
3. Triaquatriamminechromium (III) chloride
4. Triamminetriaquachromium (II) chloride

79. Match List I with List II:

List I	List II
Coordinate compound	Magnetic moment
A. [NiCl₄]^2-	I. 0 BM
B. [Co(NH₃)₆]³⁺	II. 3.87 BM
C. [Fe(CN)₆]^3-	III. 2.82 BM
D. [Cr(NH₃)₆]³⁺	IV. 1.732 BM

(Atomic Number of Cr =24, Fe=26, Co=27 , Ni=28)
Choose the correct answer from the options given below:

	(A)	(B)	(C)	(D)
1.	III	I	II	IV
2.	I	II	III	IV
3.	III	I	IV	II
4.	I	III	IV	II

80. Out of CCl₄, SiCl₄, SnCl₄, and PbCl_4, the compound that will not be easily hydrolyzed by water is:
1. CCl₄
2. SiCl₄
3. SnCl₄
4. PbCl₄

81. The shape of BCl₃. NH₃is/are :
1. Planar only.
2. Square planer only.
3. Tetrahedral only.
4. Both planar and tetrahedral.

82. The oxidation numbers of three carbons in C₃O₂are:
[Given: Structure of C₃O₂ is

]
1. \(\frac43;\frac43;\frac43 \)
2. \(+2; 0; +2 \)
3. \(+2; +2; 0 \)
4. \(0; +2; +2 \)

83. Select the correct option for the relationship between root mean square speed (U_r_ms), average speed (U_av), and the most probable speed (U_mp) :
1. U_r_ms > U_mp > U_av
2. U_r_ms> U_av> U_mp
3. U_av> U_mp> U_r_ms
4. U_mp > U_r_ms > U_av

84. A golf ball has a mass of 46 g and a speed of 45 m/s. If the speed can be measured within the accuracy of 3%, the uncertainty in the position is:
1. 8.4×10^-34m
2. 6.4×10^-33m
3. 6.6×10^-39m
4. 2.1×10^-34m

85. If density of a 3 M solution of NaCl is 1.25 gm mL^-1, then its molality will be:
1. 2.79 m
2. 3.50 m
3. 4.1 m
4. 0.2 m

86. Classical smog is a mixture of:
1. Fog and SO₃
2. Fog and SO₂
3. Fog, smoke and SO₂
4.. Fog, smoke and SO₃

87. Among the following, the gas that is not a green house gas is:
1. CO₂
2. CH₄
3. O₃
4. CO

88. Ortho-sulphobenzimide is also known as:

1. Saccharin
2. Sucralose
3. Aspartame
4. Alitame

89. A catalyst used in the given reaction is:

1. Pd(II)
2. Cu(I)
3. Pb(I)
4. Cu (II)

90. The order of reactivity of alkyl halides (RCl, RBr, RI) with aliphatic amines is:
1. \(RCl > RI > RBr \)
2. \( RBr > RCl > RI \)
3. \(RI > RBr > RCl \)
4. \(RI > RCl > RBr \)

91. The major product (Z) for the following organic reaction is:

1.		2.
3.		4.

92. The major product 'A' for the given organic reaction will be:

1.		2.
3.		4.

93. What is the major product 'A' formed in the following organic reaction?

1.		2.
3.		4.

94. Consider the following compounds:

The correct increasing order of the acid strength of the compounds will be:
1. I < II < III < IV
2. IV < II < I <III
3. I < IV < II < III
4. IV < I < II < III

95. Consider the following compounds:

I.
II.

The correct statement regarding these compounds is:
1. I and II are chiral
2. I and II are achiral
3. I is chiral and II is achiral
4. I is achiral and II is chiral

96. For the given organic reaction
\(CH_4 + H_2O \xrightarrow {A/ 1273~ K} CO + 3 H_2 \)
A is:
1. PdO
2. Cu
3. Ni
4. Pb

97. The number of sigma \((\sigma) \) and pi (\(\pi\)) bonds present in the given compound will be:

1. \(26 \sigma, 3 \pi\)
2. \(24 \sigma, 4 \pi\)
3. \(24 \sigma, 3 \pi\)
4. \(26 \sigma, 4 \pi\)

98. A mixture of phenol and aniline is an example of:

1.	Ideal solution.
2.	Non-ideal solution exhibiting positive deviation from Raoult's law.
3.	Non-ideal solution exhibiting negative deviation from Raoult's law.
4.	Minimum boiling azeotrope.

99. The amount of \(\text{CaCl}_2~ (i = 2.47) \) that must be dissolved in 3 litre of water such that its osmotic pressure is 4.94 atm at 27 °C is:
1. \(2.405 \times 10^{-3} ~ \text {mol} \)
2. \(0.243 ~ \text {mol} \)
3. \(0.0267 ~ \text {mol} \)
4. \(1.486 ~ \text {mol} \)

100. Real gases show nearly ideal behaviour at:
1. Low pressure and low temperature.
2. High pressure and low temperature.
3. High pressure and high temperature.
4. Low pressure and high temperature.

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