1. The molarity of a solution obtained by mixing 750 mL of 0.5 M HCl with 250mL of 2M HCl will be
a) 0.875 M
b) 1.00 M
c) 1.75 M
d) 0.0975 M

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2. The mass of potassium dichromate crystals required to oxidise 750 cm² of 0.6 M Mohr's salt solution is (molar mass = 392)
a) 0.49 g
b) 0.45 g
c) 22.05 g
d) 2.2 g

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1. The edge length of a face centered cubic cell of an ionic substance is 508 pm. If the radius of cation is 110 pm, the radius of the anion is
a) 288 pm
b) 398 pm
c) 618 pm
d) 144 pm

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2. In van der Waals equation of state of the gas law, the constant b is a measure of
a) intermolecular replusion
b) intermolecular attraction
c) volume occupied by the molecules
d) intermolecular collisions per unit volume

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1. The electrons identified by quantum numbers n and l
(1) n=4, l=1
(2) n=4 , l=0,br> (3) n=3 , l = 2
(4) n = 3, l = 1
can be placed in the order of increasing energy as
a) (3)<(4)<(2)<(1)
b) (4)<(2)<(3)<(1)
c) (2)<(4)<(1)<(3)
d) (1)<(3)<(2)<(4)

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2. Uncertainty in position of a particle  of 25 g in space is 10^-5. Hence, uncertainty in velocity (ms^-1) is Plancks constant, h = 6.6 × 10^-34 Js)
a) 2.1 × 10^-28
b) 2.1 × 10^-34
c) 0.5 × 10^-34
d) 5.0 × 10^-24

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1. The bond order in NO is 2.5 while that in NO⁺ is 3. Which of the following statements is true for these two species?
a) Bond length in NO⁺ is greater than in NO
b) Bond length in NO is greater than in NO⁺
c) Bond length in NO⁺ is equal to that in NO
d) Bond length is unpredictable

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2. Which of the following molecules/ions does not contain unpaired electrons?
a) $O_{2}^{2-}$
b) B₂
c) $N_{2}^{+}$
d) O₂

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1. The standard enthalpy of formation $\left (\Delta H_{f}^{0} \right )$ at 298 K for methane, CH₄(g) is -74.8 kJ mol^-1. The addition information required to determine the average energy for C-H bond formation would be
a) the dissociation energy of H₂ and enthalpy of sublimation of carbon
b) latent heat of vaporisation methane
c) the first four ionisation energies of carbon and electron gain enthalpy of hydrogen
d) the dissociation energy of hydrogen molecule, H₂

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2. In view of the signs of Δ_rG⁰ for the following reactions
PbO₂ + Pb → 2PbO , Δ_rG⁰ < 0
SnO₂ + Sn → 2SnO , Δ_rG⁰ > 0
Which oxidation states are more characteristic for lead and tin?
a) For lead + 4, for tin +2
b) For lead +2, for tin +4
c) For lead +4, for tin +4
d) For lead +2, for tin +4

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1. Which one of the following aqueous solutions will exhibit highest boiling point?
a) 0.01 M Na₂SO₄
b) 0.01 M KNO₃
c) 0.015 M urea
d) 0.015 M glucose

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2. The molaltiy of a urea solution in which 0.0100 g of urea, [(NH₂)₂CO] is added to 0.3000 dm³ of water at STP is
a) 0.555 m
b) 5.55 x 10^-4 m
c) 33.3 m
d) 3.33 x 10^-2 m

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1. At 25⁰C, the solubility product of Mg(OH)₂ is 1.0 x 10^-11 . At which pH, will Mg²⁺ ions start precipitating in the form of Mg(OH)₂ from a solution of 0.001 M Mg²⁺ ions?
a) 9
b) 10
c) 11
d) 8

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2. For the reaction equilibrium ,
N₂O₄ (g) $\rightleftharpoons$ 2NO₂ (g)
the concentrations of N₂O₄ and NO₂ at equilibrium are 4.8 x 10^-2 and 1.2 x 10^-2 mol L^-1, respectively. the value of K_c for the reaction is
a) 3.3 x 10² mol L^-1
b) 3 x 10^-1 mol L^-1
c) 3 x 10^-3 mol L^-1
d) 3 x 10³ mol L^-1

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1. Consider the following E⁰ values:
$E_{Fe^{3+}/Fe^{2+}}$ = + 0.77 V
$E_{Sn^{2+}/Sn}$ = -0.14 V
Under standard conditions, the potential for the reaction
Sn(s) + 2Fe³⁺(aq) → 2Fe²⁺(aq) + Sn²⁺(aq) is
a) 1.68 V
b) 1.40 V
c) 0.91 V
d) 0.63 V

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2. The equivalent conductances of two strong electrolytes at infinite dilution in H₂O (where ions move freely through a solution) at 25⁰ C are given below
$\Lambda{^{0}}_{CH_{3}COONa}$ = 91.0 S cm² /equiv
$\Lambda{^{0}}_{HCl}$ = 426.2 S cm²/equiv
What additional information\quantity one needs to calculate &Lmabda;⁰ of an aqueous solution of acetic acid?
a) Λ⁰ of NaCl
b) Λ⁰ of CH₃COOK
c) The limiting equivalent conductance of H⁺ (λ⁰_H⁺)
d) Λ⁰ of chloroacetic acid (ClCH₂COOH)

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1. Rate constant , k of the first order reaction when initial concentration (C₀) and concentration (C_t) at time t, is given by equation kt = log C₀ - log C_t
Graph is a straight line if we plot
a) t vs log C₀
b) t vs log C_r
c) t^-1 vs log C_r
d) log C₀ vs log C_r

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2. The rate of a reaction double when its temperature changes from 300K to 310 K. Activation energy of such a reaction will be (R = 8.314 JK^-1 mol^-1 and log 2 = 0.301)
a) 53.6 kJ mol^-1
b) 58.6 kJ mol^-1
c) 58.5 kJ mol^-1
d) 60.5kJ mol^-1

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1. Which one of the following ions has the highest value of ionic radius?
a) Li⁺
b) B³⁺
c) O^2-
d) F^-

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2. The increasing order of the ionic radii of the given isoelectronic species is
a) Cal^-, Ca²⁺ , K⁺ , S²
b) S^2-, Cl^-,Ca²⁺, K⁺
c) Ca²⁺ , K⁺, Cl^-, S^2-
d) K⁺,S^2-, Ca²⁺,Cl^-

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1. Which method of purification is represented by the following equation?
$Ti(s) + 2I_{2}(g) \overset{523 K}{\rightarrow} Til_{4}(g)\overset{1700K}{\rightarrow} Ti(g) + 2I_{2}(g)$
a) Zone refining
b) Cupellation
c) Polling
d) van-Arkel

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2. Which series of reactions correctly represent chemical relations related to iron and its compound?
a) $Fe \overset{Dil.H_{2}SO_{4}}{\rightarrow} FeSO_{4} \overset{H_{2}SO_{4}.O_{2}}{\rightarrow} Fe_{2}\left (SO_{4} \right )_{3} \overset{Heat}{\rightarrow}Fe$
b) $Fe\overset{O_{2},heat}{\rightarrow}FeO \overset{dil.H_{2}SO_{4}}{\rightarrow}FeSO_{4}\overset{Heat}{\rightarrow}Fe$
c) $Fe\overset{Cl_{2}.heat}{\rightarrow}FeCl_{3} \overset{Heat,air }{\rightarrow}FeCl_{2}\overset{Zn}{\rightarrow}Fe$
d) $Fe\overset{O_{2}.heat}{\rightarrow}Fe_{3}O_{4}\overset{CO,600^{0}C}{\rightarrow}FeO\overset{CO,700^{0}C}{\rightarrow}Fe$

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1. What is the best description of the change that occurs when Na₂O(s) is dissolved in water?
a) Oxidation number of sodium decreases
b) Oxide ion accepts a shared pair of electrons
c) Oxide ion donates a pair of electrons
d) Oxidation number of oxygen increases

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2. In which of the following arrangements, the sequence is not strictly according to the property written against it?
a) Co₂ < SiO₂ < SnO₂ < PbO₂
increasing oxidising power
b) HF < HCl < HBr < HI
increasing acid strength
c) NH₃ < PH₃ < AsH₃ < SbH₃
increasing basic strength
d) B < C < O < N
increasing first ionisation enthalpy

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1. The magnetic moment (spin only) of [NiCl₄]^2- is
a) 1.82 BM
b) 5.46 BM
c) 2.82 BM
d) 1.41 BM

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2. The equation which is balanced and represents the correct product(s) is
a) Li₂O + 2KCl → 2LiCl + K₂O
b) [CoCl(NH₃)₅]⁺ + 5H⁺ → CO²⁺ + $5NH_{4}^{+}$ + Cl^-
c) $[Mg(H_{2}O)_{6}]^{2+} + (EDTA)^{4-} \overset{excess NaOH}{\rightarrow} [Mg (EDTA)]^{2+} + 6H_{2}O$
d) CuSO₄ + 4KCN → K₂ [Cu(CN)₄] + K₂SO₄

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1. The smog is essentially caused by the presence of
a) O₂ and O₃
b) O₂ and N₂
c) oxides of sulphur and nitrogen
d) O₃ and N₂

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2. Identify the wrong statements in the following
a) Chlorofluorocarbons are responsible for ozone layer depletion
b) Green house effect is responsible for global warming
c) Ozone layer does not permit infrared radiation from the sun to reach the earth
d) Acid rain is mostly because of oxides of nitrogen and sulphur

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1. Which type of isomerism is shown by 2,3-dichlorobutane?
a) Structural
b) Geometeric
c) Optical
d) Diastereo

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2. The correct order of increasing basicity of the given conjugate bases (R=CH₃) is
a) $RCO\bar{O} < HC = \bar{C} < \bar{R} < \bar{N}H_{2}$
b) $\bar{R} < HC \equiv \bar{C} < RCO\bar{O} < \bar{N}H_{2}$
c) $RCO\bar{O} < \bar{N}H_{2} < HC \equiv \bar{C} < \bar{R}$
d) $RCO\bar{O} < HC \equiv \bar{C} < \bar{N}H_{2} < \bar{R}$

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1. On mixing ethyl acetate with aqueous sodium chloride, the composition of the resultant solution is
a) $CH_{3}COOC_{2}H_{5} + NaCl$
b) $CH_{3}COONa + C_{2}H_{5}OH$
c) $CH_{3}COCl + C_{2}H_{5}OH + NaOH$
d) $CH_{3}Cl + C_{2}H_{5}COONa$

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2. The structure of the major product formed in the following reaction is

a)
b)
c) ​
d)

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1. Which one of the following undergoes reaction with 50% sodium hydroxide solution to give the corresponding alcohol and acid?
a) Phenol
b) Benzaldehyde
c) Butanol
d) Benzoic acid

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2. Aspirin is known as
a) acetyl salicyclic acid
b) phneyl salicylate
c) acetyl salicylate
d) methane salicylic acid

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1. On heating benzyl amine with chloroform and ethanolic KOH, product obtained by
a) benzyl alcohol
b) benzaldehyde
c) benzonitrile
d) benzyl isocyanide

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2. Fluorobenzene (C₆H₅F) can be synthesized in the laboratory
a) by heating phenol eith HF and KF
b) from aniline by diazotisation followed by heating the diazonium salt with HBF₄
c) by direct fluorination of benzene with F₂ gas
d) by reacting bromobenzene with NaF solution

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1. Identify the correct statement regarding enzymes.
a) Enzymes are specific biological catalysts that can normally function at very high temperatures (T - 1000K)
b) Enzymes are normally heterogeneous catalysts that are very specific in their action
c) Enzymes are specific biological catalysts that cannot be poisoned
d) Enzymes are specific biological catalysts that possess well defined active sites.

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2. Which base is present in RNA but not in DNA?
a) Uracil
b) Cytosine
c) Guanine
d) Thymine

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1. How many EDTA (ethylenediamine tetraacetic acid ) molecules are required to make an octahedral complex with a Ca²⁺ ion?
a) Six
b) Three
c) One
d) Three

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2. Coordination compounds have great importance in biological systems. In this context , which of the following statements is incorrect?
a) Chlorophyll is green pigment in plant and contain calcium
b) Haemoglobin is the red pigment of blood and contains iron
c) Cyanocobalamin is vitamin B₁₂ and contains cobalt
d) Carboxypeptidase-A is an enzyme and contains zinc

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