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Aieee Chemistry   2006
 

Aieee Chemistry 2006

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Aieee Chemistry   2006 Aieee Chemistry 2006 Presentation Transcript

  • AEEE –Past papers
    CHEMISTRY - UNSOLVED PAPER - 2006
  • SECTION – I
    Straight Objective Type
    This section contains multiple choice questions numbered 55 . Each question has 4 choices (A), (B), (C) and (D), out of which ONLY ONE is correct.
  • 01
    Problem
    HBr reacts with CH2 = CH – OCH3 under anhydrous conditions at room temperature to give
    CH3CHO and CH3Br
    BrCH2CHO and CH3OH
    BrCH2 – CH2 – OCH3
    H3C – CHBr – OCH3
  • Problem
    02
    The IPUAC name of the compound shown below is :
     
    2-bromo-6-chlorocyclohex-1-ene
    6-bromo-2-chlorocyclohexene
    3-bromo-1-chlorocyclohexene
    1-bromo-3-chlorocyclohexene
  • Problem
    03
    The increasing order of the rate of HCN addition to compounds A-D is :
    HCHO
    CH3COCH3
    PhCOCH3
    PhCOPh
    A < B < C < D
    D < B < C < A
    D < C < B < A
    C < D < B < A
  • Problem
    04
    How many moles of magnesium phosphate, Mg3(PO4)2 will contain 0.25 mole of oxygen atoms ?
     
    0.02
    3.125 x 10-2
    1.25 x 10-2
    2.5 x 10-2
  • Problem
    05
    According to Bohr’s theory, he angular momentum of an electron in 5th orbit is :
     
    25
    b. 1.0
    c. 10
    d. 2.5
  • Problem
    06
    Which of the following molecules/ions does not contain unpaired electrons ?
     
    O
    B2
    N
    O2 
  • Problem
    07
    Total volume of toms present in a face-centred cubic unit cell of metal is (r is atomic radius) :
    a.
    b.
    c.
    d.
  • Problem
    08
    A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will:
     
    Remain unchanged
    Triple
    Increases by a factor of 4
    Double
  • Problem
    09
    Which of the following chemical reactions depicts the oxidizing behaviour of H2SO4 ?
     
    2HI + H2SO4 I2 + SO2 + 2H2O
    Ca(OH)2 + H2SO4 CaSO4 + 2H2O
    NaCl + H2SO4 NaHSO4 + HCl
    2PCl5 + H2SO4 2POCl3 + 2HCl + SO2Cl2
  • Problem
    10
    The IUPAC name for he complex [Co(NO2)(NH3)5]Cl2 is :
    Nitrite-N-pentaminecobalt (III) chloride
    Nitrite-N-pentamminecobalt (II) chloride
    Pentammine nitrite-N-cobalt (II) chloride
    Pentaamine nitrite-N-cobalt (III) chloride
  • Problem
    11
    The term anomers of glucose refers to :
    Isomers of glucose that differ configuration at carbons one and four (C-1 and C - 4)
    A mixture of (D)-glucose and (L)- glucose
    Enantiomers of glucose
    Isomers of glucose that differ in configuration at carbon one (C - 1)
  • Problem
    12
    In the transformation of if one emission is an -particle, what should be the other emission (s) ?
     
    Two -β
    Two -βand one + β
    One β and one
    One β and one β
  • Problem
    13
    Phenyl magnesium bromide reacts with methanol to give :
    A mixture of anisol and Mg(OH)Br
    A mixture of benzene and Mg(OMe)Br
    A mixture of toluence and Mg(OH)Br
    A mixture Phenol and Mg (Me)Br
  • Problem
    14
    The decreasing order of the rate of the above reaction with nucleophiles (Nu-) A to D is : [Nu- = (A) PhO-, (B)AcO-, (C) HO-, (D) CH3O-]
     
    D > C > A < B
    D > C > B > A
    A > B > C > D
    B > D > C > A
  • Problem
    15
    The pyrimidine bases present in DNA are :
     
    Cytosine and adenine
    Cytosine and guanine
    Cytosine and thymine
    Cytosine and uracil
  • Problem
    16
    Among the following the one that gives positive iodoform test upon reaction with I2 and NaOH is :
    a. CH3CH2CH(OH)CH2CH3
    b. C6H5CH2CH2OH 
    PhCHOHCH3
     
  • Problem
    17
    The increasing order of stability of the following free radicals is :
     
    (CH3)2 H < (CH3)3 < (C6H5)2 H < (C6H5)3
    (C6H5)3 (C6H5)2 H< (CH3)3 < (CH3)2 H
    (C6H5)2 H<(C6H5)3 <(CH3)3 < (CH3)2 H
    (CH3)2 H < (CH3)3 < (C6H5)3 < (C6H5)2 H
  • Problem
    18
    Uncertainty in the position of an electron (mass = 9.1 x 10-31 kg) moving with a velocity 300 ms-1, accurate upon 0.001% will be :
     
    19.2 x 10-2 m
    5.76 x 10-2 m
    1.92 x 10-2 m
    3.84 x 10-2 m
    (h= 6.63 x 10-34 Js)
  • Problem
    19
    Phosphorus pentachloride dissociates as follows, in a closed reaction vessel,
    If total pressure at equilibrium of the reaction mixture is P and degree of dissociation of PCl5 is x, the partial pressure of PCl3 will be:
    a.
    b.
    c.
    d.
  • Problem
    20
    The standard enthalpy of formation at 298 K for methane, CH4(g), is -78.4 kJ mol-1. The additional information required to determine the average energy for C-H bond formation would be:
     
    The dissociation energy of H2 and enthalpy of sublimation of carbon
    Latent heat of vaporization of methane
    The first four ionization energies of carbon and electron gain enthalpy of hydrogen
    The dissociation energy of hydrogen molecule, H2
  • Problem
    21
    Among the following mixtures, dipole-dipole as the major interaction, is present in:
     
    Benzene and ethanol
    Acetonitrile and acetone
    KCl and water
    Benzene and carbon tetrachloride
  • Problem
    22
    Fluorobenzene (C6H5F) can be synthesized in the laboratory:
     
    By heating phenol with HF and KF
    From aniline by diazotization followed by heating the diazonium salt with HBF4
    By direct fluorination of benzene with F2 gas
    By reacting bromobenzene with NaF solution
  • Problem
    23
    A metal, M forms chlorides in its + 2 and + 4 oxidation states. Which of the following statements about these chlorides is correct?
     
    MCl2 is more volatile than MCl4
    MCl2 is more soluble in anhydrous ethanol than MCl4
    MCl2 is more ionic than MCl4
    MCl2 is more easily hydrolysed than MCl4
  • Problem
    24
    Which of the following statement is true ?
     
    H3PO3 is stronger acid than H2SO3­
    In aqueous medium HF is a stronger acid than HCl
    HClO4 is a weaker acid than HClO3
    HNO3 is a stronger acid than HNO2
  • Problem
    25
    The molar conductivities at infinite dilution in water at 250C are 91.0 and 426.2 S cm2/ mol respectively. To calculate the additional value required is:
    a.
    b.
    c.
    d.
  • Problem
    26
    Which one of the following sets of ions represents a collection of isoelectronic species ?
     
    K+, Cl-, Ca2+, Sc3+
    Ba2+, Sr2+, K+, S2-
    N3-, O2-, F-, S2-
    Li+, Na+, Mg2+, Ca2+
  • Problem
    27
    The correct order of increasing acid strength of the compounds:
    CH2CO2H
    MeOCH2CO2H
    CF3CO2H
     
    B < D < A < C
    D < A < C < B
    D < A < B < C
    A < D < C < B
  • Problem
    28
    In which of the following molecules/ions all the bonds are not equal?
     
    SF4
    SiF4
    XeF4
    BF4
  • Problem
    29
    What products are expected from the disproportionation reaction of hypochlorous acid?
     
    HClO3 and Cl2O
    HClO2 and HClO4
    HCl and Cl2O
    HCl and HClO3
  • Problem
    30
    Nickel (Z = 28) combines with a uninegativemonodentateligand X- to form a paramagnetic complex [NiX4]2-. The number of unpaired electron(s) in the nickel and geometry of this complex ion are respectively :
     
    One, tetrahedral
    Two, tetrahedral
    One, square planar
    Two, square planar
  • Problem
    31
    In Fe(CO)s, the Fe-C bond possesses:
     
    Character only
    Both and characters
    Ionic character
    Character only
  • Problem
    32
    The increasing order of the first ionization enthalpies of the elements B, P, S and F (lowest first) is :
     
    F < S < P < B
    P < S < B < F
    B < P < S < F
    B < S < P < F
  • Problem
    33
    An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system, If Ti is the initial temperature and Tf is the final temperature, which of the following statements is correct ?
     
    (Tf)irrev > (Tf)rev
    Tf > Ti for reversible process but Tf = Ti for irreversible process
    (Tf)rev = (Tf)irrev
    Tf = Ti for both reversible and irreversible
  • Problem
    34
    In languir’s model of adsorption of a gas on a solid surface :
     
    The rate of dissociation of adsorbed molecules from the surface does not depend on the surface covered
    The adorption at a single site on the surface may involve multiple molecules at the same time
    The mass of gas striking a given area of surface is proportional to the pressure of the gas
    The mass of gas striking a given area of surface is independent of the pressure of the gas
  • Problem
    35
    Rate of a reaction can be expressed by Arrhenius equation as: k = A e−E /RT In this equation, E represents
    the energy above which all the colliding molecules will react
    the energy below which colliding molecules will not react
    the total energy of the reacting molecules at a temperature, T
    the fraction of molecules with energy greater than the activation energy of the reaction
  • Problem
    36
    The structure of the major product formed in the following reaction is :
    a.
    b.
    c.
    d.
  • Problem
    37
    Reaction of trans-2-phenyl-1-bromocyclopentane on reaction with alcoholic KOH produces:  
    4-phenylcyclopentene
    2-phenylcylocpentene
    1-phenylcylopentene
    3-phenylcylopentene
  • Problem
    38
    Increasing order of stability among the three main conformations (i.e., Eclipse, Anti, Gauche) of 2-fluoroethanol is :
     
    Eclipse, Gauche, Anti
    Gauche, Eclipse, Anti
    Eclipse, Anti, Gauche
    Anti, Gauche, Eclipse
  • Problem
    39
    The structure of the compound that gives a tribromo derivative on treatment with bromine water is
    a.
    b.
    c.
    d.
  • Problem
    40
    The decreasing values of bond angles form NH3(1060) to SbH3(1010) down group-15 of the periodic table is due to:
     
    Increasing bp-bp repulsion
    Increasing p-orbital character in sp3
    Decreasing lp-bp repulsion
    Decreasing electronegativity 
  • Problem
    41
    The alkene formed as a major product in the above elimination reaction is
     The ‘spin-only’ magnetic moment [in units of Bohr magneton, ( )] of Ni2+ in aqueous solution would be (Atomic number of Ni = 28) :
    a. b.
    c. d.
     
  • Problem
    42
    The ‘spin – only’ magnetic moment in uints of Bohr magneton, of Ni2+ in aueous solution would be (automatic number of Ni =28):
    2.84
    4.90
    0
    1.73
  • Problem
    43
    The equilibrium constant for the reaction is
    Kc= 4.9 x 10-2. The value of Kc for the reaction will be:
     
    416
    2.40 x 10-3
    9.8 x 10-2
    4.9 x 10-2
  • Problem
    44
    Following statements regarding the periodic trends of chemical reactivity of the alkali metals and the halogens are given. Which of these statements gives the correct picture?
     
    The reactivity decreases in the alkali metals but increases in the halogens with increase in atomic number down the group
    In both the alkali metals and the halogens the chemical reactivity decreases with increase in atomic number down the group
    Chemical reactivity increases with increase in atomic number down the group in both the alkali metals and halogens
    In alkali metals the reactivity increases but in the halogens it decreases with increase in atomic number down the group
  • Problem
    45
    Given the data at 250C,
    Ag + I-AgI + e- ; E0 = 0.152 V
    Ag Ag+ + e - ; E0 = - 0.800 V
    What is the value of log Ksp for AgI ?
    -8.12
    + 8.612
    - 37.83
    - 16.13
  • Problem
    46
    The following mechanism has been proposed for the reaction of NO with Br2 to form NOBr:
    NO(g) + Br2(g) NOBr2 (g)
    NOBr2 (g) + NO (g) 2NOBr(g)
    If the second step is the rate determining step, the order of the reaction with respect to NO (g) is :
     
    1
    0
    3
    2
  • Problem
    47
    Lanthanoid contraction is caused due to :
     
    The appreciable shielding on outer electrons by 4f electrons from the nuclear charge
    The appreciable shielding on outer electrons by 5d electrons from the nuclear charge
    The same effective nuclear charge from Ce to Lu
    The imperfect shielding on outer electrons by 4f electrons from the nuclear charge
  • Problem
    48
    Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.01 M is 100 . The conductivity of this solution is 1.29 S m-1. Resistance of the same cell when filled with 0.2 M of the same solution is 520 . The molar conductivity of 0.02 M solution of the electrolyte will be :
     
    124 x 10-4 S m2 mol-1
    1240 x 10-4 S m2 mol-1
    1.24 x 10-4 S m2 mol-1
    12.4 x 10-4 S m2 mol-1
  • Problem
    49
    The ionic mobility of alkali metal ions in aqueous solution is maximum for :
     
    K+
    Rb+
    Li+
    Na+
  • Problem
    50
    Density of a 2.05 M solution of acetic acid in water is 1.02 g/ml. The molality of the solution is :
     
    1.14 mol kg-1
    3.28 mol kg-1
    2.28 mol kg-1
    0.44 mol kg-1
  • Problem
    51
    The enthalpy changes for the following processes are listed below :
    Cl2(g) = 2Cl(g), 242.3 kJ mol-1
    I2(g) = 2I (g), 151.0 kJ mol-1
    ICl (g) = I (g) + Cl (g), 211.3 kJ mol-1
    I2(s) = I2 (g), 62.76 kJ mol-1
    Given that the standard states for iodine and chlorine are I2(s) and Cl2(g), the standard enthalpy of formation of ICI (g) is :
     
    - 14.6 kJ mol-1
    -16.8 kJ mol-1
    + 16.8 kJ mol-1
    + 244.8 kJ mol-1
  • Problem
    52
    How many EDTA (ethylenediaminetetra acetic acid) molecules are required to make an octanhedral complex with a Ca2+ ion?
     
    Six
    Three
    One
    Two
  • Problem
    53
    The electrophile involved in the above reaction is :
     
    Dichloromethylcation ( HCl2)
    Dichlorocarbene (: CCl2)
    Trichloromethyl anion ( Cl2)
    Formylcation ( HO)
  • Problem
    54
    18 g of glucose (C6H12O6) is added to 178.2 g of water. The vapour pressure of water for this aqueous solution at 1000C is :
     
    759.00 torr
    7.60 torr
    76.00 torr
    752.40 torr
  • Problem
    55
    for the formation of carbon monoxide (CO) from its elements at 298 K is : (R = 8.314 JK-1 mol-1)
     
    -1238.78 J mol-1
    1238.78 J mol-1
    -2477.57 J mol‑1
    2477.57 J mol-1
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