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CHEMISTRY
1. Mohr's salt is:
(1) FeSO4.7H2O
(2) FeSO4(NH4)2SO4.6H2O
(3) MgSO4.7H2O
(4) Fe(SO4)3(NH4)2SO4.6H2O 2. Asbestos is:
(1) Calcium silicate
(2) Magnesium silicate
(3) Calcium-magnesium silicate
(4) Alumina 3. Nichrome used as heating element in hot-air oven is an alloy of:
(1) Ni and Cr
(2) Ni and Fe
(3) Fe and Cr
(4) Ni, Fe and Cr 4. The indicator used to detect the end point in the titration of a
weak acid and strong base (pH-8-10) is:
(1) Methyl orange
(2) Methyl red
(3) Phenolphthalein
(4) Litmus 5. The monomer unit of polyvinyl chloride unit has the formula:
CH2=CH2
(1)
(2) CH3=CH2CI
(3) CH2=CHCI
(4) CHCI=CHCI 6. According to Markownikoff's rule, when hydrogen chloride adds
to an unsymmetrical alkene, the hydrogen of HX attaches to:
number of hydrogens
(1) Carbon with least
(2) Carbon with most number of hydrogens
(3) Carbon at the end of the molecule
(4) Carbon in the middle of the molecule 7. Which fraction of the petroleum
corresponds to kerosene oil?
(1) C1-C4
(2) C5-C9
(3) C10-C12
(4) C15-C18 8. Phenol reacts with bromine water to give
(2) 4-bromophenol
(3) 2,4-dibromophenol
(1) 2-bromophenol
(4) 2,4,6-tribromophenol 9. Which one of the following gives iodoform test?
Formaldehyde
(1)
(2) Benzaldehyde
(3) Ethanol
(4) Benzyl alcohol 10. Amino acids are produced by the hydrolysis of:
Carbohydrates
(1)
(2) Fats
(3) Nuclei acids
(4) Proteins 11. Froth flotation process is primarily used to concentrate......ores
(1) Chloride
(2) Silicate
(3) Carbonate
(4) sulphide 12. Stainless steel is an alloy of iron with:
(1) 12% Cr, 1% Ni
(2) 2% Cr, 3% C
(3) 10% Ni, 2% Mn
(4) 8% Cr, 5% Mn 13. Presence of halogens is organic compounds is detected by:
(1) Iodoform test
(2) Silver nitrate test
(3) Millon's test
(4) Beilstein's test 14. Number of ions present in K3[Fe(CN)6] are:
(1) 2
(2) 3
(3) 4
(4) 10 15. During the extraction of copper from chalcopyrites, the matter obtained is
mainly.
(1) Cuprous sulphide
(2) Cuprous oxide
(3) Mixture of cuprous oxide and sulphide
(4) Copper metal 16. Potassium metasulphite used as a food preservative is:
A positive catalyst
(2) A negative catalyst
(3) A homogeneous catalyst
(4) A heterogeneous catalyst 17.` Highest pH (14) is given by:
(2) IN NaOH
(1) IN HCI
(1)
(3) 0.1M NaOH
(4) IM H2SO4 18. The free energy change due to a reaction is zero when:
reactants are completely consumed
(1) The
(2) The system is at equilibrium
(3) A catalyst is added
(4) The reactants are initially mixed 19. For the reaction CI2(g) + 2 NO (g) 2
NOCI (g) doubling the concentration of both reactants increases the rate by a factor of
eight. If only the concentration of CI2 is doubled, the rate increases by a factor of two,
The order of the reaction with respect to NO is:
(1) 1
(2) 2
(3) 0.5
(4) 3 20. In the Daniel cell constructed in the laboratory, the voltage observed was
0.9 V instead of 1.1 V of the standard cell. A possible explanation is:
[Cu2+]
(1) [Zn2+] >
(2) [Zn2+] < [Cu2+]
(3) The Zn electrode has twice the surface of Cu electrode
(4) Mole ratio of Zn2+ : Cu2+ is 2 :1 21. The compound which does not leave any
residue on heating is:
(1) AgNO3
(2) CuSO4
(3) NH4NO3
(4) NaNO3 22. Oxidation number of P in H3PO2 is:
(1) +5
(2) +3
(3) +2
(4) +1 23. The H-O-H bond angle in water is:
(1) 1090280
(2) 900
(3) 1800
(4) 1040500 24. Which of the following is a complex halide ion?
(1) HF
(2) KBr
(3) KI3
(4) CCI4 25. The IUPAC name of CH2= CHCH(CH3)2 is:
propene
(2) 3-methyl-1-butene
(3) 2-vinyl propene
(1) 1, 1-dimethyl-2-
(4) I-isopropyl ethylene 26. Usually ionic compounds are soluble in polar solvents
and covalent compounds is non-polar solvents. However covalent compounds dissolve in
polar solvents like water due to:
(1) H-bond formation
(2) Proton transfer reaction
(3) Their behaviour as Lewis acids
(4) Any of the above 27. Nitrogen atom has three unpaired electrons because of:
(1) Aufbau principle
(2) Pauli's Exclusion principle
(3) Uncertainly principle
(4) Hund's rule 28. Which of the following set of quantum numbers is not possible?
n l m1 ms
(1) 3 2 1 +1/2
(2) 3 2 1 - 1/2
(3) 3 2 1 0
(4) 3 2 -1 + 1/2 29. The magnetic quantum number m1 is fixed by the azimulthal
quantum number 1. If 1=2, the type and number of orbitals are indicated by:
(1) 3s, 1
(2) 3P,3
(3) 3d,5
(4) 4f,7 30. The molecule with highest % ionic character is:
(1) HF
(2) HCI
(3) HBr
(4) HI 31. Assuming sweetness of the cane sugar to be 10, the sweetness of glucose
is
(1) 5
(2) 15
(3) 7.5
(4) 12.5 32. Nitric acid is manufactured by
(1) Ostwald's process
(2) Deacon's process
(3) Contact process
(4) Lablanc process 33. The percentage of nitrogen in urea is:
(1) 25
(2) 46
(3) 54
(4) 59 34. The chemical formula of pyrophosphoric acid is
(1) H4P2O7
(2) HPO3
(3) H3PO4
(4) H3PO3 35. Mixture of white dnd red phosphorus can be separated by using:
(1) Iodine
(2) Kerosene
(3) NaOH
(4) HNO3 36. In nucleic acids the sequence is
(1) Base-sugar-phosphate
(2) Base-phosphate-sugar
(3) Phosphate-base-sugar
(4) Sugar-base-phosphate 37. Which of the following is an example of heterogeneous
catalyst?
FeCl3
(1) 2H2O2(aq) 
2H2O+O2
MnO2
(2) 2H2O2(aq) 
2H2O+O2
H+

(3) Sucrose + H2O
glucose+fructose
NO
(4) 2SO2+O2+2H2O

2H2SO4
38. Catalyst used in Friedel-Craft's reaction is
(1) Anhydrous aluminium chloride
(2) Sodium
(3) Ferric chloride
(4) Zinc oxide 39. Which of the following can give a buffer solution?
NaOH
(1) HCI +
(2) CH3COONa +HCI
(3) HCOOH + HCOONa
(4) H2SO4 + Na2SO4 40. In an FCC metal the atoms are in physical contact along
(1) Body diagonal
(2) Face diagonal
(3) Cube edge
(4) All the above directions 41. A real gas tends to behave more ideally at:
High temperature and high pressure
(1)
(2) High temperature and low pressure
(3) Low temperature and high pressure
(4) Low temperature and low pressure 42. The half-life of a radioactive isotope is 1.5
hours. If its initial mass is 32 grams, the mass that remains after 6 hours is
(1) 2g
(2) 4g
(3) 8g
(4) 16g ` 43. The shape of atomic orbitals is given by
number
(1) Principal quantum
(2) Subsidiary quantum number
(3) Magnetic quantum number
(4) Spin quantum number 44. High purity hydrogen is produced by the reaction
(1)
(2)
(3)
(4) 45. H2O2 is
(1) An oxidizing agent
(2) A reducing agent
(3) Both an oxidizing and a reducing agent
(4) Neither oxidizing nor reducing agent 46. Calculate H0 for the reaction H2O (l)
(g) +O2(g) given 2 H2 (g) +O2(g) (l) H=-571.6 kJ
(1) - 285.8 kJ
(2) 285.8 kJ
(3) -571.6 kJ
(4) 571.6 kJ 47. P2O5 is an anhydride of
(1) H2PO3
(2) H3PO4
(3) HPO3
(4) H4P2O7 48. Identify the reaction which is endothermic:
 HCI (aq)
(2) NH4NO3(s) +H2O (l) NH4NO3(aq)
(1) HCI (g) + H2O (l)
(3) H2SO4(l) +H2O (l) H2SO4(aq)
(4) NaOH(s) +2H2O (l) NaOH(aq) 49. In which of the following systems at
equilibrium and room temperature, doubling the volume will shift the reaction to the
right?
(1) PCI5(g)PCI3(g) + CI2(g)
(2) N2(g)3 H2(g) 2NH3(g)
(3) 2NOCI(g)2(g)2CO2(g)
(4) H2(g)CI2(g) 2 HCI(g) 50. For which of the following reactions kp and ke are
numerically equal?
(1) H2 (g) + I2 (s) 2HI (g)
(2) H2 (g) + CI2 (g) 2HCI (g)
(3) 2 NOCI (g) 2HO(g) +CI2 (g)
(4) COCI2(g)2 HCI (g) 51. An example of an amino acid containing benzene ring
is :
(1) Alanine
(2) Tyrosine
(3) Lysine
(4) Serine 52. Among the naturally occurring carbohydrates, furanose ring is found in
the
(1) Galactose unit of lactose
(2) Glucose unit of cellulose
(3) Fructose unit of cane sugar
(4) Glucose unit of cane sugar 53. Two other useful by-products of Solvay pressure
are:
(1) NaHCO3 and CO2
(2) NH4CI and CaO
(3) NaHCO3 and NH4CI
(4) CaO and CO2 54. Aromatic primary amine when treated with cold HNO2 gives:
(1) Benzyl alcohol
(2) Nitrobenzene
(3) Diazonium salt
(4) Benzene 55. Functional group present in cresol is:
(1) Alcoholic-OH
(2) Aldehydic-CHO
(3) Phenolic-OH
(4) Carboxylic-COOH 56. During the titration of KMnO4 with oxalic acid in acid
medium, the oxidation number of MN+7 changes to:
(1) +5
(2) +3
(3) +2
(4) 0 57. In the reaction of NO-3 ions with Cu turnings and cone, H2SO4 the blue
solution formed is due to
(1) Cu(NO3)2
(2) CuSO4
(3) Cu(HSO4)2
(4) Cu(NO2)2 58. Acetylene reacts with HBr to give
(1) CH3Br
(2) C2H5Br
(3) Ethylene bromide
(4) Ethylidene bromide 59. Aldehydes and ketones can be distinguished by:
Bromoform
(1)
(2) Tollen's test
(3) Molisch test
(4) Solubility in water 60. Ethyl bromide can be obtained by the action of H Br on
(1) Ethanol
(2) Ethane
(3) Propene
(4) AcetyleneRA