SOLVE THE SAMPLE PAPER
1. Give the IUPAC
name of (CH3)3 – C – COOH.
2. What is meant by
protective colloid?
3. Define coagulation
value.
4. Give the role of
desorption in the process of catalysis.
5. What is an isoelectric
point?
6. How is cast iron
different from pig iron?
7. Give reasons:
(i) Aldehydes do
not form stable hydrates but chloral exists as chloral hydrate.
(ii) Acetic acid
can be halogenated in presence of red phosphorus and chlorine but formic
acid cannot
be halogenated.
8. Give the application of Henry’s law on scuba drivers.
9. Explain Frenkel defect.
10. Silver forms ccplattice and X-ray studies
of its crystals show that the edge length of its unit cell is
408.6 pm. Calculate
the density of silver (Atomic mass = 107.9 u).
11. Write a note on order of a reaction.
12. (a) Identify all the possible monochloro structural isomers
expected to be formed on free radical
monochlorination
of (CH3)2CHCH2CH3.
(b) During the
reaction of alcohols with KI, sulphuric acid is not used. Give reason.
(c) Alkyl halides
though polar, are immiscible with water. Why?
13. How the presence of sulphur dioxide is detected?
14. Vapour pressure of chloroform (CHCl3) and dichloromethane (CH2Cl2) at 298 K are 200 mm Hg
and 415 mm Hg respectively.
 15 .(a)
Calculate the vapour pressure of the solution prepared by mixing 25.5 g of CHCl3 and 40 g of
CH2Cl2
at 298 K.
(b) The mole fractions
of each component in vapour phase.
16. Complete the following reactions:
(a) HgCl2 + PH3
(b) NaClO3 + I2
(c) SCl2+ NaF
17. Define the term:
(a) Monosaccharides
(b) Oligosaccharides
(c) Polysaccharides
18. Calculate the mole
fraction of ethylene glycol (C2H6O2) in a solution
containing 20% of C2H6O2by
mass.
20. (a) Why noble
gases have low boiling points?
(b) Why are the
elements of group 18 known as noble gases?
(c) Why He is used
in diving apparatus?
21. What are the factors which determine the magnitude of
the orbital splitting energy?
22.How the nature of the ligand affect
the stability of a complex ion?
23. Differentiate addition and condensation polymers.
24. The decomposition of N2O5 in
CCl4 at 318K has been studied by monitoring the concentration of
N2O5
in the solution. Initially the concentration
of N2O5 is 2.33 mol L–1 and after 184 minutes,
it is
reduced to 2.08
mol L–1.
The reaction takes place according to the equation
2N2O5
(g) 4 NO2 (g) + O2 (g)
(a) Calculate the
average rate of this reaction in terms of hours, minutes and seconds.
(b) What is the
rate of production of NO2 during
this period?
25. (a) Give the structures
of chromate ion and dichromate ion.
(b) Give the preparation
of potassium permanganate.
(c) Give the structure
of manganite ion and permanganate ion.
(d) Give the schematic
representation of chemical reactions of lanthanoids.
26. Convert the following
into benzoic acid:
(a) Ethylbenzene
(b) Acetophenone
(c) Bromobenzene
(d) Styrene
27. An organic compound
X contains 69.77% C, 11.63% H and rest Oxygen. The molecular mass of
the compound is
86. The compound X does not reduce Tollen’s reagent, but forms an addition
compound with sodium
hydrogen sulphite and gives positive iodoform test. On vigorous
oxidation, X gives
ethanoic and propanoic acids. Identify the possible structure of X.
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