SUB: CHEMISTRY (Paper – 1)
Max Marks: 70
[Answer all questions in Part – I and six questions from Part - II choosing two questions
from each of the Sections A, B and C.]
PART - I [20 Marks]
Question 1
I.
a.
b.
c.
d.
e.
Fill in the blanks using appropriate words given in the brackets:
[5]
(olefenic, aldol, safety matches, sodium sulphite, homolytic, organometallic, rat
poison, pesticides, antiknock, heterolytic, flowers of sulphur, aldol-condensation,
antichlor, free radicals, hydroxide, charged species)
Red phosphorous is used in manufacture of ____________ and ____________.
TEL is on ____________ compound, is used as an ____________ agent.
The breaking of covalent bonds may be either through ____________ or by
____________ fission.
Hypo is prepared by boiling ____________ solution with ____________ in
alkaline medium.
Acetaldehyde in presence of dilute alkali gives ____________ and the reaction is
called ____________.
II.
Correct the following statements:
a.
b.
Molarity of a solution is independent of temperature.
A system which can exchange neither matter nor energy with surroundings is called
closed system
Linear overlap of two atomic p-orbitals leads to the formation of π-bond.
Graphite has 2-Dimensional sheet like structure in which each C-atom is sp3
hybridised.
Osmotic pressure and boiling point are colligative properties.
c.
d.
e.
[5]
III. Complete the following statements by selecting the correct alternative from
the choices given:
[5]
a.
The mineral that doesn’t contain aluminium is:
i.
Bauxite
iii. Fluorspar
ii.
Feldspar
iv. Cryolite
b.
The process of removing impurities from a crude metal is called:
i.
Concentration
iii. Calcination
ii.
Refining
iv. Roasting
c.
Glucose on treatment with NH4OH undergoes:
i.
Condensation
iii. Reaction
ii.
Hydrolysis
iv. Oxidation
d.
Entropy is an example of:
i.
Intensive property
ii.
Optical-activity
iii.
iv.
Extensive property
Colligative property
e.
A quantitative relationship between temperature and rate constant for a reaction is
given by:
i.
Nernst equation
iii. Arrhenius equation
ii.
Henderson’s equation
iv. Van’t Hoff equation
IV.
Match the following:
a.
b.
c.
d.
e.
Nernst equation
Ostwald’s dilution law
Optical activity
Zwitter ion
Wilkinson’s Catalyst
[5]
-
Glycine
Lactic acid
Organometallic compounds
Weak electrolyte
Electrode potential
PART - II [50 Marks]
SECTION - A [Attempt any two questions]
[20 Marks]
Question 2
a.
An aq. Solution containing 1.70g of cane sugar in 100ml water begins to freeze at 0.093°c. The cryoscopic constant of water is 1.86 K Kg mole-1. Calculate the
molecular weight of cane sugar.
[3]
b.
A decinormal solution of Sodium chloride exerts an osmotic pressure of 4.82 atm at
27°C. Calculate the degree of dissociation of NaCl.
[3]
c.
Define Osmotic Pressure out of 0.1 M of NaCl and glucose. Which will have the
more Osmotic Pressure? Give reasons in support of your answer.
[4]
Question 3
a.
A cell is constructed by dipping a Zn rod in 0.1 M Zn(NO3)2 solution and a lead rod
in 0.2 M Pb(NO3)2 solution.
[4]
2+
2+
E° Pb /Pb = - 0.13V
&
E° Zn /Zn = 0.76V
i.
Write the spontaneous cell reaction.
ii.
Calculate the standard e.m.f and e.m.f of cell.
b.
Explain the purification of NaCl by bubbling HCl gas through its solution. [3]
c.
The initial rate of [A+B  Product] is doubled when the initial concentration of
A is doubled and increases eight-folds when the initial concentration of both
A and B were doubled. State the order of the reaction w.r.t A and w.r.t B.
Write the rate equation.
[3]
Question 4
a.
Draw a graph which is used to calculate the activation energy of a reaction.
Give the appropriate expressions used to calculate the activation energy
graphically.
[4]
Two ionic compounds AB and AB2 have the same solubility product which of the
two compounds has a higher solubility at the same temperature. Justify your
answer.
[4]
b.
i.
How many Na+ and Cl- are present in a unit cell of NaCl?
[2]
ii.
What is co-ordination number of Sodium and Chloride ions in NaCl crystals?
SECTION - B [Attempt any two questions]
[10 Marks]
Question 5
a.
Predict the number of unpaired electrons in the following:
[3]
3+
3i.
[Cr(NH3)6]
ii.
[Fe(CN)6]
iii. Ni(CO)4
b.
Ni(CO)4 has a tetrahedral geometry while [Ni(CN)4]2- has a square planar
geometry. Give reasons.
[2]
Question 6
a.
Write balanced chemical equations for each of the following reactions:
i.
Sodium thiosulphate with aq. AgNO3
ii.
Copper sulphate with aq. Potassium iodide
iii. Ozone with moist Iodine
iv. Hydrogen peroxide with acidified ferrous Sulphate solution
v.
Bleaching powder with excess of dilute HCl.
[5]
Question 7
a.
i.
ii.
Discuss the structure of thiosulphate ion.
[3]
Name one ore each of tin and lead. What is the main constituent
of each?
[2]
SECTION - C [Attempt any two questions]
[20 Marks]
Question 8
a.
b.
How will you convert the following (write the relevant equations):
i.
Acetic anhydride to methyl amine.
ii.
Phenol to Salicylic acid.
iii. Glucose to Osazone.
iv. Phenol to Picric acid.
v.
Formaldehyde to Urotropin.
𝑒𝑒𝑒𝑒ℎ𝑦𝑦𝑦𝑦 𝑎𝑎𝑎𝑎𝑎𝑎
A
B+ C
(Organic compound)
Products
2: 4 𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝐷𝐷
𝑃𝑃ℎ𝑒𝑒𝑒𝑒𝑒𝑒𝑒𝑒 ℎ𝑦𝑦𝑦𝑦𝑦𝑦𝑦𝑦𝑦𝑦𝑦𝑦𝑦𝑦𝑦𝑦 (𝐶𝐶3 𝐻𝐻6 𝑂𝑂)
𝐻𝐻3 𝑂𝑂+
E
(C3H6O)
B+
[5]
[3]
D
KMnO4
𝐶𝐶𝐶𝐶(𝑂𝑂𝑂𝑂)2
B
E doesn’t react with Tollen’s reagent and Fehling solution.
Identify A, B, C, D and E.
Question 9
a.
C6H5CONH2
𝐵𝐵𝐵𝐵2 /𝐾𝐾𝐾𝐾𝐾𝐾
A
𝐶𝐶𝐶𝐶𝐶𝐶𝐶𝐶3
+
𝐾𝐾𝐾𝐾𝐾𝐾
(𝑖𝑖)𝑁𝑁𝑁𝑁𝑁𝑁𝑁𝑁2 /𝐻𝐻𝐻𝐻𝐻𝐻
(𝑖𝑖𝑖𝑖)𝑆𝑆𝑆𝑆𝑆𝑆𝑆𝑆𝑆𝑆
D
B
𝐶𝐶6 𝐻𝐻5 𝑁𝑁2 𝐶𝐶𝐶𝐶
𝑖𝑖𝑖𝑖𝑖𝑖 𝑐𝑐𝑐𝑐𝑐𝑐𝑐𝑐
C
[3]
CH3COOH
E
Identify A, B, C, D and E.
b.
Draw the isomer of the following and name the type of isomerism:
[5]
i.
C4H10
iii. CHCl = CHCl
v.
CH3CHOHCOOH
ii.
C2H6O
iv. C4H8
Question 10
a.
b.
Match the items in the following two columns:
i.
Ascorbic acid
a.
ii.
Haemoglobin
b.
iii. Glyceride
c.
iv. Insulin
d.
v.
Phospholipids
e.
vi. Testosterone
f.
[6]
Blood glucose
Cell membrane
Male sex hormone
Oxygen transport
Scurvy
Ester
Give two tests each to distinguish between:
i.
Acetaldehyde and Acetone
ii.
Aniline and Dimethylaniline
************
[4]