General Instructions :

Read the following instructions very carefully and follow them :

(i) This question paper contains 35 questions. All questions are

compulsory.

(ii) Question paper is divided into FIVE sections – Section A, B, C, D

and E.

(iii) In section – A : Question Numbers 1 to 18 are Multiple Choice (MCQ) type

Questions carrying 1 mark each.

(iv) In section – B : Question Numbers 19 to 25 are Very Short Answer (VSA)

type questions carrying 2 marks each.

(v) In section – C : Question Numbers 26 to 30 are Short Answer (SA) type

questions carrying 3 marks each.

(vi) In section – D : Question Numbers 31 and 32 are case based questions

carrying 4 marks each.

(vii) In section – E : Question Numbers 33 to 35 are Long Answer (LA) type

questions carrying 5 marks each.

(viii) There is no overall choice. However, an internal choice has been provided in
2 questions in Section – B, 2 questions in Section – C, 2 questions in
Section – D and 2 questions in Section – E.

(ix) Use of calculators is NOT allowed.

SECTION – A

1. The magnetic moment of [NiCl4]2– 1

(a) 1.82 BM (b) 2.82 BM

(c) 4.42 BM (d) 5.46 BM

[Atomic number : Ni = 28]

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2. The following experimental rate data were obtained for a reaction carried
out at 25 C : 1
A(g) + B(g)  C(g) + D(g)
Initial [A(g)]/mol dm–3 Initial [B(g)]/mol dm–3 Initial rate/mol dm–3s–1
3.0 × 10–2 2.0 × 10–2 1.89 × 10–4
3.0 × 10–2 4.0 × 10–2 1.89 × 10–4
6.0 × 10–2 4.0 × 10–2 7.56 × 10–4
What are the orders with respect to A(g) and B(g) ?
Order with respect to A(g) Order with respect to B(g)
(a) Zero Second
(b) First Zero
(c) Second Zero
(d) Second First

3. Consider the following standard electrode potential values : 1

Sn2+(aq) + 2e–  Sn(s) E = – 0.14 V
Fe3+(aq) + e–  Fe2+(aq) E = + 0.77 V
What is the cell reaction and potential for the spontaneous reaction that
occurs ?
(a) 2 Fe2+(aq) + Sn2+(aq)  2 Fe3+(aq) + Sn(s) E = – 0.91 V
(b) 2 Fe3+(aq) + Sn(s)  2 Fe2+(aq) + Sn2+(aq) E = + 0.91 V
(c) 2 Fe2+(aq) + Sn2+(aq)  2 Fe3+(aq) + Sn(s) E = + 0.91 V
(d) 2 Fe3+(aq) + Sn(s)  2 Fe2+(aq) + Sn2+(aq) E = + 1.68 V

4. Which of the following cell was used in Apollo space programme ? 1

(a) Mercury cell (b) Daniel cell
(c) H2–O2 Fuel cell (d) Dry cell

5. Which of the following alcohols will not undergo oxidation ? 1

(a) Butanol (b) Butan-2-ol
(c) 2-Methylbutan-2-ol (d) 3-Methylbutan-2-ol

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6. The unit of molar conductivity is 1
(a) S cm–2 mol–1 (b) S cm2 mol–1
(c) S–1 cm2 mol–1 (d) S cm2 mol

7. Out of the following 1.0 M aqueous solutions, which one will show largest
freezing point depression ? 1
(a) NaCl (b) Na2SO4
(c) C6H12O6 (d) Al2(SO4)3

8. Which of the following molecules has a chiral centre correctly labelled

with an asterisk (*) ? 1
(a) CH3C*HBrCH3 (b) CH3C*HClCH2Br
(c) HOCH2C*H(OH)CH2OH (d) CH3C*Br2CH3

9. In the reaction 1
C6H5NH2 + CHCl3 + 3 KOH  A + 3B + 3C the product A is
(a) C6H5NC (b) C6H5CN
(c) C6H5Cl (d) C6H5NHCH3

10. -pleated sheet structure in proteins refers to 1

(a) primary structure (b) secondary structure
(c) tertiary structure (d) quaternary structure

11. Four half reactions I to IV are shown below : 1

I. 2Cl–  Cl2 + 2e–
II. 4OH–  O2 + 2H2O + 2e–
III. Na+ + e–  Na
IV. 2H+ + 2e–  H2
Which two of these reactions are most likely to occur when concentrated
brine is electrolysed ?
(a) I and III (b) I and IV
(c) II and III (d) II and IV

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12. Which property of transition metals enables them to behave as catalysts ? 1
(a) High melting point (b) High ionisation enthalpy
(c) Alloy formation (d) Variable oxidation states

13. Which of the following would not be a good choice for reducing
nitrobenzene to aniline ? 1
(a) LiAlH4 (b) H2/Ni

(c) Fe and HCl (d) Sn and HCl

14. Which one of the following has lowest pKa value ? 1

(a) CH3 – COOH (b) O2N – CH2 – COOH

(c) Cl – CH2 – COOH (d) HCOOH

For questions number 15 to 18, two statements are given – one labelled as
Assertion (A) and the other labelled as Reason (R). Select the correct answer
to these questions from the codes (a), (b), (c) and (d) as given below :
(a) Both Assertion (A) and Reason (R) are true and Reason (R) is the
correct explanation of the Assertion (A).
(b) Both Assertion (A) and Reason (R) are true, but Reason (R) is not the
correct explanation of the Assertion (A).
(c) Assertion (A) is true, but Reason (R) is false.
(d) Assertion (A) is false, but Reason (R) is true.

15. Assertion (A) : The backbone of DNA and RNA molecules is a chain
consisting of heterocyclic base, pentose sugar and phosphate group. 1

Reason (R) : Nucleotides and nucleosides mainly differ from each other
in presence of phosphate group.

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16. Assertion (A) : Order of reaction is applicable to elementary as well as
complex reactions. 1
Reason (R) : For a complex reaction molecularity has no meaning.

17. Assertion (A) : The final product in Aldol condensation is always -
unsaturated carbonyl compound. 1
Reason (R) : -unsaturated carbonyl compounds are stabilised due to
conjugation.

18. Assertion (A) : [Co(NH3)5 SO4] Cl gives a white precipitate with silver
nitrate solution. 1
Reason (R) : The complex dissociates to give Cl– and SO42– ions.

SECTION – B

19. For the pair phenol and cyclohexanol, answer the following : 2×1=2
(a) Why is phenol more acidic than cyclohexanol ?
(b) Give one chemical test to distinguish between the two.

20. (a) Which of the following species cannot act as a ligand ? Give reason.
OH–, NH4 , CH3NH2, H2O 2×1=2
(b) The complex [Co(NH3)5(NO2)]Cl2 is red in colour. Give IUPAC name
of its linkage isomer.

21. What happens to the rate constant k and activation energy Ea as the
temperature of a chemical reaction is increased ? Justify. 2

22. Why haloarenes are not reactive towards nucleophilic substitution

reaction ? Give two reasons. 2

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23. (a) (i) What should be the signs (positive/negative) for ECell and G
for a spontaneous redox reaction occurring under standard
conditions ? 2×1=2
(ii) State Faraday’s first law of electrolysis.
OR
(b) Calculate the emf of the following cell at 298 K :
Fe(s) | Fe2+ (0.01M) H+(1M) | H2(g) (1 bar), Pt(s)

Given ECell = 0.44 V. 2

24. (a) (i) Draw the zwitter ion structure for sulphanilic acid. 2×1=2
(ii) How can the activating effect of –NH2 group in aniline be
controlled ?
OR
(b) (i) Complete the reaction with the main product formed : 2×1=2

3  
CH CH OH
2

(ii) Convert Bromoethane to Propanamine.

25. Give the reaction of heating glucose with hydroxylamine. Presence of

which group is confirmed by this reaction ? 2

SECTION – C

26. Give reasons for any 3 of the following observations : 3×1=3

(a) Penta-acetate of glucose does not react with hydroxylamine.
(b) Amino acids behave like salts.
(c) Water soluble vitamins must be taken regularly in diet.
(d) The two strands in DNA are complimentary to each other.

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27. (a) On the basis of crystal field theory, write the electronic configuration
for d4 with a strong field ligand for which 0 > P. 1+2=3

(b) A solution of [Ni(H2O)6]2+ is green but a solution of [Ni(CO)4] is

colourless. Explain.

[Atomic number : Ni = 28]

28. (a) (i) Why is the C – O bond length in phenols less than that in methanol ?

3×1=3

(ii) Arrange the following in order of increasing boiling point :

Ethoxyethane, Butanal, Butanol, n-butane

(iii) How can phenol be prepared from anisole ? Give reaction.

OR
(b) (i) Give mechanism of the following reaction : 2+1=3
H2SO4
CH3CH2OH –––––– CH3CH2 – O – CH2CH3 + H2O
413 K
(ii) Illustrate hydroboration – oxidation reaction with an example.

29. (a) Illustrate Sandmeyer’s reaction with an equation. 1+2=3

(b) Explain, why (CH3)2NH is more basic than (CH3)3N in aqueous

solution.

30. (a) For the reaction 1+2=3

2N2O5(g)  4NO2(g) + O2(g) at 318 K

calculate the rate of reaction if rate of disappearance of N2O5(g) is

1.4  10–3 m s–1.

(b) For a first order reaction derive the relationship t99% = 2t90%

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 SECTION – D

The following questions are case-based questions. Read the passage

carefully and answer the questions that follow :

31. Nucleophilic Substitution

Nucleophilic Substitution reaction of haloalkane can be conducted
according to both SN1 and SN2 mechanisms. SN1 is a two step reaction
while SN2 is a single step reaction. For any haloalkane which mechanism
is followed depends on factors such as structure of haloalkane, properties
of leaving group, nucleophilic reagent and solvent.
Influences of solvent polarity : In SN1 reaction, the polarity of the system
increases from the reactant to the transition state, because a polar solvent
has a greater effect on the transition state than the reactant, thereby
reducing activation energy and accelerating the reaction. In SN2 reaction,
the polarity of the system generally does not change from the reactant to
the transition state and only charge dispersion occurs. At this time, polar
solvent has a great stabilizing effect on Nu than the transition state,
thereby increasing activation energy and slow down the reaction rate. For
example, the decomposition rate (SN1) of tertiary chlorobutane at 25 C in
water (dielectric constant 79) is 300000 times faster than in ethanol
(dielectric constant 24). The reaction rate (SN2) of 2-Bromopropane and
NaOH in ethanol containing 40% water is twice slower than in absolute
ethanol. Hence the level of solvent polarity has influence on both SN1 and
SN2 reaction, but with different results. Generally speaking weak polar
solvent is favourable for SN2 reaction, while strong polar solvent is
favourable for SN1. Generally speaking the substitution reaction of
tertiary haloalkane is based on SN1 mechanism in solvents with a strong
polarity (for example ethanol containing water).

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 Answer the following questions :
(a) Why racemisation occurs in SN1 ? 1
(b) Why is ethanol less polar than water ? 1
(c) Which one of the following in each pair is more reactive towards SN2
reaction ?
(i) CH3 – CH2 – I or CH3CH2 – Cl

(ii) Cl or CH2 – Cl 21

OR
(c) Arrange the following in the increasing order of their reactivity
towards SN1 reactions :
(i) 2-Bromo-2-methylbutane, 1-Bromopentane, 2-Bromopentane
(ii) 1-Bromo-3-methylbutane, 2-Bromo-2-methylbutane, 2-Bromo-3-
methylbutane 21

32. Rahul set-up an experiment to find resistance of aqueous KCl solution for
different concentrations at 298 K using a conductivity cell connected to a
Wheatstone bridge. He fed the Wheatstone bridge with a.c. power in the
audio frequency range 550 to 5000 cycles per second. Once the resistance
was calculated from null point he also calculated the conductivity K
and molar conductivity m and recorded his readings in tabular form.
S.No. Conc.(M) k S cm–1  m S cm2 mol–1
1. 1.00 111.3 × 10–3 111.3
2. 0.10 12.9 × 10–3 129.0
3. 0.01 1.41 × 10–3 141.0

Answer the following questions :

(a) Why does conductivity increase though the conductivity decrease
with dilution ? 1
(b) If m of KCl is 150.0 S cm mol , calculate the degree of dissociation
o 2 –1

of 0.01 M KCl. 1
(c) If Rahul had used HCl instead to KCl then would you expect the m
values to be more or less than those per KCl for a given
concentration. Justify. 21
OR
(c) Amit a classmate of Rahul repeated the same experiment with
CH3COOH solution instead of KCl solution. Give one point that
would be similar and one that would be different in his observations
as compared to Rahul. 21

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 SECTION – E
33. (a) (i) Write the reaction involved in Cannizaro’s reaction. 1+1+3=5
(ii) Why are the boiling point of aldehydes and ketones lower than
that of corresponding carboxylic acids ?
(iii) An organic compound ‘A’ with molecular formula C5H8O2 is
reduced to n-pentane with hydrazine followed by heating with
NaOH and Glycol. ‘A’ forms a dioxime with hydroxylamine and
gives a positive Iodoform and Tollen’s test. Identify ‘A’ and give
its reaction for Iodoform and Tollen’s test.
OR
(b) (i) Give a chemical test to distinguish between ethanal acid and
ethanoic acid. 1+1+3=5
(ii) Why is the -hydrogens of aldehydes and ketones are acidic in
nature ?
(iii) An organic compound ‘A’ with molecular formula C4H8O2
undergoes acid hydrolysis to form two compounds ‘B’ and ‘C’.
Oxidation of ‘C’ with acidified potassium permanganate also
produces ‘B’. Sodium salt of ‘B’ on heating with soda lime gives
methane.
(1) Identify ‘A’, ‘B’ and ‘C’.
(2) Out of ‘B’ and ‘C’, which will have higher boiling point ?
Give reason.

34. (a) (i) Why is boiling point of 1M NaCl solution more than that of 1M
glucose solution ? 1+2+2=5
(ii) A non-volatile solute ‘X’ (molar mass = 50 g mol–1) when
dissolved in 78g of benzene reduced its vapour pressure to 90%.
Calculate the mass of X dissolved in the solution.
(iii) Calculate the boiling point elevation for a solution prepared by
adding 10g of MgCl2 to 200g of water assuming MgCl2 is
completely dissociated.
(Kb for Water = 0.512 K kg mol–1, Molar mass MgCl2 = 95g mol–1)
OR

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 (b) (i) Why is the value of Van’t Hoff factor for ethanoic acid in
benzene close to 0.5 ? 1+2+2=5
(ii) Determine the osmotic pressure of a solution prepared by
dissolving 2.32  10–2g of K2SO4 in 2L of solution at 25 C,
assuming that K2SO4 is completely dissociated.
(R = 0.082 L atm K–1 mol–1, Molar mass K2SO4 = 174g mol–1)
(iii) When 25.6g of Sulphur was dissolved in 1000g of benzene, the
freezing point lowered by 0.512 K. Calculate the formula of
Sulphur (Sx).
(Kf for benzene = 5.12 K kg mol–1, Atomic mass of Sulphur = 32g
mol–1)

35. (a) Write the number of unpaired electrons in Cr3+.

(Atomic number of Cr = 24) 1+2+2=5
(b) Complete the reaction mentioning all the products formed :
Cr2O72– + 3H2S + 8H+ 

(c) Account for the following :

(i) Mn2+ is more stable than Fe2+ towards oxidation to +3 state.
(ii)  2+/M value.
Copper has exceptionally positive EM

(iii) Eu2+ with electronic configuration [Xe] 4f76s2 is a strong reducing

agent.

___________________

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