1.
1.100 mL solution of NaOH (containing 4.0 g NaOH per litre) and 50 mL of HCI (containing 7.3
g HCI per litre) react as NaOH (aq)+ HCI(aq)—> NaCI(aq)+ H2O(/) Thus, NaCl formed is
(a) 0.585 g (c) 0.1170 g (b) 0.0293 g (d) 0.0365 g
2.Using the data given below to find out the strongest reducing agent.
EᶱCr2O7
2-
/Cr3+
= 1.33V
EᶱMnO4
–
/Mn2+
= 1.51V
EᶱCl2/Cl–
= 1.36V
EᶱCr3+
/Cr = -0.74V
(a) Cl–
(b) Cr
(c) Cr3+
(d)Mn+2
3. Which of the following statements is not correct about an order of a reaction.
(a) The order of a reaction can be a fractional number.
(b) Order of a reaction is experimentally determined quantity.
(c) The order of a reaction is always equal to the sum of the stoichiometric
coefficients of reactants in the balanced chemical equation for a reaction.
(d) The order of a reaction is the sum of the powers of the molar concentration
of the reactants in the rate law expression.
4.A first-order reaction is 50% completed in 1.26 × 1014 s. How much time
would it take for 100% completion?
(a) 1.26 × 1015
s
(b) 2.52 × 1014
s
(c) 2.52 × 1028
s
(d) infinite
5.A chelating agent has two or more than two donor atoms to bind to a single
metal ion. Which of the following is not a chelating agent?
(a) thiosulphate
(b) oxalate
(c) glycinato
(d) ethane-1,2-diamine

2.
6. Reaction of C6H5CH2Br with aqueous sodium hydroxide follows ____________.
(a) SN1 mechanism
(b) SN2 mechanism
(c) Any of the above two depending upon the temperature of the reaction
(d) Saytzeff rule
7.Which of the following compounds will react with sodium hydroxide solution in water?
(a) C6H5OH
(b) C6H5CH2OH
(c) (CH3)3 COH
(d)CH3CH2OH
8.Which of the following ores are concentrated by froth flotation?
(a) Haematite
(b) limonite
(c) Copper pyrites
(d) MagnetiteSolution:
9.For oxidation of iron at 298 K, 4Fe(s)+ 3O2(g)----- > 2Fe2O3(s) ∆S0
= - 549.4 J K'1 mol-1 and
∆H° = - 1648.0 kJ mol-1
Select the correct alternate
(a) This reaction is spontaneous
(b) ∆S°(surrounding) > 0
(c) ∆S° total]) > 0
(d) All of the above are correct statements
10.What is heat of neutralization on mixing 100 mL of 1 M Ca(OH)2 and 100 mL of 1M H2SO4
(consider electrolytes as strong)?
a)-57.3 KJ b)+57.3KJ c)-11.46KJ d)+11.46 KJ
11.For the following gaseous phase reaction at 298 K F2+ 2HCI----- > 2HF+ Cl2, AH° = - 84.4
kcal If ∆Hf
0
(HF) = - 64.2 kcal mol"1 then ∆Hf°(HCI) is
(a) 20.2 kcal mol-1 (b) - 22.0 kcal mol-1 c) - 20.2 kcal mol-1 d) +22.0 kcal mo-1
Group B
12Calculate the enthalpy of formation of gaseous 3-methyl-1-butene from the following data
using the following data using Hess law.

3.
What is bond enthalpy?
or
Study the following reactions carried out at 25O
C.
ClNO2 (g) + NO (g) → NO2 (g) + ClNO (g)
a) Calculate the ∆S° Given(standard molar entropy for ClNO2 (g) is 272.23 J/mol•K;
entropy for NO (g) is 210.8 J/mol•K; entropy for NO2 (g) is 240.1 J/mol•K; entropy
for ClNO (g) is 261.58 J/mol•K. )[1]
b) Calculate the ∆H° (∆Hf for ClNO2 (g) is 12.5 kJ/mol; ∆Hf for NO (g) is 90.25
kJ/mol; ∆Hf for NO2 (g) is 33.18 kJ/mol; ∆Hf for ClNO (g) is 51.71 kJ/mol.)
c) Calculate ∆G°[1]
d) Predict if the process is spontaneous or not.[1]
e) What is enthalpy change of formation?
13.Iodide ion is oxidized in acidic solution to triiodide ion by H2O2.as
H2O2 + 3I- + 2H+----- > I3
- + 2H2O Given,
a)Write the rate law[1]
b)Determine the overall order of reaction[1]
c)How many times the rate of reaction changes when the concentration of each reactant is
doubled?[1]
d)Write two differences between molecularity and order of reaction.[2]
14.Write example of the following reaction[5]
a)Willamsons etherififcation
b)Oxoprocess
c)Dows reaction
d)Coupling reaction
e)Kolbes reaction
15. Given Hg2Cl2+2e-
→2Hg+Cl-
E0
=0.280V(1MKCl) and Ag(s)→Ag+
(aq)+e-
E0
=0.80V[5]
a)Construct a galvanic cell.[1]
bWrite the cell notation [1]

4.
c)Calculate the standard cell potential.[1]
d)Write the cell reaction at cathode or anode[1]
e) Calculate the Gibbs free energy change[1]
16. In the acid-base titration the standard Na2CO3 was titrated against HCl.[5]
a)What are primary and secondary standards?
b)Write the principle of Volumetric analysis.
c)Are the equivalence point and end point the same?
d)The titration of Na2CO3 with HCl, methyl orange is used as an indicator. Why?
e)What amount of standard Na2CO3 is required to prepare 0.1molar solution of 250 ml?
17. Is ( NH-CHR-CO ) n , a homopolymer or copolymer?why?[5]
a)Define thermoplastics and thermosetting polymers with one examples of each.[1]
b)What is azo-dye??write example[1]
c)Write the reaction of formation of formaldehyde-phenol resin ?[2]
d)What is antipyretic drug and analgesic drug?write example[1]
18. How can you separate RNH2 R2NH and R3N by Hoffmann separation method
19. Write the sequence of reaction to convert from one form to another form.
C6H5N2Cl C6H6O C6H7N C6H5NO2 C6H6
Group C.
20. a)An organic halide A C5H11Br on treatment with aq. NaOH gives a compound B C5H12O,On
oxidation Compound B gives Ketone C. Oxidation of C under drastic condition gives a mixture
of ethanoic acid and propanoic acid. What are A,B and C. Give reaction also.[4]
b) Why is phenol more acidic than aliphatic alcohol?[2]
c)Convert 1- propanol to 2- propanol and vice versa[2]
Or
a)Write down the laboratory method of preparation of chloroform from ethanol.[2]
b)Write down the laboratory method of preparation of diethyl ether from ethanol.[2]
c)Write down the two distinguishing reactions given by ethanol and phenol.[2]
d)Arrange water, ethanol and phenol in increasing order of acidity and give a reason for your answer.[2]
21.a) An aromatic compound A on reduction yields parent hydrocarbon B.B on nitration gives C. C on acidic
reduction gives D.D on coupling with diazonium salt gives diazoaminobenze.[4]
Identify A,B C and Write the reaction involved.
b) Why does nitrobenzene undergo electrophilic substitution reaction at meta position?[2]
c)Why is nucleophilic substitution reaction difficult in haloarene?[2]

5.
22.a)100 mL of 0.1 M KOH is mixed with 200 mL of 0.1 M Ca(OH)2. and 300 mL of 0.1 M
H2SO4. What is the normality of the resultant mixture?[3]
b) A reaction is of second order with respect to a reactant. How will the rate of reaction be
affected if the concentration of this reactant (i) doubled, (ii) reduced to half?[3]
c) Derive the integrated rate law for first order reaction and its half life period[3]