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Asked by  | 19th Mar, 2013, 07:35: PM

Expert Answer:

Sample Paper- 2013

MM: 70                                                                                     Time:3.00 Hr.

 

1.         State the relationship between :                                                                                  1

(i) Empirical and molecular formula.  

(ii) Molecular wt. and vapour density.                                                                                   

2.         Write IUPAC name for;                          CH3COOCH3                                                                   1

 

            

                                           

 

3.         Which one of the following atomic orbitals is not possible ? Why ?                          1

            (i) n = 3, l = 1, m = –2             (ii) n = 4, l = 0, m = 0

4.         What is the significance of van der Waal's constant 'b' ?                                           1

5.         What is inductive effect ?.                                                                                          1

6.         State why heat changes in chemical processes are indicated as enthalpy changes and not internal energy changes ?                                                                                                1

7.         What is the condition required for the precipitation to occur ?                                  1

8.         Give an example of a b–elimination reaction.                                                            1

9.         A compound contains 4.07 % hydrogen, 24.27 % carbon and 71.65 % chlorine. It's molar mass is 98.96 g . Deduce  the empirical and molecular formulae.                                    2

            [ At. masses : H = 1 ; O = 16 ; Cl = 35.5 ]

10.       How would you separate a mixture of ethylene, acetylene and ethane ?                   2

11.       Explain the significance of the terms ‘isolated gaseous atom’  and  ‘ground state’ while     defining ionization enthalpy and electron gain enthalpy.                                      2

12.       State why :                                                                                                                  2

            (a) In any period, the alkali metal has lowest ionization energy.

            (b) van der Waals' radii are always larger than covalent radii.

13.       (a) Write an expression to calculate angular momentum of an electron ?

            (b) State the significance of minus sign in Bohr's equation.                                       2

OR

(a) Which quantum number does not follow from the solution of Schrodinger wave                                                             

      equation ?

            (b) An electron has s = + ½ and m = -1, it cannot be present in which of the orbitals and                      why ?

14.       Differentiate between primary and secondary pollutants.                                         2

15.       The following system is in equilibrium ;                                                                     2

                       

                        SO2Cl2 + Heat    ----->              SO2 + Cl2

 

            What will happen to the temperature of the system if some Cl2 into it at constant volume ?            Give reason.

16.       Write the conformations of ethane and compare their stability.                                 2

17.       Account for the following :                                                                                        2

            (a) Alkali metals are used in photoelectric cells.

            (b) There is a very large difference between first and second ionization energies of alkali

      metals.

18.       Explain why :                                                                                                              2

            (i) B––X bond length in BX3 is shorter than theoretically expected values.

            (ii) BCl3 has a higher stability than TlCl3.

19.       Write down chemical equations (only) corresponding to the following :                  3

            (i) Friedel-Craft's reaction

            (ii) Wurtz reaction

            (iii) Baeyer's test

20.       Why is benzene extra ordinarily stable although it contains three double bonds ?    3

21.       What are electrophiles and nucleophiles ? How are the produced during bond

fission ?                                                                                                                       3

22.       (a) Define wave number.                                                                                            3         

            (b) Calculate the uncertainty in the velocity of a wagon of mass 3000 kg whose                                   position is known to an accuracy of ± 10 pm [ Planck's constant = 6.63 × 10-34 Js ]               

23.       (i) State one application of Dalton's law.                                                               3

            (ii) A gaseous mixture contains 56 g of N2, 44 g of CO2 and 16 g of CH4. The total                              pressure of the mixture is 720 mm Hg. What is the partial pressure of CH4 ?           

24.       (i) Derive the relationship :  Kp ? Kc (RT)?n . Symbols having usual sense.              3

            (ii) Name the conjugate acids of the following species :

                 (a) CO32-                 (b) OH-

25.       (a) In terms of oxidation number, What is an oxidizing agent ?                                3

(b) Balance  the following equation in acidic medium by half equation method :    

                        Sn(s) + NO3-(aq) + H+(aq)  ?   Sn2+(aq) + NH4+(aq) + H2O(l)

26.       State what are :                                                                                                           3

(a)   Isotope effect.                   (b) Anion Exchange resins.                                                    

(c)  Hydride gap.

27.       (a) What is diagonal relationship?                                                                              3

            (b) Alkali and alkaline earth metals cannot be obtained by chemical reduction method.                       Comment.

            (c) Write chemical equation showing the conversion of gypsum to P.O.P.

OR

(a) Li shows similarities to which element of periodic table ? What this phenomenon is

     called ?

            (b) Write the chemical equation corresponding to the slaking of lime.                                  (c) Why an aqueous solution of Na2CO3 is alkaline ?

28.       (a) Account for the following :                                                                                   5

                 (i) Bond length follows the order : C—C > C?C > C?C for di carbon species .

                 (ii) pi-bond is always formed in association with sigma-bond.

            (b) Use MOT to explain why N2+ is less stable than N2 and O2+ is more stable than O2.

OR

            (a) Account for the following :                                                                      

                 (i) Free rotation around a ?-bond is not possible. 

                 (ii) Predict the type of hybridization and shape of IF7 molecule.

            (b) In terms of MOT, taking a suitable example explain why noble gases do not

      exist as diatomic species.   

29.       (a) Derive qp =  qv + ?ngRT, symbols having usual sense.                                          5

            (b) Calculate the enthalpy change accompanying the transformation of C (graphite) to                         C (diamond). Given that the enthalpies of combustion of graphite and diamond are

                  393.5 and 395.4  KJ mol-1 respectively.

            (c) Define Gibb's free energy.

OR

            (a) Derive the expression Cp - Cv = R. Symbols having usual meaning.                  

            (b) Calculate ?Hf  of ethene (C2H4) from the following data :                                                          (i) C(s) + O2(g)  ?  CO2(g) ; ?H = – 396 KJ

                        (ii) H2(g) +  ½ O2(g)  ?  H2O(l) ; ?H = – 287 KJ

                        (iii) C2H4(g) + 3O2(g) ?  2CO2(g) + 2H2O(l) ; ?H = –1400 KJ

            (c) State Hess's Law.

30.       (a) With the help of relevant chemical equations, state what is borax bead test ? What                         type of cations are tested by this test ?                                                                                   (b) Comment :                                                                                                             5                           (i) ) PbCl2 is ionic but PbCl4 is covalent.

                 (ii) No form of elemental silicon is comparable to graphite ?

OR

            (a) State what are :                                                                                                     

                 (i) Inorganic benzene

                 (ii) Fullerenes

            (b) Account for the following :

                 (i) CCl4 is not hydrolyzed by water but SiCl4 is easily hydrolyzed.

                 (ii) SnCl2 is ionic whereas SnCl4 is covalent.

                 (iii) BF3 is less acidic than BCl3 although flourine is more electronegative than

                        chlorine?

 

 

 

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Answered by  | 20th Mar, 2013, 06:03: AM

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