CBSE Class 12 Chemistry Question Paper 2020 Set 56-5-2

Series : HMJ/5 SET – 2
OSS/1GRLH/1  .
Code No. 56/5/2
 .    -  - 
Roll No.   
Candidates must write the Code on
the title page of the answer-book.

 NOTE
(I)       -   (I) Please check that this question
 15   paper contains 15 printed pages.
(II) -         (II) Code number given on the right
   -  -  hand side of the question paper
should be written on the title page
 
of the answer-book by the candidate.
(III)      -  37  (III) Please check that this question
  paper contains 37 questions.
(IV)         (IV) Please write down the Serial
,       Number of the question in the
answer-book before attempting
it.
(V)  -     15   (V) 15 minute time has been allotted
     -    to read this question paper. The
question paper will be distributed
 10.15     10.15  
at 10.15 a.m. From 10.15 a.m. to
10.30     -   10.30 a.m., the students will read
      -  the question paper only and will
     not write any answer on the
answer-book during this period.

  ()
CHEMISTRY (Theory)

{ZYm©[aV g‘¶ : 3 KÊQ>o A{YH$V‘ A§H$ : 70
Time allowed : 3 hours Maximum Marks : 70

.56/5/2. 322B 1 P.T.O.

  

           

(i) -      – , ,    

(ii)  -  37        

(iii) - – - 1  20   -    ,   1 

              

(iv) - – - 21  27  -    ,   2  
 

(v) - – - 28  34  - -1   ,   3 
  

(vi) - – - 35  37  - -2   ,   5 
  

(vii)       , -     , -     

 -                 
    

(viii)  , ,            

(ix)           

.56/5/2. 2

General Instructions :

Read the following instructions very carefully and strictly follow them :

(i) Question paper comprises four sections – A, B, C and D.

(ii) There are 37 questions in the questions paper. All questions are
compulsory.

(iii) Section – A : Q. No. 1 to 20 are very short answer type questions
carrying one mark each. Answer these questions in one word or one
sentence.

(iv) Section – B : Q. No. 21 to 27 are short answer type questions carrying
two marks each.

(v) Section – C : Q. No. 28 to 34 are long answer type-I questions carrying
three marks each.

(vi) Section – D : Q. No. 35 to 37 are long answer type-II questions carrying
five marks each.

(vii) There is NO overall choice in the question paper. However, an internal
choice has been provided in 2 questions of two marks, 2 questions of
three marks and all the 3 questions of five marks. You have to
attempt only one of the choices in such questions.

(viii) However, separate instructions are given with each section and
question, wherever necessary.

(ix) Use of calculators and log tables is NOT permitted.

.56/5/2. 3 P.T.O.

 : 
         1  5    
  -           
        – 1       
              ,
              
              ,
,              ,
       (HX)         
  XX', XX'3, XX'5  XX7        
  

1.           ?

2.            ?

3.   (HF  HI)           

4.         ?

5.    X  X     ?

  6  10     :

6.     OH–   SN1     ?

7.     

8.           ?

9.               

10.            (-)    
     

.56/5/2. 4

SECTION : A
Read the given passage and answer the questions 1 to 5 that follow :
The halogens have the smallest atomic radii in their respective periods.
The atomic radius of fluorine is extremely small. All halogens exhibit – 1
oxidation state. They are strong oxidising agents and have maximum
negative electron gain enthalpy. Among halogens, fluorine shows
anomalous behaviour in many properties. For example electro negativity
and ionisation enthalpy are higher for fluorine than expected whereas
bond dissociation enthalpy, m.p and b.p and electron gain enthalpy are
quite lower than expected. Halogens react with hydrogen to give hydrogen
halides (HX) and combine amongst themselves to form a number of
compounds of the type XX, XX3, XX5 and XX7 called inter-halogens.

1. Why halogens have maximum negative electron gain enthalpy ?

2. Why fluorine shows anomalous behaviour as compared to other halogens ?

3. Arrange the hydrogen halides (HF to HI) in the decreasing order of their
reducing character.

4. Why fluorine is a stronger oxidizing agent than chlorine ?

5. What are the sizes of X and X in the interhalogen compounds ?

Questions 6 to 10 are one word answers :

6. Out of and , which will undergo SN1 reaction faster with
OH– ?

7. Write the IUPAC name of .

8. What type of linkage is present in polysaccharides ?

9. Name an artificial sweetener whose use is limited to cold drinks.

10. Name the polymer which is used for making non-stick utensils.

.56/5/2. 5 P.T.O.

 . 11  15    
11.          
 = 0 – A C
        ?
(a)  = 0  C  A (b)  = 0  C  
(c)  = 0  C  0 (d)  = 0  C  1

12.         
(a)     
(b)     
(c)             
(d)    

13.    X  Y ,      ‘X’       
        ‘X’      
(a) 1 (b) 0
(c) 2 (d) 1/2

14.     AgNO3        ?
(a) K2 [Pt(en)2Cl2] (b) [Co (NH3)3Cl3]
(c) [Cr (H2O)6]Cl3 (d) [Fe (H2O)3Cl3]

15.     
(a) Cu2S, Cu2O   (b) Cu2S, CuO  
(c) Cu2S, FeO   (d) Cu2S, FeS  

 16  20 
(A)  (A)   (R)       (R),  (A)  
  
(B)  (A)   (R)       (R),  (A)  
   
(C)  (A)  ,   (R)    
(D)  (A)  ,   (R)    
16.  (A) :    0.1 M KCl     0.1 M  
    
 (R) :  , KCl          

.56/5/2. 6

Question 11 to 15 are multiple choice questions.
11. Kohlrausch given the following relation for strong electrolytes :
 = 0 – A C
Which of the following equality holds ?
(a)  = 0 as C  A (b)  = 0 as C  
(c)  = 0 as C  0 (d)  = 0 as C  1

12. In an electrochemical process, a salt bridge is used
(a) as a reducing agent.
(b) as an oxidizing agent.
(c) to complete the circuit so that current can flow.
(d) None of these

13. In a chemical reaction X  Y, it is found that the rate of reaction doubles
when the concentration of X is increased four times. The order of the
reaction with respect to X is
(a) 1 (b) 0
(c) 2 (d) 1/2

14. Which of the following will give a white precipitate upon reacting with AgNO3 ?
(a) K2 [Pt(en)2Cl2] (b) [Co (NH3)3Cl3]
(c) [Cr (H2O)6]Cl3 (d) [Fe (H2O)3Cl3]

15. Copper matte contains
(a) Cu2S, Cu2O and silica (b) Cu2S, CuO and silica
(c) Cu2S, FeO and silica (d) Cu2S, FeS and silica

Questions 16 to 20.
(A) Both Assertion (A) and Reason (R) are correct statements, and
Reason (R) is the correct explanation of the Assertion (A).
(B) Both Assertion (A) and Reason (R) are correct statements, but
Reason (R) is not the correct explanation of the Assertion (A).
(C) Assertion (A) is correct, but Reason (R) is wrong statement.
(D) Assertion (A) is wrong, but Reason (R) is correct statement.

16. Assertion (A) : 0.1 M solution of KCl has greater osmotic pressure than
0.1 M solution of glucose at same temperature.
Reason (R) : In solution, KCl dissociates to produce more number of
particles.
.56/5/2. 7 P.T.O.

17.  (A) :          
 (R) :             

18.  (A) :              
 (R) :           
        

19.  (A) :            
 (R) :   C – H       C – C  
  

20.  (A) :           
 (R) :         ,    
   20  1 = 20

 : 
21.     
(a)      NaCN 
(b)     CO   2

            ?      
     2

22.                  
    ? 2

23.     
(i) H2 S2 O 7
(ii) BrF5 2

24.               
 ? 2

               ?  
        ? 2

.56/5/2. 8

17. Assertion (A) : Conductivity of an electrolyte increases with decrease in
concentration.
Reason (R) : Number of ions per unit volume decreases on dilution.

18. Assertion (A) : Ortho and para-nitrophenols can be separated by steam
distillation.
Reason (R) : Ortho isomer associates through intermolecular
hydrogen bonding while Para isomer associates through
intramolecular hydrogen bonding.

19. Assertion (A) : Oxidation of ketones is easier than aldehydes.
Reason (R) : C-C bond of ketones is stronger than C-H bond of
aldehydes.

20. Assertion (A) : Low spin tetrahedral complexes are rarely observed.
Reason (R) : Crystal field splitting energy is less than pairing energy
for tetrahedral complexes. 20  1 = 20

SECTION : B
21. Write the role of
(a) Dilute NaCN in the extraction of Gold.
(b) CO in the extraction of Iron. 2
OR
How is leaching carried out in the case of low grade copper ores ? Name
the method used for refining of copper metal. 2

22. State Raoult’s law for a solution containing volatile components. What is
the similarity between Raoult’s law and Henry’s law ? 2

23. Draw the structures of the following :
(i) H2S2O7
(ii) BrF5 2

24. Define adsorption with an example. What is the role of adsorption in
heterogeneous catalysis ? 2
OR
Define Brownian movement. What is the cause of Brownian movement in
colloidal particles ? How is it responsible for the stability of Colloidal Sol ? 2
.56/5/2. 9 P.T.O.

25.       

(i)

(ii) 2

26.           2

27. ,        ?         
         2

 : 
28.   A, B, C, D, E  F   

6½=3

29. AlCl3  0.01 m   – 0.068 C       
   [      Kf = 1.86 K kg mol–1] 3

30.            
(a)  
(b)   
(c)    1+1+1=3

31.       A  B  ZnSO4  CuSO4 
 ,  2A        B    2g Cu   
       ?  A    Zn      ?
[   Cu = 63.5 g mol–1, Zn = 65 g mol–1; 1F = 96500 C mol–1] 3

32.           3

     
(i)   (ii)   (iii)  1 + 1 + 1 = 3
.56/5/2. 10

25. Identify the monomers in the following polymers :

(i)

(ii) 2

26. Discuss the nature of bonding in metal carbonyls. 2

27. How do antiseptics differ from disinfectants ? Name a substance which
can be used as a disinfectant as well as an antiseptic. 2

SECTION : C
28. Identify A, B, C, D, E and F in the following :

6½=3

29. A 0.01 m aqueous solution of AlCl3 freezes at – 0.068 C. Calculate the
percentage of dissociation. [Given : Kf for Water = 1.86 K kg mol–1] 3

30. Define the following terms with a suitable example in each :
(a) Polysaccharides (b) Denatured protein (c) Fibrous protein
1+1+1=3

31. When a steady current of 2A was passed through two electrolytic cells A
and B containing electrolytes ZnSO4 and CuSO4 connected in series, 2 g of
Cu were deposited at the cathode of cell B. How long did the current flow ?
What mass of Zn was deposited at cathode of cell A ?
[Atomic mass : Cu = 63.5 g mol–1, Zn = 65 g mol–1; 1F = 96500 C mol–1] 3

32. Write three differences between lyophobic sol and lyophilic sol. 3
OR
Define the following terms :
(i) Protective colloid (ii) Zeta potential (iii) Emulsifying agent
1+1+1=3
.56/5/2. 11 P.T.O.

33.          
(i)        H2O2   
(ii) 358 K  20% H3PO4       (CH3)3C–OH   

(iii) HI        31=3

      ?
(i)   o- 
(ii)    
(iii)     31=3

34.   
(i)  -    
(ii)                
(iii)            31=3

 : 
35. (a)       25%    40        
       80%   ?
(b)             
         3+2=5

(a)       50%    300 K  30     320
K  10        (Ea)   
(R = 8.314 J K–1 mol–1)
(b)           
(c)                ?
[   log 2 = 0.3010, log 3 = 0.4771, log 4 = 0.6021, log 5 = 0.6991]
3+1+1=5
36. (a)   
(i)          
(ii)          
(iii) Zn, Cd  Hg        
(b)     
(i) Na2CrO4  Na2Cr2O7
(ii) MnO2  K2MnO4 3+2=5

.56/5/2. 12

33. Give the structures of final products expected from the following reactions :
(i) Hydroboration of propene followed by oxidation with H2O2 in
alkaline medium.
(ii) Dehydration of (CH3)3C–OH by heating it with 20% H3PO4 at 358 K.
(iii) Heating of with HI. 31=3
OR
How can you convert the following ?
(i) Phenol to o-hydroxy benzaldehyde.
(ii) Methanal to ethanol
(iii) Phenol to phenyl ethanoate. 31=3
34. Give reasons :
(i) Aniline does not undergo Friedal-Crafts reaction.
(ii) Aromatic primary amines cannot be prepared by Gabriel’s
phthalimide synthesis.
(iii) Aliphatic amines are stronger bases than ammonia. 31=3

SECTION : D
35. (a) A first order reaction is 25% complete in 40 minutes. Calculate the value
of rate constant. In what time will the reaction be 80% completed ?
(b) Define order of reaction. Write the condition under which a
bimolecular reaction follows first order kinetics. 32=5
OR
(a) A first order reaction is 50% complete in 30 minutes at 300 K and in 10
minutes at 320 K. Calculate activation energy (Ea) for the reaction.
(R = 8.314 J K–1 mol–1)
(b) Write the two conditions for collisions to be effective collisions.
(c) How order of reaction and molecularity differ towards a complex
reaction ?
[Given : log 2 = 0.3010, log 3 = 0.4771, log 4 = 0.6021, log 5 = 0.6991]
3+1+1=5
36. (a) Give reasons :
(i) Transition metals and their compounds show catalytic activities.
(ii) Separation of a mixture of Lanthanoid elements is difficult.
(iii) Zn, Cd and Hg are soft and have low melting point.
(b) Write the preparation of the following :
(i) Na2Cr2O7 from Na2CrO4
(ii) K2MnO4 from MnO2 3+2=5
OR

.56/5/2. 13 P.T.O.

(a)      
(i)    Ti3+    Sc3+   
(ii) Cr2+     
(b)           
(c)      
2
3 MnO4 + 4H+  2+2+1=5

37. (a)             
 
(i)  NaOH    CH3CHO

(ii) H2N – NH

 NaOH
(iii)
(b)      
(i) CH3 – CH = CH – CO – CH3  CH3 – CH2 – CO – CH = CH2
(ii)    3 + (1 + 1) = 5

(a)       
CH3
Zn/Hg
(i) C = O 
 HCl
CH3
NaOH/CaO
(ii) 

(a) DIBAL-H
(iii) CH2 = CH – CH2 – CN 
(b) H3O+
(b)            
   
CH3COCH3, HCHO, CH3CHO,

(c)   2, 4 – ...      3+1+1=5
___________

.56/5/2. 14

(a) Account for the following :
(i) Ti3+ is coloured whereas Sc3+ is colourless in aqueous solution.
(ii) Cr2+ is a strong reducing agent.
(b) Write two similarities between chemistry of lanthanoids and
actinoids.
(c) Complete the following ionic equation :
2
3 MnO4 + 4H+  2+2+1=5

37. (a) Write the products formed when benzaldehyde reacts with the
following reagents :
(i) CH3CHO in presence of dilute NaOH

(ii) H2N – NH

(iii) Conc. NaOH
(b) Distinguish between following :
(i) CH3 – CH = CH – CO – CH3 and CH3 – CH2 – CO – CH = CH2
(ii) Benzaldehyde and Benzoic acid. 3 + (1 + 1) = 5
OR
(a) Write the final products in the following :
CH3
Zn/Hg
(i) C = O 
Conc HCl
CH3
NaOH/CaO
(ii) 

(a) DIBAL-H
(iii) CH2 = CH – CH2 – CN 
(b) H3O+
(b) Arrange the following in the increasing order of their reactivity
towards nucleophilic addition reaction :
CH3COCH3, HCHO, CH3CHO,

(c) Draw the structure of 2, 4 DNP derivative of acetaldehyde. 3+1+1=5
___________

.56/5/2. 15 P.T.O.

.56/5/2. 16