Previous Year Question Paper: Chemistry, 2010 (with answer key), Class 12 Class 12 Notes | EduRev

Class 12 : Previous Year Question Paper: Chemistry, 2010 (with answer key), Class 12 Class 12 Notes | EduRev

 Page 1


174
CHEMISTRY (Theory)
Time allowed : 3 hours Maximum Marks : 70
General Instructions:
(i) All questions are compulsory.
(ii) Marks for each question are indicated against it.
(iii) Question numbers 1 to 8 are very short-answer questions and carry 1 mark
each.
(iv) Question numbers 9 to 18 are short-answer questions and carry 2 marks
each.
(v) Question numbers 19 to 27 are also short-answer questions and carry 3 marks
each.
(vi) Question numbers 28 to 30 are long-answer questions and carry 5 marks each.
(vii) Use Log Tables, if necessary, Use of calculators is not allowed.
QUESTION PAPER CODE 56/1/1
1. Write a feature which will distinguish a metallic solid from an ionic solid. 1
2. Define ‘order of a reaction’. 1
3. What is an emulsion? 1
4. Why does NO
2
 dimerise ? 1
5. Give an example of linkage isomerism. 1
6. A solution of KOH hydrolyses CH
3
CHClCH
2
CH
3
 and CH
3
CH
2
CH
2
CH
2
Cl.
Which one of these is more easily hydrolysed? 1
7. Draw the structural formula of I-phenylpropan-l-one molecule. 1
8. Give the IUPAC name of H
2
N – CH
2
 – CH
2
 - CH = CH
2
.1
Page 2


174
CHEMISTRY (Theory)
Time allowed : 3 hours Maximum Marks : 70
General Instructions:
(i) All questions are compulsory.
(ii) Marks for each question are indicated against it.
(iii) Question numbers 1 to 8 are very short-answer questions and carry 1 mark
each.
(iv) Question numbers 9 to 18 are short-answer questions and carry 2 marks
each.
(v) Question numbers 19 to 27 are also short-answer questions and carry 3 marks
each.
(vi) Question numbers 28 to 30 are long-answer questions and carry 5 marks each.
(vii) Use Log Tables, if necessary, Use of calculators is not allowed.
QUESTION PAPER CODE 56/1/1
1. Write a feature which will distinguish a metallic solid from an ionic solid. 1
2. Define ‘order of a reaction’. 1
3. What is an emulsion? 1
4. Why does NO
2
 dimerise ? 1
5. Give an example of linkage isomerism. 1
6. A solution of KOH hydrolyses CH
3
CHClCH
2
CH
3
 and CH
3
CH
2
CH
2
CH
2
Cl.
Which one of these is more easily hydrolysed? 1
7. Draw the structural formula of I-phenylpropan-l-one molecule. 1
8. Give the IUPAC name of H
2
N – CH
2
 – CH
2
 - CH = CH
2
.1
175
9. Non-ideal solutions exhibit either positive or negative deviations from Raoult’s law.
What are these deviations and why are they caused? Explain with one example for
each type. 2
10. A reaction is of first order in reactant A and of second order in reactant B. How is
the rate of this reaction affected when (i) the concentration of B alone is increased to
three times (ii) the concentrations of A as well as B are doubled? 2
11. The rate constant for a reaction of zero order in A is 0.0030 mol L 
–1
 s
–1
. How long
will it take for the initial concentration of A to fall from 0.10 M to 0.075 M ? 2
12. Draw the structures of white phosphorus and red phosphorus. Which one of these
two types of phosphorus is more reactive and why? 2
13. Explain the following observations:
(i) Generally there is an increase in density of elements from titanium (Z = 22) to
copper (Z = 29) in the first series of transition elements.
(ii) Transition elements and their compounds are generally found to be good
catalysts in chemical reactions. 2
14. Name the following coordination compounds according to IUP AC system of nom-
enclature:
(i) [Co(NH
3
)
4
 (H
2
O)Cl]Cl
2
(ii) [CrCl
2
(en)
2
]Cl, (en = ethane – 1, 2 – diamine) 2
15. Illustrate the following reactions giving a chemical equation for each:
(i) Kolbe’s reaction,
(ii) W illiamson synthesis. 2
16. How are the following conversions carried out?
(i) Benzyl chloride to benzyl alcohol,
(ii) Methyl magnesium bromide to 2-methylpropan-2-ol. 2
Page 3


174
CHEMISTRY (Theory)
Time allowed : 3 hours Maximum Marks : 70
General Instructions:
(i) All questions are compulsory.
(ii) Marks for each question are indicated against it.
(iii) Question numbers 1 to 8 are very short-answer questions and carry 1 mark
each.
(iv) Question numbers 9 to 18 are short-answer questions and carry 2 marks
each.
(v) Question numbers 19 to 27 are also short-answer questions and carry 3 marks
each.
(vi) Question numbers 28 to 30 are long-answer questions and carry 5 marks each.
(vii) Use Log Tables, if necessary, Use of calculators is not allowed.
QUESTION PAPER CODE 56/1/1
1. Write a feature which will distinguish a metallic solid from an ionic solid. 1
2. Define ‘order of a reaction’. 1
3. What is an emulsion? 1
4. Why does NO
2
 dimerise ? 1
5. Give an example of linkage isomerism. 1
6. A solution of KOH hydrolyses CH
3
CHClCH
2
CH
3
 and CH
3
CH
2
CH
2
CH
2
Cl.
Which one of these is more easily hydrolysed? 1
7. Draw the structural formula of I-phenylpropan-l-one molecule. 1
8. Give the IUPAC name of H
2
N – CH
2
 – CH
2
 - CH = CH
2
.1
175
9. Non-ideal solutions exhibit either positive or negative deviations from Raoult’s law.
What are these deviations and why are they caused? Explain with one example for
each type. 2
10. A reaction is of first order in reactant A and of second order in reactant B. How is
the rate of this reaction affected when (i) the concentration of B alone is increased to
three times (ii) the concentrations of A as well as B are doubled? 2
11. The rate constant for a reaction of zero order in A is 0.0030 mol L 
–1
 s
–1
. How long
will it take for the initial concentration of A to fall from 0.10 M to 0.075 M ? 2
12. Draw the structures of white phosphorus and red phosphorus. Which one of these
two types of phosphorus is more reactive and why? 2
13. Explain the following observations:
(i) Generally there is an increase in density of elements from titanium (Z = 22) to
copper (Z = 29) in the first series of transition elements.
(ii) Transition elements and their compounds are generally found to be good
catalysts in chemical reactions. 2
14. Name the following coordination compounds according to IUP AC system of nom-
enclature:
(i) [Co(NH
3
)
4
 (H
2
O)Cl]Cl
2
(ii) [CrCl
2
(en)
2
]Cl, (en = ethane – 1, 2 – diamine) 2
15. Illustrate the following reactions giving a chemical equation for each:
(i) Kolbe’s reaction,
(ii) W illiamson synthesis. 2
16. How are the following conversions carried out?
(i) Benzyl chloride to benzyl alcohol,
(ii) Methyl magnesium bromide to 2-methylpropan-2-ol. 2
176
17. Explain the following terms. :
(i) Invert sugar
(ii) Polypeptides
OR
Name the products of hydrolysis of sucrose. Why is sucrose not a reducing sugar? 2
18. What are essential and non-essential amino acids in human food? Give one example
of each type. 2
19. The well known mineral fluorite is chemically calcium fluoride. It is known that in
one unit cell of this mineral there are 4 Ca
2+
 ions and 8 F
–
 ions and that Ca
2+
 ions are
arranged in a fcc lattice. The F
–
 ions fill all the tetrahedral holes in the face centred
cubic lattice of Ca
2+
 ions. The edge of the unit cell is 5.46x10
–8
 cm in length. The
density of the solid is 3.18 g cm
–3
. Use this information to calculate Avogadro’s
number (Molar mass of CaF
2
 = 78.08 g mol
–1
)3
20. A solution prepared by dissolving 1.25 g of oil of winter green (methyl salicylate) in
99.0 g of benzene has a boiling point of 80.31 °C. Determine the molar mass of this
compound. (B.P . of pure benzene = 80.10 °C and K
b
 for benzene = 2.53 °C kg
mol
–1
) 3
21. What is the difference between multi molecular and macromolecular colloids? Give
one example of each type. How are associated colloids different from these two
types of col1oids ? 3
22. Describe how the following changes are brought about:
(i) Pig iron into steel.
(ii) Zinc oxide into metallic zinc.
(iii) Impure titanium into pure titanium. 3
OR
Describe the role of
(i) NaCN in the extraction of gold from gold are.
Page 4


174
CHEMISTRY (Theory)
Time allowed : 3 hours Maximum Marks : 70
General Instructions:
(i) All questions are compulsory.
(ii) Marks for each question are indicated against it.
(iii) Question numbers 1 to 8 are very short-answer questions and carry 1 mark
each.
(iv) Question numbers 9 to 18 are short-answer questions and carry 2 marks
each.
(v) Question numbers 19 to 27 are also short-answer questions and carry 3 marks
each.
(vi) Question numbers 28 to 30 are long-answer questions and carry 5 marks each.
(vii) Use Log Tables, if necessary, Use of calculators is not allowed.
QUESTION PAPER CODE 56/1/1
1. Write a feature which will distinguish a metallic solid from an ionic solid. 1
2. Define ‘order of a reaction’. 1
3. What is an emulsion? 1
4. Why does NO
2
 dimerise ? 1
5. Give an example of linkage isomerism. 1
6. A solution of KOH hydrolyses CH
3
CHClCH
2
CH
3
 and CH
3
CH
2
CH
2
CH
2
Cl.
Which one of these is more easily hydrolysed? 1
7. Draw the structural formula of I-phenylpropan-l-one molecule. 1
8. Give the IUPAC name of H
2
N – CH
2
 – CH
2
 - CH = CH
2
.1
175
9. Non-ideal solutions exhibit either positive or negative deviations from Raoult’s law.
What are these deviations and why are they caused? Explain with one example for
each type. 2
10. A reaction is of first order in reactant A and of second order in reactant B. How is
the rate of this reaction affected when (i) the concentration of B alone is increased to
three times (ii) the concentrations of A as well as B are doubled? 2
11. The rate constant for a reaction of zero order in A is 0.0030 mol L 
–1
 s
–1
. How long
will it take for the initial concentration of A to fall from 0.10 M to 0.075 M ? 2
12. Draw the structures of white phosphorus and red phosphorus. Which one of these
two types of phosphorus is more reactive and why? 2
13. Explain the following observations:
(i) Generally there is an increase in density of elements from titanium (Z = 22) to
copper (Z = 29) in the first series of transition elements.
(ii) Transition elements and their compounds are generally found to be good
catalysts in chemical reactions. 2
14. Name the following coordination compounds according to IUP AC system of nom-
enclature:
(i) [Co(NH
3
)
4
 (H
2
O)Cl]Cl
2
(ii) [CrCl
2
(en)
2
]Cl, (en = ethane – 1, 2 – diamine) 2
15. Illustrate the following reactions giving a chemical equation for each:
(i) Kolbe’s reaction,
(ii) W illiamson synthesis. 2
16. How are the following conversions carried out?
(i) Benzyl chloride to benzyl alcohol,
(ii) Methyl magnesium bromide to 2-methylpropan-2-ol. 2
176
17. Explain the following terms. :
(i) Invert sugar
(ii) Polypeptides
OR
Name the products of hydrolysis of sucrose. Why is sucrose not a reducing sugar? 2
18. What are essential and non-essential amino acids in human food? Give one example
of each type. 2
19. The well known mineral fluorite is chemically calcium fluoride. It is known that in
one unit cell of this mineral there are 4 Ca
2+
 ions and 8 F
–
 ions and that Ca
2+
 ions are
arranged in a fcc lattice. The F
–
 ions fill all the tetrahedral holes in the face centred
cubic lattice of Ca
2+
 ions. The edge of the unit cell is 5.46x10
–8
 cm in length. The
density of the solid is 3.18 g cm
–3
. Use this information to calculate Avogadro’s
number (Molar mass of CaF
2
 = 78.08 g mol
–1
)3
20. A solution prepared by dissolving 1.25 g of oil of winter green (methyl salicylate) in
99.0 g of benzene has a boiling point of 80.31 °C. Determine the molar mass of this
compound. (B.P . of pure benzene = 80.10 °C and K
b
 for benzene = 2.53 °C kg
mol
–1
) 3
21. What is the difference between multi molecular and macromolecular colloids? Give
one example of each type. How are associated colloids different from these two
types of col1oids ? 3
22. Describe how the following changes are brought about:
(i) Pig iron into steel.
(ii) Zinc oxide into metallic zinc.
(iii) Impure titanium into pure titanium. 3
OR
Describe the role of
(i) NaCN in the extraction of gold from gold are.
177
(ii) SiO
2
 in the extraction of copper from copper matte.
(iii) Iodine in the refining of zirconium.
Write chemical equations for the involved reactions.
23. How would you account for the following?
(i) The atomic radii of the metals of the third (5d) series of transition elements are
virtually the same as those of the corresponding members of the second (4d)
series.
(ii) The E
o
 value for the Mn
3+
/Mn
2+
 couple is much more positive than that for
Cr
3+
/Cr
2+
 couple or Fe
3+
/Fe
2+
 couple.
(iii) The highest oxidation state of a metal is exhibited in its oxide or fluoride. 3
24. (i) State one use each of DDT and iodoform.
(ii) Which compound in the following couples will react faster in S
N
2
 displacement
and why?
(a) 1-Bromopentane or 2-bromopentane
(b) 1-Bromo-2-methylbutane or 2-bromo-2-methylbutane. 3
25. In the following cases rearrange the compounds as directed:
(i) In an increasing order of basic strength:
C
6
H
5
NH
2
, C
6
H
5
N(CH
3
)
2
, (C
2
H
5
)
6
NH and CH
3
NH
2
(ii) In a decreasing order of basic strength:
Aniline, p-nitroaniline and p-toluidine
(iii) In an increasing order of pK
b
 values:
C
2
H
5
NH
2
, C
6
H
5
 NHCH
3
, (C
2
H
5
)
2
NH and C
6
H
5
NH
2
3
Page 5


174
CHEMISTRY (Theory)
Time allowed : 3 hours Maximum Marks : 70
General Instructions:
(i) All questions are compulsory.
(ii) Marks for each question are indicated against it.
(iii) Question numbers 1 to 8 are very short-answer questions and carry 1 mark
each.
(iv) Question numbers 9 to 18 are short-answer questions and carry 2 marks
each.
(v) Question numbers 19 to 27 are also short-answer questions and carry 3 marks
each.
(vi) Question numbers 28 to 30 are long-answer questions and carry 5 marks each.
(vii) Use Log Tables, if necessary, Use of calculators is not allowed.
QUESTION PAPER CODE 56/1/1
1. Write a feature which will distinguish a metallic solid from an ionic solid. 1
2. Define ‘order of a reaction’. 1
3. What is an emulsion? 1
4. Why does NO
2
 dimerise ? 1
5. Give an example of linkage isomerism. 1
6. A solution of KOH hydrolyses CH
3
CHClCH
2
CH
3
 and CH
3
CH
2
CH
2
CH
2
Cl.
Which one of these is more easily hydrolysed? 1
7. Draw the structural formula of I-phenylpropan-l-one molecule. 1
8. Give the IUPAC name of H
2
N – CH
2
 – CH
2
 - CH = CH
2
.1
175
9. Non-ideal solutions exhibit either positive or negative deviations from Raoult’s law.
What are these deviations and why are they caused? Explain with one example for
each type. 2
10. A reaction is of first order in reactant A and of second order in reactant B. How is
the rate of this reaction affected when (i) the concentration of B alone is increased to
three times (ii) the concentrations of A as well as B are doubled? 2
11. The rate constant for a reaction of zero order in A is 0.0030 mol L 
–1
 s
–1
. How long
will it take for the initial concentration of A to fall from 0.10 M to 0.075 M ? 2
12. Draw the structures of white phosphorus and red phosphorus. Which one of these
two types of phosphorus is more reactive and why? 2
13. Explain the following observations:
(i) Generally there is an increase in density of elements from titanium (Z = 22) to
copper (Z = 29) in the first series of transition elements.
(ii) Transition elements and their compounds are generally found to be good
catalysts in chemical reactions. 2
14. Name the following coordination compounds according to IUP AC system of nom-
enclature:
(i) [Co(NH
3
)
4
 (H
2
O)Cl]Cl
2
(ii) [CrCl
2
(en)
2
]Cl, (en = ethane – 1, 2 – diamine) 2
15. Illustrate the following reactions giving a chemical equation for each:
(i) Kolbe’s reaction,
(ii) W illiamson synthesis. 2
16. How are the following conversions carried out?
(i) Benzyl chloride to benzyl alcohol,
(ii) Methyl magnesium bromide to 2-methylpropan-2-ol. 2
176
17. Explain the following terms. :
(i) Invert sugar
(ii) Polypeptides
OR
Name the products of hydrolysis of sucrose. Why is sucrose not a reducing sugar? 2
18. What are essential and non-essential amino acids in human food? Give one example
of each type. 2
19. The well known mineral fluorite is chemically calcium fluoride. It is known that in
one unit cell of this mineral there are 4 Ca
2+
 ions and 8 F
–
 ions and that Ca
2+
 ions are
arranged in a fcc lattice. The F
–
 ions fill all the tetrahedral holes in the face centred
cubic lattice of Ca
2+
 ions. The edge of the unit cell is 5.46x10
–8
 cm in length. The
density of the solid is 3.18 g cm
–3
. Use this information to calculate Avogadro’s
number (Molar mass of CaF
2
 = 78.08 g mol
–1
)3
20. A solution prepared by dissolving 1.25 g of oil of winter green (methyl salicylate) in
99.0 g of benzene has a boiling point of 80.31 °C. Determine the molar mass of this
compound. (B.P . of pure benzene = 80.10 °C and K
b
 for benzene = 2.53 °C kg
mol
–1
) 3
21. What is the difference between multi molecular and macromolecular colloids? Give
one example of each type. How are associated colloids different from these two
types of col1oids ? 3
22. Describe how the following changes are brought about:
(i) Pig iron into steel.
(ii) Zinc oxide into metallic zinc.
(iii) Impure titanium into pure titanium. 3
OR
Describe the role of
(i) NaCN in the extraction of gold from gold are.
177
(ii) SiO
2
 in the extraction of copper from copper matte.
(iii) Iodine in the refining of zirconium.
Write chemical equations for the involved reactions.
23. How would you account for the following?
(i) The atomic radii of the metals of the third (5d) series of transition elements are
virtually the same as those of the corresponding members of the second (4d)
series.
(ii) The E
o
 value for the Mn
3+
/Mn
2+
 couple is much more positive than that for
Cr
3+
/Cr
2+
 couple or Fe
3+
/Fe
2+
 couple.
(iii) The highest oxidation state of a metal is exhibited in its oxide or fluoride. 3
24. (i) State one use each of DDT and iodoform.
(ii) Which compound in the following couples will react faster in S
N
2
 displacement
and why?
(a) 1-Bromopentane or 2-bromopentane
(b) 1-Bromo-2-methylbutane or 2-bromo-2-methylbutane. 3
25. In the following cases rearrange the compounds as directed:
(i) In an increasing order of basic strength:
C
6
H
5
NH
2
, C
6
H
5
N(CH
3
)
2
, (C
2
H
5
)
6
NH and CH
3
NH
2
(ii) In a decreasing order of basic strength:
Aniline, p-nitroaniline and p-toluidine
(iii) In an increasing order of pK
b
 values:
C
2
H
5
NH
2
, C
6
H
5
 NHCH
3
, (C
2
H
5
)
2
NH and C
6
H
5
NH
2
3
178
26. Give one example each of
(i) addition polymers,
(ii) condensation polymers,
(iii) copolymers. 3
27. What are analgesic medicines? How are they c1assifiedand when are they
commonly recommended for use? 3
28. (a) State Kohlrausch law of independent migration of ions. Write an expression
for the molar conductivity of acetic acid at infinite dilution according to
Kohlrausch law .
(b) Calculate /\
o
m
 for acetic acid.
Given that /\
o
m
 (HCl) = 426 S cm
2
 mol
–1
/\
o
m
 (NaCl) = 126 S cm
2
 mol
–1
/\
o
m
 (CH
3
COONa) = 91 S cm
2
 mol
–1
5
OR
(a) Write the anode and cathode reactions and the overall reaction occurring in a
lead storage battery.
(b) A copper-silver cell is set up. The copper ion concentration is 0.10 M. The
concentration of silver ion is not known. The cell potential when measured
was 0.422 V . Determine the concentration of silver ions in the cell. (Given
E
o
 
Ag+/Ag
 = + 0.80 V , E
o
 
cu
2+
/cu
 =  + 0.34 V) 5
29. (a) Complete the following chemical equations:
(i) NaOH
(aq)
 + Cl
2(g)
 
(Hot and cone.)
(ii) XeF
6
(s) + H
2
O(l) 
Read More
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