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Page 1
CBSE XII | Chemistry
Sample Paper 2
CBSE
Class XII Chemistry
Sample Paper 2
Time: 3 Hrs Total marks: 70
______________________________________________________________________________________________________________
General Instructions:
? All questions are compulsory.
? Section A: Q.no. 1 to 5 are very short answer questions and carry 1 mark each.
? Section B: Q.no. 6 to 12 are short answer questions and carry 2 marks each.
? Section C: Q.no. 13 to 24 are also short answer questions and carry 3 marks each.
? Section D: Q.no. 25 to 27 are long answer questions and carry 5 marks each.
? There is no overall choice. However, an internal choice has been provided in two questions
of one mark, two questions of two marks, four questions of three marks and all the three
questions of five marks weightage. You have to attempt only one of the choices in such
questions.
? Use log tables if necessary. Use of a calculator is not allowed.
Section A
1. Alcohols have a higher boiling point compared to isomeric ethers. Why? [1]
2. Define: Polymerisation [1]
3. What is the number of atoms in a unit cell of a cubic crystal? [1]
OR
What type of crystal defect is produced when sodium chloride is doped with MgCl2?
4. Give one example each of ‘oil in water’ and ‘water in oil’ emulsion. [1]
5. Calculate the magnetic moment of a divalent ion in aqueous solution if its atomic number is
25. [1]
OR
Arrange the following radicals in increasing order of their oxidising power:
7
2
4 2 2
MnO , VO , Cr O
? ? ?
Section B
6. A solution prepared by dissolving 1.25 g of methyl salicylate in 99.0 g of benzene has a
boiling point of 80.31 ?C. Determine the molar mass of this compound. [2]
(BP of pure benzene = 80.10 ?C and Kb for benzene = 2.53 ?C kg mol
-1
)
OR
Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr2 in 200 g of
water. (Molar mass of MgBr2 = 84 g) (Kf for water = 1.86 K kg mol
-1
)
Page 2
CBSE XII | Chemistry
Sample Paper 2
CBSE
Class XII Chemistry
Sample Paper 2
Time: 3 Hrs Total marks: 70
______________________________________________________________________________________________________________
General Instructions:
? All questions are compulsory.
? Section A: Q.no. 1 to 5 are very short answer questions and carry 1 mark each.
? Section B: Q.no. 6 to 12 are short answer questions and carry 2 marks each.
? Section C: Q.no. 13 to 24 are also short answer questions and carry 3 marks each.
? Section D: Q.no. 25 to 27 are long answer questions and carry 5 marks each.
? There is no overall choice. However, an internal choice has been provided in two questions
of one mark, two questions of two marks, four questions of three marks and all the three
questions of five marks weightage. You have to attempt only one of the choices in such
questions.
? Use log tables if necessary. Use of a calculator is not allowed.
Section A
1. Alcohols have a higher boiling point compared to isomeric ethers. Why? [1]
2. Define: Polymerisation [1]
3. What is the number of atoms in a unit cell of a cubic crystal? [1]
OR
What type of crystal defect is produced when sodium chloride is doped with MgCl2?
4. Give one example each of ‘oil in water’ and ‘water in oil’ emulsion. [1]
5. Calculate the magnetic moment of a divalent ion in aqueous solution if its atomic number is
25. [1]
OR
Arrange the following radicals in increasing order of their oxidising power:
7
2
4 2 2
MnO , VO , Cr O
? ? ?
Section B
6. A solution prepared by dissolving 1.25 g of methyl salicylate in 99.0 g of benzene has a
boiling point of 80.31 ?C. Determine the molar mass of this compound. [2]
(BP of pure benzene = 80.10 ?C and Kb for benzene = 2.53 ?C kg mol
-1
)
OR
Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr2 in 200 g of
water. (Molar mass of MgBr2 = 84 g) (Kf for water = 1.86 K kg mol
-1
)
CBSE XII | Chemistry
Sample Paper 2
7. Give the resonating structures of NO2 and N2O5. [2]
8. How is acetone obtained from ethanol? [2]
9. Write the electrode reactions taking place in the Ni–Cd cell. [2]
10. For reaction: A + H2O ? B, Rate a [A], what is its [2]
(a) Molecularity
(b) Order of reaction
11. Give a chemical test to distinguish between the following pairs of compounds. [2]
(a)
(b)
12. Classify the following as addition and condensation polymers: [2]
terylene, Bakelite, polyvinyl chloride, polyethene
Section C
13. Draw the structures of isomers, if any, and write the names of the following complexes: [3]
(a) [Cr(NH3)4Cl2]
+
(b) [Co(en)3]
3+
(c) [CoCl2(en)2]Cl
14. Examine the illustration of a portion of the defective crystal and answer the following
questions: [3]
(a) What are these types of valency defects called?
(b) How is the density of a crystal affected by these defects?
(c) Name one ionic compound which can show this type of
defect in the crystalline state.
Page 3
CBSE XII | Chemistry
Sample Paper 2
CBSE
Class XII Chemistry
Sample Paper 2
Time: 3 Hrs Total marks: 70
______________________________________________________________________________________________________________
General Instructions:
? All questions are compulsory.
? Section A: Q.no. 1 to 5 are very short answer questions and carry 1 mark each.
? Section B: Q.no. 6 to 12 are short answer questions and carry 2 marks each.
? Section C: Q.no. 13 to 24 are also short answer questions and carry 3 marks each.
? Section D: Q.no. 25 to 27 are long answer questions and carry 5 marks each.
? There is no overall choice. However, an internal choice has been provided in two questions
of one mark, two questions of two marks, four questions of three marks and all the three
questions of five marks weightage. You have to attempt only one of the choices in such
questions.
? Use log tables if necessary. Use of a calculator is not allowed.
Section A
1. Alcohols have a higher boiling point compared to isomeric ethers. Why? [1]
2. Define: Polymerisation [1]
3. What is the number of atoms in a unit cell of a cubic crystal? [1]
OR
What type of crystal defect is produced when sodium chloride is doped with MgCl2?
4. Give one example each of ‘oil in water’ and ‘water in oil’ emulsion. [1]
5. Calculate the magnetic moment of a divalent ion in aqueous solution if its atomic number is
25. [1]
OR
Arrange the following radicals in increasing order of their oxidising power:
7
2
4 2 2
MnO , VO , Cr O
? ? ?
Section B
6. A solution prepared by dissolving 1.25 g of methyl salicylate in 99.0 g of benzene has a
boiling point of 80.31 ?C. Determine the molar mass of this compound. [2]
(BP of pure benzene = 80.10 ?C and Kb for benzene = 2.53 ?C kg mol
-1
)
OR
Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr2 in 200 g of
water. (Molar mass of MgBr2 = 84 g) (Kf for water = 1.86 K kg mol
-1
)
CBSE XII | Chemistry
Sample Paper 2
7. Give the resonating structures of NO2 and N2O5. [2]
8. How is acetone obtained from ethanol? [2]
9. Write the electrode reactions taking place in the Ni–Cd cell. [2]
10. For reaction: A + H2O ? B, Rate a [A], what is its [2]
(a) Molecularity
(b) Order of reaction
11. Give a chemical test to distinguish between the following pairs of compounds. [2]
(a)
(b)
12. Classify the following as addition and condensation polymers: [2]
terylene, Bakelite, polyvinyl chloride, polyethene
Section C
13. Draw the structures of isomers, if any, and write the names of the following complexes: [3]
(a) [Cr(NH3)4Cl2]
+
(b) [Co(en)3]
3+
(c) [CoCl2(en)2]Cl
14. Examine the illustration of a portion of the defective crystal and answer the following
questions: [3]
(a) What are these types of valency defects called?
(b) How is the density of a crystal affected by these defects?
(c) Name one ionic compound which can show this type of
defect in the crystalline state.
CBSE XII | Chemistry
Sample Paper 2
15. What method would you suggest for the separation of metals in the following mixtures? [3]
(a) Zinc and iron
(b) Copper and magnesium
(c) Rare earth
OR
Write the reactions taking place in the different zones in the blast furnace during the
extraction of iron.
16. 18 g of glucose, C6H12O6, is dissolved in 1 kg of water in a saucepan. At what temperature
will water boil at 1.013 bar? (Kb for water is 0.52 K kg mol
-1
.) [3]
OR
Why is the boiling point of a solution containing a non-volatile solute more than that of pure
solvent? Explain graphically.
17. [3]
(a) Give the mechanism of acid-catalysed dehydration of ethanol to yield ethyne.
(b) Compound (A) C4H10O is found to be soluble in sulphuric acid. (A) does not react with
sodium metal or potassium permanganate. When it is heated with excess of HI, it is
converted to a single alkyl halide. What is the structural formula of (A)?
18. It is observed that the rate of a chemical reaction doubles with every 10
°
rise in
temperature. If this generalisation holds good for a reaction in the temperature range 295–
305 K, what would be the volume of activation energy for this reaction? [3]
(R = 8.314 J/Kmol)
19. [3]
(a) Give two reasons to support the cyclic structure of glucose.
(b) Why are amino acids soluble in water?
(c) Name the pyrimidine bases present in DNA and RNA.
20. Explain the following observations: [3]
(a) Lyophilic colloid is more stable than lyophobic colloid.
(b) Coagulation takes place when sodium chloride solution is added to a colloidal solution of
ferric hydroxide.
(c) The sky appears blue in colour.
21. [3]
(a) Distinguish between
(i) Aniline and benzyl amine
(ii) CH3CH2NH2 and (CH3)2NH
(b) Write a note on the Hoffmann bromamide reaction.
Page 4
CBSE XII | Chemistry
Sample Paper 2
CBSE
Class XII Chemistry
Sample Paper 2
Time: 3 Hrs Total marks: 70
______________________________________________________________________________________________________________
General Instructions:
? All questions are compulsory.
? Section A: Q.no. 1 to 5 are very short answer questions and carry 1 mark each.
? Section B: Q.no. 6 to 12 are short answer questions and carry 2 marks each.
? Section C: Q.no. 13 to 24 are also short answer questions and carry 3 marks each.
? Section D: Q.no. 25 to 27 are long answer questions and carry 5 marks each.
? There is no overall choice. However, an internal choice has been provided in two questions
of one mark, two questions of two marks, four questions of three marks and all the three
questions of five marks weightage. You have to attempt only one of the choices in such
questions.
? Use log tables if necessary. Use of a calculator is not allowed.
Section A
1. Alcohols have a higher boiling point compared to isomeric ethers. Why? [1]
2. Define: Polymerisation [1]
3. What is the number of atoms in a unit cell of a cubic crystal? [1]
OR
What type of crystal defect is produced when sodium chloride is doped with MgCl2?
4. Give one example each of ‘oil in water’ and ‘water in oil’ emulsion. [1]
5. Calculate the magnetic moment of a divalent ion in aqueous solution if its atomic number is
25. [1]
OR
Arrange the following radicals in increasing order of their oxidising power:
7
2
4 2 2
MnO , VO , Cr O
? ? ?
Section B
6. A solution prepared by dissolving 1.25 g of methyl salicylate in 99.0 g of benzene has a
boiling point of 80.31 ?C. Determine the molar mass of this compound. [2]
(BP of pure benzene = 80.10 ?C and Kb for benzene = 2.53 ?C kg mol
-1
)
OR
Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr2 in 200 g of
water. (Molar mass of MgBr2 = 84 g) (Kf for water = 1.86 K kg mol
-1
)
CBSE XII | Chemistry
Sample Paper 2
7. Give the resonating structures of NO2 and N2O5. [2]
8. How is acetone obtained from ethanol? [2]
9. Write the electrode reactions taking place in the Ni–Cd cell. [2]
10. For reaction: A + H2O ? B, Rate a [A], what is its [2]
(a) Molecularity
(b) Order of reaction
11. Give a chemical test to distinguish between the following pairs of compounds. [2]
(a)
(b)
12. Classify the following as addition and condensation polymers: [2]
terylene, Bakelite, polyvinyl chloride, polyethene
Section C
13. Draw the structures of isomers, if any, and write the names of the following complexes: [3]
(a) [Cr(NH3)4Cl2]
+
(b) [Co(en)3]
3+
(c) [CoCl2(en)2]Cl
14. Examine the illustration of a portion of the defective crystal and answer the following
questions: [3]
(a) What are these types of valency defects called?
(b) How is the density of a crystal affected by these defects?
(c) Name one ionic compound which can show this type of
defect in the crystalline state.
CBSE XII | Chemistry
Sample Paper 2
15. What method would you suggest for the separation of metals in the following mixtures? [3]
(a) Zinc and iron
(b) Copper and magnesium
(c) Rare earth
OR
Write the reactions taking place in the different zones in the blast furnace during the
extraction of iron.
16. 18 g of glucose, C6H12O6, is dissolved in 1 kg of water in a saucepan. At what temperature
will water boil at 1.013 bar? (Kb for water is 0.52 K kg mol
-1
.) [3]
OR
Why is the boiling point of a solution containing a non-volatile solute more than that of pure
solvent? Explain graphically.
17. [3]
(a) Give the mechanism of acid-catalysed dehydration of ethanol to yield ethyne.
(b) Compound (A) C4H10O is found to be soluble in sulphuric acid. (A) does not react with
sodium metal or potassium permanganate. When it is heated with excess of HI, it is
converted to a single alkyl halide. What is the structural formula of (A)?
18. It is observed that the rate of a chemical reaction doubles with every 10
°
rise in
temperature. If this generalisation holds good for a reaction in the temperature range 295–
305 K, what would be the volume of activation energy for this reaction? [3]
(R = 8.314 J/Kmol)
19. [3]
(a) Give two reasons to support the cyclic structure of glucose.
(b) Why are amino acids soluble in water?
(c) Name the pyrimidine bases present in DNA and RNA.
20. Explain the following observations: [3]
(a) Lyophilic colloid is more stable than lyophobic colloid.
(b) Coagulation takes place when sodium chloride solution is added to a colloidal solution of
ferric hydroxide.
(c) The sky appears blue in colour.
21. [3]
(a) Distinguish between
(i) Aniline and benzyl amine
(ii) CH3CH2NH2 and (CH3)2NH
(b) Write a note on the Hoffmann bromamide reaction.
CBSE XII | Chemistry
Sample Paper 2
22. [3]
(a) Why do transition metals form complex compounds?
(b) What is lanthanoid contraction?
(c) Why does Cr have a high melting point?
23. Arrange the following in order of increasing reactivity in SN1 and SN2 reactions: [3]
C6H5CH2Br, C6H5CH (C6H5) Br, C6H5CH (CH3) Br, C6H5C (CH3) (C6H5) Br
OR
What happens when
(a) Chloroethane is made to react with KCN.
(b) 1-Bromopropane reacts with silver acetate.
Give equations involved.
24. What are antihistamines? Give an example. Discuss their working in the human body. [3]
OR
Account for the following:
(a) Aspirin drug helps in the prevention of heart attack.
(b) Diabetic patients are advised to take artificial sweeteners instead of natural
sweeteners.
(c) Detergents are non-biodegradable, while soaps are biodegradable.
Section D
25. Complete the equations: [5]
(a) NaCl + MnO2 + H2SO4
(b) Al + O2
(c)
(d) C + H 2SO4 (conc.)
(e) PbS + O3
OR
Complete the equations:
(a) NH4Cl(aq) + NaNO2(aq)
(b) P4 + NaOH + H2O
(c) CaF2 + H2SO4
(d) NaOH (conc. hot) + Cl2
(e) PCl3 + H2O
?
?
? ? ? ? ?
673 K
32
2Pb(NO )
?
?
?
?
?
?
?
Page 5
CBSE XII | Chemistry
Sample Paper 2
CBSE
Class XII Chemistry
Sample Paper 2
Time: 3 Hrs Total marks: 70
______________________________________________________________________________________________________________
General Instructions:
? All questions are compulsory.
? Section A: Q.no. 1 to 5 are very short answer questions and carry 1 mark each.
? Section B: Q.no. 6 to 12 are short answer questions and carry 2 marks each.
? Section C: Q.no. 13 to 24 are also short answer questions and carry 3 marks each.
? Section D: Q.no. 25 to 27 are long answer questions and carry 5 marks each.
? There is no overall choice. However, an internal choice has been provided in two questions
of one mark, two questions of two marks, four questions of three marks and all the three
questions of five marks weightage. You have to attempt only one of the choices in such
questions.
? Use log tables if necessary. Use of a calculator is not allowed.
Section A
1. Alcohols have a higher boiling point compared to isomeric ethers. Why? [1]
2. Define: Polymerisation [1]
3. What is the number of atoms in a unit cell of a cubic crystal? [1]
OR
What type of crystal defect is produced when sodium chloride is doped with MgCl2?
4. Give one example each of ‘oil in water’ and ‘water in oil’ emulsion. [1]
5. Calculate the magnetic moment of a divalent ion in aqueous solution if its atomic number is
25. [1]
OR
Arrange the following radicals in increasing order of their oxidising power:
7
2
4 2 2
MnO , VO , Cr O
? ? ?
Section B
6. A solution prepared by dissolving 1.25 g of methyl salicylate in 99.0 g of benzene has a
boiling point of 80.31 ?C. Determine the molar mass of this compound. [2]
(BP of pure benzene = 80.10 ?C and Kb for benzene = 2.53 ?C kg mol
-1
)
OR
Calculate the freezing point of an aqueous solution containing 10.50 g of MgBr2 in 200 g of
water. (Molar mass of MgBr2 = 84 g) (Kf for water = 1.86 K kg mol
-1
)
CBSE XII | Chemistry
Sample Paper 2
7. Give the resonating structures of NO2 and N2O5. [2]
8. How is acetone obtained from ethanol? [2]
9. Write the electrode reactions taking place in the Ni–Cd cell. [2]
10. For reaction: A + H2O ? B, Rate a [A], what is its [2]
(a) Molecularity
(b) Order of reaction
11. Give a chemical test to distinguish between the following pairs of compounds. [2]
(a)
(b)
12. Classify the following as addition and condensation polymers: [2]
terylene, Bakelite, polyvinyl chloride, polyethene
Section C
13. Draw the structures of isomers, if any, and write the names of the following complexes: [3]
(a) [Cr(NH3)4Cl2]
+
(b) [Co(en)3]
3+
(c) [CoCl2(en)2]Cl
14. Examine the illustration of a portion of the defective crystal and answer the following
questions: [3]
(a) What are these types of valency defects called?
(b) How is the density of a crystal affected by these defects?
(c) Name one ionic compound which can show this type of
defect in the crystalline state.
CBSE XII | Chemistry
Sample Paper 2
15. What method would you suggest for the separation of metals in the following mixtures? [3]
(a) Zinc and iron
(b) Copper and magnesium
(c) Rare earth
OR
Write the reactions taking place in the different zones in the blast furnace during the
extraction of iron.
16. 18 g of glucose, C6H12O6, is dissolved in 1 kg of water in a saucepan. At what temperature
will water boil at 1.013 bar? (Kb for water is 0.52 K kg mol
-1
.) [3]
OR
Why is the boiling point of a solution containing a non-volatile solute more than that of pure
solvent? Explain graphically.
17. [3]
(a) Give the mechanism of acid-catalysed dehydration of ethanol to yield ethyne.
(b) Compound (A) C4H10O is found to be soluble in sulphuric acid. (A) does not react with
sodium metal or potassium permanganate. When it is heated with excess of HI, it is
converted to a single alkyl halide. What is the structural formula of (A)?
18. It is observed that the rate of a chemical reaction doubles with every 10
°
rise in
temperature. If this generalisation holds good for a reaction in the temperature range 295–
305 K, what would be the volume of activation energy for this reaction? [3]
(R = 8.314 J/Kmol)
19. [3]
(a) Give two reasons to support the cyclic structure of glucose.
(b) Why are amino acids soluble in water?
(c) Name the pyrimidine bases present in DNA and RNA.
20. Explain the following observations: [3]
(a) Lyophilic colloid is more stable than lyophobic colloid.
(b) Coagulation takes place when sodium chloride solution is added to a colloidal solution of
ferric hydroxide.
(c) The sky appears blue in colour.
21. [3]
(a) Distinguish between
(i) Aniline and benzyl amine
(ii) CH3CH2NH2 and (CH3)2NH
(b) Write a note on the Hoffmann bromamide reaction.
CBSE XII | Chemistry
Sample Paper 2
22. [3]
(a) Why do transition metals form complex compounds?
(b) What is lanthanoid contraction?
(c) Why does Cr have a high melting point?
23. Arrange the following in order of increasing reactivity in SN1 and SN2 reactions: [3]
C6H5CH2Br, C6H5CH (C6H5) Br, C6H5CH (CH3) Br, C6H5C (CH3) (C6H5) Br
OR
What happens when
(a) Chloroethane is made to react with KCN.
(b) 1-Bromopropane reacts with silver acetate.
Give equations involved.
24. What are antihistamines? Give an example. Discuss their working in the human body. [3]
OR
Account for the following:
(a) Aspirin drug helps in the prevention of heart attack.
(b) Diabetic patients are advised to take artificial sweeteners instead of natural
sweeteners.
(c) Detergents are non-biodegradable, while soaps are biodegradable.
Section D
25. Complete the equations: [5]
(a) NaCl + MnO2 + H2SO4
(b) Al + O2
(c)
(d) C + H 2SO4 (conc.)
(e) PbS + O3
OR
Complete the equations:
(a) NH4Cl(aq) + NaNO2(aq)
(b) P4 + NaOH + H2O
(c) CaF2 + H2SO4
(d) NaOH (conc. hot) + Cl2
(e) PCl3 + H2O
?
?
? ? ? ? ?
673 K
32
2Pb(NO )
?
?
?
?
?
?
?
CBSE XII | Chemistry
Sample Paper 2
26. [5]
(a) Decomposition of a compound follows first order kinetics. It takes 15 min for 20% of
the starting compound to react. Calculate
(i) Rate constant for the reaction.
(ii) Time at which 10% of the reactant is left unreacted.
(iii) Time taken for the next 20% of the reactant to react after the first 15 min.
(b) Derive a relationship between rate constant and half-life for a zero-order reaction.
OR
(a) The rates of a reaction starting with initial concentrations 2.0 × 10
-3
M and 1.0 × 10
-3
M are equal to 2.40 × 10
-4
M s
-1
and 0.60 × 10
-4
M s
-1
, respectively. Calculate the
order of the reaction with respect to the reactant and also the rate constant.
(b) For a reaction A + B C, it is found that
(i) Rate becomes double when concentration of A is doubled.
(ii) Rate becomes 16 times when concentration of both A and B are doubled.
(iii) Write the rate expression and calculate the overall order of the reaction.
27. [5]
(a) Convert:
(i) Acetic acid to ethylamine
(ii) Propionic acid to lactic acid
(b) Identify A, B and C in the following reactions:
OR
(a) Convert:
(i) Acetaldehyde to crotonic acid
(ii) Formaldehyde to chloroethane
(iii) Acetic acid to propanoic acid
(b) Identify A and B in the given equation:
?
? ? ? ? ? ? ? ? ? ? ? ? ? ? ? ?
42
LiAlH SOCl KOH(alc)
33
CH COCH A B C
? ? ? ? ? ? ?
Conc.NaOH
HCHO A + B
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FAQs on Chemistry: Sample Question Paper- 2, Class 12 - Sample Papers for Class 12 Medical and Non-Medical
| 1. What is the format of the Chemistry Class 12 Sample Question Paper-2? |  |
Ans. The format of the Chemistry Class 12 Sample Question Paper-2 typically includes multiple-choice questions, short-answer questions, and long-answer questions covering various topics in Chemistry.
| 2. What is the purpose of the Sample Question Paper-2 in Chemistry Class 12? | |
Ans. The purpose of the Sample Question Paper-2 in Chemistry Class 12 is to provide students with a practice test that simulates the actual exam. It helps them understand the exam pattern, assess their knowledge and exam readiness, and identify areas for improvement.
| 3. How can the Chemistry Class 12 Sample Question Paper-2 help in exam preparation? | |
Ans. The Chemistry Class 12 Sample Question Paper-2 can help in exam preparation by providing students with an opportunity to practice answering different types of questions. It familiarizes them with the question format, helps them manage time effectively, and allows them to identify their strengths and weaknesses in the subject.
| 4. What topics are covered in the Chemistry Class 12 Sample Question Paper-2? | |
Ans. The Chemistry Class 12 Sample Question Paper-2 covers a wide range of topics, including but not limited to: chemical reactions, chemical kinetics, electrochemistry, coordination compounds, organic chemistry, biomolecules, polymers, and surface chemistry. The paper aims to assess students' understanding of these topics as per the prescribed curriculum.
| 5. Are the questions in the Chemistry Class 12 Sample Question Paper-2 aligned with the difficulty level of the actual exam? | |
Ans. Yes, the questions in the Chemistry Class 12 Sample Question Paper-2 are designed to align with the difficulty level of the actual exam. They are carefully crafted to reflect the depth of understanding, analytical skills, and application of concepts required to excel in the subject. Students can use this sample paper to gauge their preparedness for the real exam.
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