This Practice Paper is prepared by Sankalp Institute after analyzing and collecting all the relevant information about how to prepare for the examination on behalf of the Jharkhand Academic Council. During the creation of this Practice Paper, the Institute took into account the challenges that students face when taking their examinations, such as understanding the types of questions, learning how to manage their time, and learning how to write clear answers in a well-structured manner.
This Practice Paper is designed in a manner in which the layout of the Practice Paper is easy for students to understand and follow. The content within this Practice Paper strictly follows the syllabus of the Jharkhand Academic Council, along with the pattern of the examination. The Practice Paper includes the important topics for which students, throughout the entire curriculum of JAC, are most frequently asked questions, in addition to all types of questions that can be expected in the examinations. The intention of providing the written Practice Paper is to assist students in their preparation, in addition to providing comfort to the students with respect to their examination process.
This Practice Paper is structured in a manner to provide all students with a combination of objective, short answer, and long answer questions to give complete exam-oriented preparation. This structure proves to be beneficial as it provides a means for all students to evaluate their knowledge base, locate areas of weakness, and continually improve on those identified areas of weakness through continuous practice and testing of knowledge.
The Practice Paper is a helpful study resource for all students of the Jharkhand Academic Council. If students choose to regularly utilize the Practice Paper, it can offer students increased confidence in their ability to perform well in the examination and provide a cosy and calming atmosphere within the examination hall.
Model Practice Set
Class: XII
Subject: Chemistry
Time: 3 Hours
Full Marks: 70
GENERAL INSTRUCTIONS:
Read the following instructions carefully.
1. There are 32 questions in this question paper with internal choice.All questions are compulsory.
2. Section A consists of 10 multiple-choice questions carrying 1 mark each.
3. Section B consists of 10 very short answer questions carrying 2 marks each,
4. Section C consists of 8 short answer questions carrying 3 marks each.
5. Section D consists of 4 long answer type questions carrying 5 marks each.
6. Use of log tables and calculators is not allowed.
Section – A
(Objective Type Questions)
(1 × 10 = 10 Marks)
Q1. Which of the following is a strong electrolyte?
(a) Acetic acid
(b) Ammonium hydroxide
(c) Sodium chloride
(d) Phenol
Q2. The shape of the complex ion [Ni(CN)₄]²⁻ is:
(a) Tetrahedral
(b) Square planar
(c) Octahedral
(d) Trigonal planar
Q3. Which of the following pairs forms an ideal solution?
(a) Ethanol + water
(b) Acetone + chloroform
(c) Benzene + toluene
(d) Acetone + water
Q4. The oxidation state of chromium in Cr₂O₇²⁻ is:
(a) +3
(b) +4
(c) +6
(d) +7
Q5. Which alcohol gives an immediate positive Lucas test?
(a) Methanol
(b) Ethanol
(c) Propan-1-ol
(d) tert-Butyl alcohol
Q6. Which gas is evolved when zinc reacts with dilute hydrochloric acid?
(a) Oxygen
(b) Nitrogen
(c) Hydrogen
(d) Chlorine
Q7. The number of moles present in 44 g of CO₂ is:
(a) 0.5
(b) 1
(c) 2
(d) 44
Q8. Which of the following compounds does not show hydrogen bonding?
(a) Water
(b) Ethanol
(c) Ammonia
(d) Methane
Q9. Which of the following acts as an oxidising agent in acidic medium?
(a) KMnO₄
(b) NaCl
(c) Zn
(d) Cu
Q10. The IUPAC name of CH₃CH₂OH is:
(a) Methanol
(b) Propanol
(c) Ethanol
(d) Ethanal
Section – B
(Very Short Answer Type)
(2 × 10 = 20 Marks)
Q11. (a) Define molar conductivity. Explain its variation with concentration for strong electrolytes.
(b)Mention any two functions of RNA present in living cells.
Q12. (a) Distinguish between molarity and molality.
(b)Write any two characteristics of an ideal solution.
Q13. (a)Explain why transition metals form complex compounds.
(b)Find the oxidation state of iron in K₄[Fe(CN)₆].
Q14. Write the geometrical isomers of the coordination compound [CoCl₃(NH₃)₃].
Q15. Write any two differences between methanol and ethanol.
Q16. What happens when phenol reacts with:
(a) Sodium hydroxide
(b) Dilute nitric acid
Q17. Complete the following reactions:
(i) R–OH + PCl₅ →
(ii) R–OH + PCl₃ →
Q18. Complete the reactions:
(i) I₂ + Na₂S₂O₃ →
(ii) NaBr + H₂SO₄ (Δ, MnO₂) →
Q19. Write balanced chemical equations for:
(i) Cr₂O₇²⁻ + Fe²⁺ + H⁺ →
(ii) Cr₂O₇²⁻ + I⁻ + H⁺ →
Q20. (a) Mention any two factors that affect the rate of a chemical reaction.
(b) What is activation energy?
Section – C
(Short Answer Type)
(3 × 8 = 24 Marks)
Q21. State Kohlrausch’s law of independent migration of ions and explain it briefly.
Q22. 6.02 × 10²⁴ molecules of urea are present in 100 mL of solution. Calculate the concentration of the solution.
Q23. What are transition elements? Explain why zinc is not considered a transition element.
Q24. Complete the following reactions:
(i) P₄ + HNO₃ →
(ii) Ca₃P₂ + H₂O →
(iii) NaClO₄ + HCl →
Q25. Complete the reactions:
(i) CH₃CHO + NH₂OH →
(ii) Aniline + Bromine water →
Q26. Distinguish between:
(i) Chlorobenzene and benzyl chloride
(ii) Chlorobenzene and cyclohexyl chloride
Q27. Define the following terms:
(i) Molarity
(ii) Molality
(iii) Mole fraction
Q28. Calculate the oxidation state of the central metal ion in the following complexes:
(i) [Cr(H₂O)₆]Cl
(ii) [Co(NH₃)₆]Cl₃
Section – D
(Long Answer Type Questions)
(5 × 4 = 20 Marks)
Q29. (a) How will you carry out the following conversions?
(i) Propane → Propan-2-ol
(ii) Ethyl magnesium bromide → Propan-2-ol
(iii) Benzyl chloride → Benzyl alcohol
(b) Why is zinc not regarded as a transition element?
(c) What is meant by a ligand in coordination chemistry?
Q30. (a) Complete the following reactions with suitable conditions:
(i) Aniline + CHCl₃ + KOH →
(ii) Benzene diazonium chloride + Ethanol →
(iii) Ethylamine + Nitrous acid →
(b) Calculate the electrode potential of Mg²⁺/Mg electrode when
E° = −2.36 V and concentration of Mg²⁺ is 0.01 M.
Q31. (a) Explain the dehydration of alcohols with a suitable example.
(b) Write the IUPAC name of K₃[Fe(CN)₆].
(c) Why is aniline weaker as a base compared to ethylamine?
Q32. (a) Write the IUPAC names of the following coordination compounds:
(i) [Mn(H₂O)₆]²⁺
(ii) K₃[Fe(CN)₆]
(iii) [Cr(NH₃)₆]Cl₃
(b) Write any two differences between physisorption and chemisorption.
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