JAC Class 12 Chemistry Question Paper 2015 with Solution

About this paper

This is the Jharkhand Academic Council (JAC) Class 12 Chemistry paper from the 2015 board examination, with answers under most questions. Its 34 questions are grouped as multiple choice (Questions 1–8), very short answer (9–15), Short Answer I (16–23), Short Answer II (24–31) and long answer (32–34), with 'Or' choices in Questions 21, 25, 26, 32, 33 and 34. Numerical items include the electrode potential of an Mg²⁺/Mg electrode at 0.01 M and the rates of production of N₂ and H₂ in the zero-order decomposition of ammonia on platinum. Marks and time are not printed. Several printed multiple-choice answers are wrong, so check them before relying on them.

Exam

JAC Class 12

Subject

Chemistry

Year

2015

Questions

34

Pages

3

Answers included

Yes

Paper pattern

• Questions 1–8

  Multiple-choice questions

• Questions 9–15

  Very short answer questions

• Questions 16–23

  Short Answer I questions; internal choice in Question 21

• Questions 24–31

  Short Answer II questions; internal choice in Questions 25 and 26

• Questions 32–34

  Long answer questions, each with an 'Or' choice

Topics covered

• Solid state
• Solutions and colligative properties
• Electrochemistry
• Chemical kinetics
• Surface chemistry
• Minerals and ores
• p-Block elements
• d- and f-block elements
• Coordination compounds
• Haloalkanes and haloarenes
• Alcohols, ethers, carbonyl compounds and amines
• Biomolecules, polymers and drugs

Questions from this paper

1. Can we separate the components of an azeotropic mixture by fractional distillation?
2. State and explain Kohlrausch's law.
3. Aniline is a weaker base than ethylamine. Explain.
4. Find the volume in mL of 0.1 M HCl required to completely neutralise 1 g of a mixture of Na₂CO₃ and NaHCO₃ containing equal numbers of moles of each.
5. What is the value of the electrode potential of an Mg²⁺/Mg electrode dipped in a solution in which the concentration of Mg²⁺ is 0.01 M? (E°Mg²⁺/Mg = −2.36 V)
6. Derive the integrated rate equation for a first-order reaction.