PSEB Class 12 Chemistry September Examination – Sample Paper

PSEB Class 12 Chemistry September Sample Paper 2026 – Punjab Board 12th Chemistry Model Paper

PSEB Class 12 Chemistry September Sample Paper 2026 is now available for students preparing for the September examination. This sample paper has been prepared according to the syllabus covered for the September exam and follows the planned 70-mark theory paper structure.

This PSEB 12th Chemistry Sample Paper 2026 is useful for students who want to practise MCQs, short-answer questions, numericals, competency-based questions, case-study questions and long-answer questions before the September examination.

Important: This is a practice/sample paper prepared for students. It should be used along with the official PSEB syllabus, instructions and school-level examination guidance.

PSEB Class 12 Chemistry September Sample Paper 2026

Particular	Details
Board	Punjab School Education Board (PSEB)
Class	12th / Senior Secondary
Subject	Chemistry
Exam	September Examination 2026
Session	2026-27
Theory Marks	70 Marks
Time	3 Hours
Question Paper	21 Main Questions

PSEB Class 12 Chemistry September Exam Syllabus 2026

The September sample paper covers the chapters included in the September examination preparation:

1. Solutions
2. Electrochemistry
3. Chemical Kinetics
4. d- and f-Block Elements
5. Coordination Compounds
6. Biomolecules

Students should revise the complete prescribed content of these chapters before attempting the sample paper. The question selection includes conceptual questions, numerical problems, reasoning-based questions and application-oriented questions.

Chapter-Wise Marks Distribution

Chapter	Marks
Solutions	12
Electrochemistry	11
Chemical Kinetics	12
d- and f-Block Elements	12
Coordination Compounds	12
Biomolecules	11
Total	70 Marks

The distribution has been kept approximately balanced so that students get practice from all the chapters included in the September examination.

PSEB Class 12 Chemistry Question Paper Structure 2026

The sample paper has been arranged into four sections:

Section	Question Type	Questions	Marks
Section A	Multiple Choice Questions	18	18
Section B	Very Short Answer	12 × 2 marks	24
Section C	Short Answer	6 × 3 marks	18
Section D	Long Answer	2 × 5 marks	10
Total			70

What Types of Questions Are Included?

The PSEB Class 12 Chemistry September Sample Paper 2026 includes different types of questions so that students can practise the complete examination pattern.

• Multiple Choice Questions (MCQs)
• Conceptual questions
• Numerical problems
• Reasoning-based questions
• Application-based questions
• Analysis-based questions
• Case-study based question
• Short-answer questions
• Long-answer questions
• Questions with internal choice

Competencies Used in the Chemistry Sample Paper

The sample paper has been designed with attention to different learning competencies rather than relying only on memory-based questions.

1. Knowledge

Knowledge-based questions test basic facts, definitions, formulae, terminology and fundamental concepts. Examples include identifying a colligative property, the standard hydrogen electrode potential, a ligand or a nitrogenous base.

2. Understanding

Understanding-based questions require students to explain concepts and demonstrate that they understand the reason behind a chemical phenomenon. Questions related to molality, pseudo-first-order reactions, catalysts, hydrogen bonding and coordination compounds are examples of this category.

3. Application

Application-based questions require students to use a concept, formula or principle in a given situation. Numerical problems from Solutions, Electrochemistry and Chemical Kinetics are particularly useful for developing this competency.

4. Analysis

Analysis-based questions require students to interpret information, compare situations and apply chemical reasoning. Examples include explaining colour in transition-metal ions, magnetic behaviour of coordination compounds and the effect of concentration on reaction rate.

The purpose of including these competencies is to make preparation more useful for both school examinations and the final board examination.

Numerical Questions Included

Numerical practice is an important part of Class 12 Chemistry preparation. The sample paper includes numerical questions from important areas such as:

• Molality and molar mass
• Elevation in boiling point
• Standard cell EMF
• Electrochemical calculations
• Rate constant and half-life
• First-order reaction calculations
• Percentage decomposition

Students should write the formula first, substitute the values carefully and mention the correct unit in the final answer.

Internal Choice in the Sample Paper

Internal choices have been included in the sample paper to provide students with examination-style practice.

• Internal choices in selected 2-mark questions
• Internal choices in selected 3-mark questions
• Internal choice in both 5-mark questions

Students should practise both alternatives rather than preparing only one question from an internal-choice pair.

Case Study Question

The sample paper also includes a case-study based question. The case is based on glucose and asks students to apply their knowledge of carbohydrates, energy and the reducing nature of glucose.

Case-study questions are important because students need to read the given situation carefully before answering the individual sub-questions.

How to Prepare for the PSEB Class 12 Chemistry September Exam?

1. Complete the six chapters first

Make sure that the complete September syllabus is revised before starting the sample paper.

2. Memorise important formulae

Pay special attention to formulae from Solutions, Electrochemistry and Chemical Kinetics. Practise using the formulae instead of merely memorising them.

3. Practise numericals regularly

Numerical questions can become scoring questions if the calculation steps are written correctly. Practise at least a few numerical problems every day.

4. Revise inorganic chemistry systematically

For d- and f-Block Elements and Coordination Compounds, revise oxidation states, colour, magnetic properties, important reactions, ligands, nomenclature, coordination number and related concepts.

5. Prepare Biomolecules through comparison tables

For Biomolecules, revise carbohydrates, amino acids, proteins, vitamins and DNA/RNA through short notes and comparison tables.

6. Attempt the sample paper in 3 hours

Do not solve the sample paper casually. Sit for the complete three-hour duration and attempt it as if you were appearing in the actual examination.

Benefits of Solving This Sample Paper

• Helps students understand the September examination pattern.
• Provides practice for 1, 2, 3 and 5-mark questions.
• Improves numerical-solving speed.
• Provides practice for competency-based questions.
• Helps identify weak chapters before the examination.
• Improves time management.
• Provides practice with internal-choice questions.
• Helps students revise the September syllabus systematically.

PSEB Class 12 Chemistry Sample Paper 2026 – Important Keywords

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Frequently Asked Questions (FAQs)

What is the total marks of the PSEB Class 12 Chemistry theory paper?

The Chemistry theory component is 70 marks. The PSEB 2026–27 scheme lists Chemistry with 70 theory marks, 25 practical marks and 5 marks for project work/internal assessment.

Which chapters are included in this September Chemistry sample paper?

The sample paper covers Solutions, Electrochemistry, Chemical Kinetics, d- and f-Block Elements, Coordination Compounds and Biomolecules.

How many questions are included in the sample paper?

The paper contains 21 main questions, divided into four sections and carrying a total of 70 marks.

Does the sample paper include numerical questions?

Yes. Numerical questions have been included particularly from Solutions, Electrochemistry and Chemical Kinetics.

Does the paper contain competency-based questions?

Yes. The questions have been planned around Knowledge, Understanding, Application and Analysis so that students practise different levels of learning.

Is this the official PSEB September question paper?

No. This is a practice/sample paper prepared for examination preparation. Students should always follow the latest official PSEB instructions and syllabus for their examination.

Conclusion

The PSEB Class 12 Chemistry September Sample Paper 2026 is designed to provide structured practice for the September examination. Students should first revise the prescribed chapters, then attempt the complete paper within three hours and finally analyse their mistakes.

Regular practice of MCQs, numericals, short-answer questions, competency-based questions and long-answer questions can help students improve both accuracy and confidence before the examination.

Best wishes to all Class 12 Chemistry students for the September Examination 2026!

 

PSEB Class 12 Chemistry September Examination – Sample Paper

Time: 3 Hours
Maximum Marks: 70

General Instructions

1. All questions are compulsory.

2. The question paper consists of four sections – A, B, C and D.

3. Section A contains 18 multiple-choice questions of 1 mark each.

4. Section B contains 12 questions of 2 marks each. Internal choice is provided in three questions.

5. Section C contains 6 questions of 3 marks each. Internal choice is provided in two questions.

6. Section D contains 2 questions of 5 marks each. Both questions have internal choice.

7. Use of calculator is not permitted.

8. Show all necessary steps in numerical questions.

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SECTION A

Multiple Choice Questions

18 × 1 = 18 Marks

Q1. The number of moles of NaCl present in 3 L of a 3 M solution is:

a) 1 mol
b) 3 mol
c) 9 mol
d) 27 mol

Q2. Which of the following is a colligative property?

a) Vapour pressure
b) Relative lowering of vapour pressure
c) Viscosity
d) Surface tension

Q3. A solute undergoes dissociation into ions in a solution. The Van't Hoff factor $i$ will generally be:

a) Less than 1
b) Equal to 1
c) Greater than 1
d) Equal to 0

Q4. The electrode potential of the Standard Hydrogen Electrode (SHE) is:

a) +0.34 V
b) −0.76 V
c) 0.00 V
d) +1.10 V

Q5. According to Faraday's first law of electrolysis, the mass of a substance deposited is directly proportional to:

a) Resistance
b) Quantity of electricity passed
c) Conductivity
d) Cell constant

Q6. The standard reduction potentials of metals A, B and C are −1.4 V, +0.6 V and −3.4 V respectively. Which metal has the highest reducing power?

a) A
b) B
c) C
d) B and C equally

Q7. For a zero-order reaction, the rate of reaction:

a) Depends directly on concentration
b) Depends inversely on concentration
c) Does not depend on reactant concentration
d) Depends on the square of concentration

Q8. A catalyst increases the rate of a reaction by:

a) Increasing activation energy
b) Decreasing activation energy
c) Increasing enthalpy change
d) Increasing equilibrium constant

Q9. For a second-order reaction with rate law

$$Rate=k[A]^2$$

if the concentration of A is doubled, the rate becomes:

a) Half
b) Double
c) Four times
d) Eight times

Q10. Which of the following is not normally considered a transition element?

a) Fe
b) Mn
c) Zn
d) Cr

Q11. Vanadium pentoxide is used as a catalyst in the:

a) Haber process
b) Contact process
c) Solvay process
d) Ostwald process

Q12. Zn²⁺ compounds are generally colourless because Zn²⁺ has:

a) 3d⁰ configuration
b) 3d⁵ configuration
c) 3d⁹ configuration
d) 3d¹⁰ configuration

Q13. The coordination number of the central metal ion in

$$[PtCl_4]^{2-}$$

is:

a) 2
b) 4
c) 6
d) 8

Q14. Ethylenediamine (en) is a:

a) Monodentate ligand
b) Bidentate ligand
c) Tridentate ligand
d) Hexadentate ligand

Q15. Which complex is expected to be diamagnetic because CN⁻ acts as a strong-field ligand?

a) $[FeF_6]^{3-}$
b) $[Fe(CN)_6]^{4-}$
c) $[NiCl_4]^{2-}$
d) $[CoF_6]^{3-}$

Q16. Which nitrogenous base is present in RNA but not in DNA?

a) Cytosine
b) Guanine
c) Uracil
d) Thymine

Q17. The helical structure of a protein is mainly stabilised by:

a) Peptide bonds
b) Hydrogen bonds
c) Glycosidic bonds
d) Ester bonds

Q18. Glucose behaves as a reducing sugar because:

a) It contains a free aldehydic group in its open-chain form
b) It contains no oxygen
c) It is a disaccharide
d) It cannot undergo oxidation

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SECTION B

Very Short Answer Questions

12 × 2 = 24 Marks

Q19.
(a) Define molality. [1]
(b) Why is molality independent of temperature? [1]

Q20. A solution contains 2 g of a non-volatile solute dissolved in 100 g of water. The elevation in boiling point is 0.52 K. Calculate the molar mass of the solute.

Given:

$$K_b=0.52\;K\,kg\,mol^{-1}$$

Q21. For the Daniell cell:

$$Zn|Zn^{2+}||Cu^{2+}|Cu$$

Given:

$$E^\circ_{Zn^{2+}/Zn}=-0.76V$$ $$E^\circ_{Cu^{2+}/Cu}=+0.34V$$

Calculate the standard EMF of the cell.

Q22.
(a) Define molar conductivity. [1]
(b) Define equivalent conductivity. [1]

Q23. What is a pseudo-first-order reaction? Give one example.

Q24. A second-order reaction has the rate law:

$$Rate=k[A]^2$$

What happens to the rate when the concentration of A is:

(a) doubled? [1]
(b) reduced to half? [1]

Q25. Why are Zn and Cd generally not considered transition elements?

Give two reasons.

Q26. Explain why Zn²⁺ ions are colourless whereas Cu²⁺ ions are coloured.

Q27. Write the IUPAC name of:

$$[Co(NH_3)_5Cl]Cl_2$$

Also state the oxidation state of cobalt.

Q28. What is a chelating ligand? Give one example.

OR

Differentiate between a double salt and a coordination compound on the basis of their behaviour in aqueous solution.

Q29.
(a) What are α-amino acids? [1]
(b) Give one example of an α-amino acid. [1]

Q30. Why can Vitamin C not be stored in our body?

OR

Differentiate between reducing sugars and non-reducing sugars.

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SECTION C

Short Answer Questions

6 × 3 = 18 Marks

Q31. During winter, ethylene glycol is added to water in automobile radiators.

Answer the following:

(a) Name the colligative property responsible for lowering the freezing point. [1]

(b) Name the colligative property responsible for raising the boiling point. [1]

(c) Why are these properties called colligative properties? [1]

---

Q32. A solution of CuSO₄ is electrolysed using copper electrodes.

(a) Write the reaction occurring at the cathode. [1]

(b) Write the reaction occurring at the anode. [1]

(c) Why does the concentration of CuSO₄ solution remain approximately unchanged? [1]

---

Q33. A first-order reaction has a rate constant:

$$k=6.2\times10^{-3}\;s^{-1}$$

Calculate:

(a) the half-life of the reaction. [1]

(b) the time required for 75% decomposition of the reactant. [2]

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Q34. Explain the following:

(a) Transition metals exhibit variable oxidation states. [1]

(b) Transition metals and their compounds often act as catalysts. [1]

(c) Zr and Hf have almost identical atomic radii. [1]

OR

What is meant by lanthanide contraction? Explain its cause and state one consequence.

---

Q35. Explain why:

$$[Ni(CO)_4]$$

is diamagnetic whereas

$$[NiCl_4]^{2-}$$

is paramagnetic.

Your answer should include the role of the ligand field.

---

Q36. Riya felt weak after a long race. Her coach gave her a glucose solution. Glucose is a monosaccharide and an important source of energy. It exists in open-chain and cyclic forms and gives positive tests with Fehling's solution and Tollens' reagent.

Answer the following:

(a) Why is glucose useful as a quick source of energy? [1]

(b) To which class of carbohydrates does glucose belong? [1]

(c) Why does glucose give a positive Tollens' test? [1]

OR

Differentiate between DNA and RNA on the basis of:

1. Sugar

2. Nitrogenous bases

3. Biological role

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SECTION D

Long Answer Questions

2 × 5 = 10 Marks

Q37.

(a) Explain why addition of a non-volatile solute lowers the vapour pressure of the solvent. [1]

(b) Explain why the boiling point of the solution is higher than that of the pure solvent. [1]

(c) Write the relationship between standard Gibbs energy change and standard cell EMF. [1]

(d) Write the Arrhenius equation. [1]

(e) How does a catalyst affect the activation energy of a reaction? [1]

OR

(a) Define osmotic pressure. [1]

(b) Why is osmotic pressure useful for determining the molar mass of macromolecules? [1]

(c) State Faraday's first law of electrolysis. [1]

(d) Define activation energy. [1]

(e) What is the effect of increasing temperature on the rate constant of a reaction? [1]

---

Q38.

(a) What is meant by lanthanide contraction? [1]

(b) State one important consequence of lanthanide contraction. [1]

(c) Define coordination number. [1]

(d) What is a bidentate ligand? Give one example. [1]

(e) State one difference between glucose and fructose on the basis of their functional groups. [1]

OR

(a) Why do transition elements show variable oxidation states? [1]

(b) Why do transition-metal compounds generally show magnetic behaviour? [1]

(c) What is a strong-field ligand? [1]

(d) Give one example of a strong-field ligand. [1]

(e) Name the vitamin whose chemical name is ascorbic acid. [1]

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MARKS SUMMARY

Section	Marks
Section A – 18 MCQs	18
Section B – 12 × 2	24
Section C – 6 × 3	18
Section D – 2 × 5	10
Total	70

Chapter-wise weightage

Unit	Marks
Solutions	12
Electrochemistry	11
Chemical Kinetics	12
d- and f-Block Elements	12
Coordination Compounds	12
Biomolecules	11
Total	70