Chemical Equilibrium JEE Questions PDF with Solution, Practice Now

Chemical Equilibrium JEE Questions is one of the most important and scoring topics of Chemistry in JEE Main and Advanced. This chapter explains how reversible reactions reach a steady state where the forward and backward reactions occur at the same rate. With JEE Main 2026 Session 2 being conducted from 2 April 2026 to 8 April 2026 by the National Testing Agency, focusing on such high-weightage topics becomes important during the ongoing exam phase.

Chemical Equilibrium forms a key part of the JEE Main exam pattern, as both theoretical concepts and numerical-based questions are frequently asked. Regular practice of chemical equilibrium questions for JEE Main and advanced-level problems helps students improve speed, accuracy, and confidence, making it easier to perform well during this crucial session.

Explore - JEE Online Courses

Chemical Equilibrium JEE Questions Overview

Chemical Equilibrium is a chapter under the section of Physical Chemistry in the JEE Main Syllabus. This chapter is given a high scoring pattern in JEE Main and Advanced. The concept of equilibrium is implemented in various day-to-day chemical reactions, like the synthesis of ammonia, biological systems, etc. Also, the industrial synthesis of some chemicals also come under equilibrium reactions. In JEE, this chapter is linked with Thermodynamics and Ionic Equilibrium, and it is one of the base chapters for other areas of Chemistry. The frequency with which chemical equilibrium questions appear in JEE Main previous years' papers indicates their importance.

Practice Chemical Equilibrium JEE Questions

By practicing a mix of chemical equilibrium JEE Mains and JEE Advanced equilibrium questions, students get exam-like experience and a feel of the depth required in each exam. Here are some Chemical Equilibrium JEE Questions: 

1. 2SrSO₄(s) ⇌ 2SrO(s) + 2SO₂(g) + O₂(g), ΔH > 0
Above equilibrium is established by taking some amount of SrSO₄(s) in a closed container at 1700 K. Then which of the following is incorrect option?

A. moles of SrO(s) will increase with the increase in temperature
B. If the volume of the container is doubled at equilibrium then partial pressure of SO₂(g) will change at new equilibrium
C. If the volume of the container is halved partial pressure of O₂(g) at new equilibrium will remain unchanged
D. moles of SrO(s) will increase on adding more strontium oxide at equilibrium

2. The vapour density of N₂O₄ at a certain temperature is 40. What is the % dissociation of N₂O₄ at this temperature?

A. 53.3 %
B. 10.66 %
C. 26.7 %
D. 15 %

3. A(s) ⇌ 2B(g) + C(g)
The above equilibrium was established by initially taking A(s) only. At equilibrium, B is removed so that its partial pressure at new equilibrium becomes 1/3rd of original total pressure. Ratio of total pressure at new equilibrium and at initial equilibrium will be:

A. 2/3
B. 14/13
C. 5/3
D. 17/19

4. A certain gas ‘x’ trimerises to a very small extent at a given temperature as 3A(g) ⇌ A₃(g). The reaction is started with one mole of A in a container of capacity 2L. Determine the value of PV/RT at equilibrium.

A. 1 − Kc/4
B. 1 − Kc/2
C. 3Kc/4
D. 1 − Kc/6

5. 2AB(g) ⇌ A₂(g) + B₂(g)
For the reaction the degree of dissociation (α) of AB(g) is related to equilibrium constant Kp by expression √x/Kp / (1 + 2√Kp). Calculate value of ‘x’.

A. 1
B. 2
C. 3
D. 5

6. The standard enthalpy change and standard free energy change for the equilibrium:
Zn(s) + H₂O(g) ⇌ ZnO(s) + H₂(g)
are 224 kJ mol⁻¹ and 33 kJ mol⁻¹ respectively at the temperature 920 K. Calculate the temperature at which equilibrium constant becomes 1. Assume ΔH remains constant.

A. 675.8 K
B. 1078.5 K
C. 987.7 K
D. 1201.2 K

7. The value of Kp for the reaction:
CO₂(g) + C(s) ⇌ 2CO(g)
is 3.0 bar at 1000 K. If initially CO₂, P = 0.48 bar, CO, P = 0 bar and pure graphite is present then determine equilibrium partial pressure of CO and CO₂.

A. PCO = 0.15 bar, PCO₂ = 0.66 bar
B. PCO = 0.66 bar, PCO₂ = 0.15 bar
C. PCO = 0.33 bar, PCO₂ = 0.66 bar
D. PCO = 0.66 bar, PCO₂ = 0.33 bar

8. Gas A (mol. mass 16) and gas B (mol. mass 4) are confined into a vessel at partial pressure of 2 atm each at 27°C. The gases are then allowed to effuse out at 27°C through a valve till the pressure inside the vessel becomes 2 atm after which the valve is closed and the gases are heated to 127°C and allowed to react as A + B ⇌ C, Kp = 0.1 atm⁻¹. Calculate the partial pressure of C at equilibrium assuming C is not formed till the effusing process is completed at 27°C.

A. 1.523 atm
B. 0.216 atm
C. 0.326 atm
D. 0.126 atm

Watch Chemical Equilibrium JEE Question Practice Video on YT

Chemical Equilibrium JEE Questions PDF with Solution

PW offers Practice Question PDFs with Answers and Solutions that match the JEE exam pattern to aid students' preparation. This PDF contains chemical equilibrium questions for JEE Mains with step-by-step solutions. Practicing from this PDF, students will learn shortcuts and formulas as well as presentation of answers in the exam.