Equilibrium Practice Questions
NEET · Chemistry · 1567 free MCQs with instant results and detailed explanations.
1567
Total
354
Easy
694
Medium
519
Hard
Start Practicing Equilibrium
Take a timed quiz or customize your practice session
Topics in Equilibrium
Chemical Equilibrium
226
Le Chatelier's Principle
236
Ionic Equilibrium
215
pH
208
Law of Mass Action
227
Buffer
230
Solubility Product
225
Sample Questions from Equilibrium
Here are 10 sample questions. Start a quiz to get randomized questions with scoring.
Q1
Easy
What is the equilibrium constant (Kc) expression for the reaction: 2A + B ⇌ 3C?
A.
Kc = [C]^3 / [A]^2[B]
B.
Kc = [A]^2[B] / [C]^3
C.
Kc = [B] / [A]^2[C]^3
D.
Kc = [A][B] / [C]^3
Show Answer & Explanation
Correct Answer: A
The equilibrium constant expression is derived from the concentrations of the products raised to their coefficients divided by the reactants raised to their coefficients. Here, Kc = [C]^3 / ([A]^2[B]).
Q2
Easy
If the concentration of reactants increases in a closed system, what will happen to the equilibrium position according to Le Chatelier's principle?
A.
Shifts to the left
B.
Shifts to the right
C.
Remains unchanged
D.
Depends on the temperature
Show Answer & Explanation
Correct Answer: B
Le Chatelier's principle states that if a change is applied to a system at equilibrium, the system adjusts in a way to counteract the change. Increasing reactant concentration causes the equilibrium to shift to the right to produce more products.
Q3
Easy
In a dynamic equilibrium, which statement is true?
A.
The concentrations of reactants and products remain constant.
B.
The forward reaction stops.
C.
The reaction has completed.
D.
All reactants are converted to products.
Show Answer & Explanation
Correct Answer: A
In dynamic equilibrium, the rate of the forward reaction equals the rate of the backward reaction, leading to constant concentrations of reactants and products, even though reactions continue to occur.
Q4
Medium
In a chemical equilibrium represented by the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), if the concentration of NH3 is increased, what will be the immediate effect on the system according to Le Chatelier's Principle?
A.
The equilibrium will shift to the left, favoring the reactants.
B.
The equilibrium will shift to the right, producing more NH3.
C.
The equilibrium will remain unchanged.
D.
The rate of the forward reaction will decrease.
Show Answer & Explanation
Correct Answer: A
According to Le Chatelier's Principle, if a change is made to a system at equilibrium, the system will adjust to counteract that change. Increasing the concentration of NH3 will cause the system to shift to the left to use up some of the added NH3, thereby favoring the formation of reactants N2 and H2.
Q5
Medium
For the equilibrium reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the volume of the container is increased?
A.
The equilibrium shifts to the right.
B.
The equilibrium shifts to the left.
C.
No change in equilibrium position.
D.
SO3 concentration increases.
Show Answer & Explanation
Correct Answer: B
Increasing the volume of the container decreases the pressure, causing the equilibrium to shift to the side with more gas molecules, which is the left side (2SO2 + O2).
Q6
Medium
In a closed system at equilibrium, if the temperature is increased in an exothermic reaction, what is the expected effect on the equilibrium position?
A.
Equilibrium shifts to the right.
B.
Equilibrium shifts to the left.
C.
Equilibrium remains unchanged.
D.
Rate of the forward reaction increases.
Show Answer & Explanation
Correct Answer: B
In an exothermic reaction, increasing the temperature shifts the equilibrium to the left to absorb the excess heat, thus favoring the reactants.
Q7
Medium
For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), calculate the equilibrium constant (Kc) if the equilibrium concentrations are [N2] = 0.2 M, [H2] = 0.6 M, and [NH3] = 0.4 M.
A.
1.0
B.
0.5
C.
2.0
D.
0.25
Show Answer & Explanation
Correct Answer: C
Kc is calculated using the formula Kc = [NH3]^2 / ([N2][H2]^3). Substituting yields Kc = (0.4^2) / (0.2 * 0.6^3) = 2.0.
Q8
Hard
At equilibrium, for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), the equilibrium constant (Kc) is 4.0 at a given temperature. If 0.5 moles of N2 and 1.5 moles of H2 are mixed in a 2L container, what is the equilibrium concentration of NH3?
A.
0.5 M
B.
1.0 M
C.
1.5 M
D.
0.25 M
Show Answer & Explanation
Correct Answer: B
At equilibrium, the concentration of NH3 is found to be 1.0 M, which satisfies the equilibrium expression Kc = [NH3]^2 / ([N2][H2]^3).
Q9
Hard
For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), if the concentration of SO2 is doubled while keeping temperature constant, what will happen to the equilibrium position according to Le Chatelier's principle?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Depends on the rate of reaction
Show Answer & Explanation
Correct Answer: A
According to Le Chatelier's principle, increasing the concentration of a reactant will shift the equilibrium position to the right to counteract the change.
Q10
Hard
A 1L container holds 2 moles of A and 1 mole of B at equilibrium in the reaction A(g) + B(g) ⇌ C(g). If Kp for this reaction is 0.5 at a certain temperature, what is the partial pressure of C at equilibrium?
A.
0.25 atm
B.
0.5 atm
C.
1.0 atm
D.
0.75 atm
Show Answer & Explanation
Correct Answer: A
Using the expression Kp = (PC) / (PA * PB), and substituting the moles and solving gives PC = 0.25 atm.
Showing 10 of 1567 questions. Start a quiz to practice all questions with scoring and timer.
Practice All 1567 Questions →More Chemistry Chapters
Other NEET Subjects
Equilibrium — NEET Chemistry Practice Questions Online
This page contains 1567 practice MCQs for the chapter Equilibrium in NEET Chemistry. The questions are organized by difficulty — 354 easy, 694 medium, 519 hard — so you can choose the right level for your preparation.
Every question includes a detailed explanation to help you understand the concept, not just memorize answers. Take a timed quiz to simulate exam conditions, or practice at your own pace with no time limit. This chapter covers 7 topics, giving you comprehensive coverage of the entire chapter.