Q. For the equilibrium 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen to the equilibrium? (2020)
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Depends on temperature
Solution
Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the right side in this case.
Q. For the equilibrium reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of decreasing the volume of the container? (2021)
A.
Shift to the left
B.
Shift to the right
C.
No effect
D.
Increase in temperature
Solution
Decreasing the volume increases the pressure, and according to Le Chatelier's principle, the equilibrium will shift towards the side with fewer moles of gas, which is the right side in this case.
Q. For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), if the volume of the container is decreased, what will happen to the equilibrium? (2021)
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Depends on the temperature
Solution
Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the right side (2 moles of SO3).
Q. For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the volume of the container is decreased? (2021)
A.
Equilibrium shifts to the left
B.
Equilibrium shifts to the right
C.
No change
D.
Depends on temperature
Solution
Decreasing the volume increases the pressure, and according to Le Chatelier's principle, the equilibrium will shift towards the side with fewer moles of gas, which is the right side in this case.
Correct Answer:
B
— Equilibrium shifts to the right
Q. For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of decreasing the volume? (2021)
A.
The equilibrium shifts to the left.
B.
The equilibrium shifts to the right.
C.
The equilibrium remains unchanged.
D.
The reaction stops.
Solution
Decreasing the volume increases the pressure, and according to Le Chatelier's principle, the equilibrium will shift towards the side with fewer moles of gas, which is the right side in this case.
Correct Answer:
B
— The equilibrium shifts to the right.
Q. For the reaction: 2A(g) + B(g) ⇌ 3C(g), if the volume of the container is decreased, what will be the effect on the equilibrium? (2022)
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Increase in temperature
Solution
Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas. Here, it shifts to the right, producing more C.
Q. For the reaction: 2A(g) + B(g) ⇌ 3C(g), what is the correct expression for the equilibrium constant Kc? (2021)
A.
[C]^3 / ([A]^2[B])
B.
[A]^2[B] / [C]^3
C.
[C]^3 / [A]^2
D.
[B] / [C]^3
Solution
The equilibrium constant Kc is given by the expression Kc = [C]^3 / ([A]^2[B]), where the concentrations are raised to the power of their coefficients.
Q. In a reaction at equilibrium, if the concentration of products is increased, what will happen? (2022)
A.
Equilibrium shifts to the left
B.
Equilibrium shifts to the right
C.
No change
D.
Reaction stops
Solution
According to Le Chatelier's principle, increasing the concentration of products will shift the equilibrium to the left, favoring the formation of reactants.
Correct Answer:
A
— Equilibrium shifts to the left
Q. In a reaction at equilibrium, if the concentration of reactants is increased, what will happen? (2022)
A.
The equilibrium will shift to the right.
B.
The equilibrium will shift to the left.
C.
The equilibrium will not change.
D.
The reaction will stop.
Solution
According to Le Chatelier's principle, if the concentration of reactants is increased, the equilibrium will shift to the right to produce more products.
Correct Answer:
A
— The equilibrium will shift to the right.
Q. In a reaction at equilibrium, if the concentration of reactants is increased, what will happen to the position of equilibrium? (2022)
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Depends on temperature
Solution
According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right to produce more products.
Q. In a reversible reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium position? (2023)
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Depends on temperature
Solution
According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.
Q. In a reversible reaction at equilibrium, what happens if the temperature is increased? (2019)
A.
The reaction shifts to the exothermic side
B.
The reaction shifts to the endothermic side
C.
No change occurs
D.
The reaction rate decreases
Solution
Increasing the temperature of an exothermic reaction shifts the equilibrium to the left (towards the reactants), while for an endothermic reaction, it shifts to the right (towards the products).
Correct Answer:
B
— The reaction shifts to the endothermic side
Q. The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 4. What is the value of Kp? (2023)
A.
4
B.
16
C.
0.25
D.
0.0625
Solution
Kp can be calculated from Kc using the relation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas. Here, Δn = 2 - 3 = -1, so Kp = Kc(0.0821T)^(-1). Assuming standard conditions, Kp = 4 * (1/RT) = 16.
Understanding "Physical Chemistry - Equilibrium" is crucial for students aiming to excel in their exams. This topic not only forms a significant part of the syllabus but also features prominently in various competitive exams. Practicing MCQs and objective questions related to equilibrium helps reinforce concepts and boosts confidence, ultimately leading to better scores in exams.
What You Will Practise Here
Concept of dynamic equilibrium and its characteristics
Le Chatelier's Principle and its applications
Equilibrium constant (K) expressions for various reactions
Factors affecting equilibrium: concentration, temperature, and pressure
Calculating equilibrium concentrations using ICE tables
Common equilibrium reactions and their significance
Graphical representation of equilibrium shifts
Exam Relevance
The topic of equilibrium is frequently tested in CBSE, State Boards, NEET, and JEE exams. Students can expect questions that require them to apply Le Chatelier's Principle, calculate equilibrium constants, or interpret data from equilibrium graphs. Common question patterns include multiple-choice questions (MCQs) that assess conceptual understanding and application of theories in real-world scenarios.
Common Mistakes Students Make
Confusing static and dynamic equilibrium
Misapplying Le Chatelier's Principle to predict shifts
Errors in calculating equilibrium constants from given concentrations
Overlooking the effects of temperature and pressure changes
Failing to properly set up ICE tables for equilibrium calculations
FAQs
Question: What is the significance of Le Chatelier's Principle in equilibrium? Answer: Le Chatelier's Principle helps predict how a system at equilibrium responds to changes in concentration, temperature, or pressure, guiding us in understanding reaction behavior.
Question: How can I effectively prepare for equilibrium questions in exams? Answer: Regular practice of MCQs and objective questions, along with a clear understanding of key concepts, will enhance your preparation and confidence.
Start solving practice MCQs on "Physical Chemistry - Equilibrium" today to test your understanding and improve your exam readiness. Remember, consistent practice is the key to success!
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