Equilibrium Class 11 MCQ Best 100 Question Answer

Q: What is dynamic equilibrium in a chemical reaction?

Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction, leading to no net change in the concentrations of reactants and products, though both reactions continue.

Q: How is the equilibrium constant (K) affected by temperature?

The value of the equilibrium constant changes with temperature. For endothermic reactions, an increase in temperature increases K, while for exothermic reactions, an increase in temperature decreases K.

Q: What does Le Chatelier’s Principle state?

Le Chatelier’s Principle states that if a system at equilibrium is disturbed by changing concentration, pressure, or temperature, the system will adjust to counteract the disturbance and restore a new equilibrium.

Q: How are Kp and Kc related for a gaseous reaction?

Kp and Kc are related by the equation: Kp = Kc × (RT)^Δn where Δn is the change in the number of moles of gas, R is the gas constant, and T is the temperature.

Q: What happens to a system at equilibrium if the pressure is increased?

Increasing pressure shifts the equilibrium towards the side with fewer moles of gas, according to Le Chatelier's Principle.

Question 1

Question 1: What role do chemical equilibria play in biological systems?

A. They maintain body temperatureB. They regulate oxygen transport through hemoglobinC. They prevent CO₂ productionD. They help with energy generation

Answer

B. Equilibria involving oxygen and hemoglobin are crucial for oxygen transport in the body. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 2

Question 2: Which molecule is responsible for oxygen transport in the human body through equilibria?

A. HemoglobinB. MyoglobinC. AlbuminD. Globulin

Answer

A. Hemoglobin binds with oxygen to facilitate its transport in the body. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 3

Question 3: Carbon monoxide is toxic because it forms a strong equilibrium with which of the following?

A. OxygenB. HemoglobinC. Red blood cellsD. White blood cells

Answer

B. Carbon monoxide forms a stronger equilibrium with hemoglobin than oxygen, leading to toxicity. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 4

Question 4: What best describes dynamic equilibrium in a chemical process?

A. Reactants are converted to products onlyB. Products and reactants are present in equal amountsC. Both forward and reverse reactions occur at the same rateD. No chemical reactions occur

Answer

C. In dynamic equilibrium, the rates of the forward and reverse reactions are equal. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 5

Question 5: What condition is necessary for a chemical system to reach equilibrium?

A. Open systemB. Closed systemC. High pressureD. Low temperature

Answer

B. A closed system is required for equilibrium to be established. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 6

Question 6: Which of the following is true for a system at equilibrium?

A. Concentration of reactants and products changes continuouslyB. The forward and reverse reactions have stoppedC. The rates of forward and reverse reactions are equalD. No products are formed

Answer

C. At equilibrium, the rates of the forward and reverse reactions are equal. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 7

Question 7: Dynamic equilibrium occurs when:

A. Reactants convert to products entirelyB. Both reactants and products are consumed at equal ratesC. Forward and reverse reactions occur at different ratesD. No further reaction occurs

Answer

B. Dynamic equilibrium is when both reactions proceed at equal rates. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 8

Question 8: The law of equilibrium states that:

A. The rate of forward reaction equals the rate of reverse reactionB. Products will always be more abundant than reactantsC. The equilibrium constant remains constant for all reactionsD. Reactants dominate products at equilibrium

Answer

A. The law of equilibrium states that the forward and reverse reaction rates are equal at equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 9

Question 9: Which expression correctly represents the equilibrium constant Kc?

A. [Products]/[Reactants]B. [Reactants]/[Products]C. [Products] + [Reactants]D. [Products] – [Reactants]

Answer

A. Kc is calculated as the concentration of products divided by the concentration of reactants. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 10

Question 10: For a gaseous reaction, the equilibrium constant Kp relates to:

A. Partial pressure of gasesB. Molar concentrationC. DensityD. Volume

Answer

A. Kp relates to the partial pressures of the gases involved. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 11

Question 11: The relationship between Kp and Kc is affected by:

A. Temperature onlyB. Pressure onlyC. The change in moles of gasD. Volume

Answer

C. The relationship between Kp and Kc is determined by the change in moles of gas in the reaction. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 12

Question 12: According to the Bronsted-Lowry concept, an acid is defined as a substance that:

A. Accepts protonsB. Donates protonsC. Donates electronsD. Accepts electrons

Answer

B. A Bronsted-Lowry acid is a proton donor. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 13

Question 13: Which of the following is a Lewis base?

A. NH₃B. HClC. CH₄D. H₂O

Answer

A. NH₃ donates an electron pair, making it a Lewis base. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 14

Question 14: Which factor does not affect the state of equilibrium?

A. TemperatureB. ConcentrationC. CatalystD. Pressure

Answer

C. A catalyst speeds up both reactions but does not affect the equilibrium state. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 15

Question 15: What is the primary function of a buffer solution?

A. To increase pH rapidlyB. To resist changes in pHC. To change the solubility of saltsD. To stabilize temperature

Answer

B. A buffer solution resists changes in pH. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 16

Question 16: The solubility product constant (Ksp) is used to describe the solubility of:

A. Strong acidsB. Ionic solidsC. Gaseous substancesD. Weak bases

Answer

B. Ksp applies to the solubility of ionic solids in water. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 17

Question 17: In buffer solutions, the pH is determined by:

A. The strong acid concentrationB. The weak acid and its conjugate base concentrationC. The amount of catalystD. The partial pressure of gases

Answer

B. The pH of a buffer solution is determined by the weak acid and its conjugate base concentration. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 18

Question 18: What is true about phase equilibrium in a closed system?

A. The rates of phase changes are unequalB. The number of molecules in each phase remains constantC. Temperature continues to changeD. Only solids are present

Answer

B. At equilibrium, the number of molecules in each phase remains constant. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 19

Question 19: At what temperature does ice and water coexist in equilibrium under atmospheric pressure?

A. 100°CB. 0°CC. 50°CD. 273°C

Answer

B. Ice and water coexist at 0°C under atmospheric pressure. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 20

Question 20: Which of the following describes a system at liquid-vapour equilibrium?

A. The liquid evaporates fullyB. Evaporation and condensation occur at the same rateC. The pressure decreases continuouslyD. No vapour is present

Answer

B. At equilibrium, the rate of evaporation equals the rate of condensation. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 21

Question 21: Which substance undergoes sublimation directly from solid to vapour in equilibrium?

A. WaterB. Carbon dioxideC. IodineD. Nitrogen

Answer

C. Iodine sublimes directly from solid to vapour in equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 22

Question 22: In a saturated solution, the rate of dissolution of a solid is:

A. Faster than crystallizationB. Slower than crystallizationC. Equal to crystallizationD. No crystallization occurs

Answer

C. In a saturated solution, the rate of dissolution equals the rate of crystallization. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 23

Question 23: Henry’s law relates to:

A. The solubility of solids in liquidsB. The solubility of gases in liquidsC. The rate of chemical reactionsD. The formation of ions in solution

Answer

B. Henry’s law describes the solubility of gases in liquids. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 24

Question 24: Which characteristic is common to all physical equilibria?

A. It occurs in open systemsB. The system temperature changes constantlyC. Opposing processes occur at the same rateD. Products dominate over reactants

Answer

C. In equilibrium, opposing processes occur at the same rate. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 25

Question 25: For a solid-liquid equilibrium, the melting point of a pure substance at 1 atm pressure is called the:

A. Boiling pointB. Freezing pointC. Sublimation pointD. Vaporization point

Answer

B. The freezing point is the temperature at which a solid and liquid are in equilibrium at 1 atm. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 26

Question 26: At equilibrium, what happens to the vapour pressure of a liquid?

A. It fluctuatesB. It decreasesC. It remains constantD. It increases continuously

Answer

C. At equilibrium, the vapour pressure of a liquid remains constant. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 27

Question 27: Which physical process is in equilibrium when dry ice sublimes to carbon dioxide gas in a closed container?

A. Solid-liquid equilibriumB. Liquid-vapour equilibriumC. Solid-vapour equilibriumD. Gaseous equilibrium

Answer

C. Solid-vapour equilibrium is observed when dry ice sublimes in a closed container. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 28

Question 28: The solubility of a gas in a liquid is directly proportional to:

A. Pressure of the gasB. Temperature of the gasC. Concentration of the solventD. Volume of the liquid

Answer

A. According to Henry’s law, the solubility of a gas in a liquid is proportional to the pressure of the gas. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 29

Question 29: For a physical process, equilibrium is possible only in a:

A. Closed system at a constant temperatureB. Open system with varying pressureC. Closed system with changing concentrationsD. None of the above

Answer

A. Equilibrium in physical processes occurs in a closed system at a constant temperature. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 30

Question 30: In solid-liquid equilibrium, the amount of solid and liquid remains constant because:

A. There is no movement of particlesB. The rate of transfer between solid and liquid is equalC. The system is closedD. The temperature keeps changing

Answer

B. At equilibrium, the rate of transfer between solid and liquid is equal, maintaining constant amounts. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 31

Question 31: In a solid-vapour equilibrium, the number of particles transitioning between phases:

A. Increases as temperature increasesB. Decreases as pressure increasesC. Remains constantD. Changes with concentration

Answer

C. In equilibrium, the number of particles transitioning between phases remains constant. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 32

Question 32: Which factor remains constant at equilibrium during the dissolution of a gas in a liquid?

A. VolumeB. SolubilityC. Vapour pressureD. Temperature

Answer

B. The solubility of a gas in a liquid remains constant at equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 33

Question 33: A system is in dynamic equilibrium when:

A. Both forward and reverse reactions stopB. The rates of forward and reverse reactions are equalC. Only products are formedD. Only reactants are present

Answer

B. Dynamic equilibrium occurs when the rates of forward and reverse reactions are equal. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 34

Question 34: In a reversible chemical reaction, which of the following is true at equilibrium?

A. The concentration of reactants continues to decreaseB. The concentration of products increasesC. There is no net change in the concentration of reactants and productsD. The forward reaction dominates

Answer

C. At equilibrium, the concentrations of reactants and products remain constant. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 35

Question 35: The Haber process for ammonia synthesis reaches equilibrium when:

A. All reactants are converted into ammoniaB. The forward and reverse reactions proceed at equal ratesC. Only nitrogen remainsD. Hydrogen is completely consumed

Answer

B. In the Haber process, equilibrium occurs when the forward and reverse reactions proceed at equal rates. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 36

Question 36: Which condition favors higher ammonia production in the Haber process?

A. High pressureB. Low pressureC. High temperatureD. No catalyst

Answer

A. High pressure favors the production of ammonia in the Haber process. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 37

Question 37: The dynamic nature of equilibrium can be demonstrated by:

A. Using isotopesB. Varying the temperature continuouslyC. Stopping the reaction halfwayD. Keeping only one reactant constant

Answer

A. Isotopes are used to demonstrate the dynamic nature of equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 38

Question 38: Which technique is commonly used to demonstrate dynamic equilibrium in chemical reactions?

A. Color change observationB. Isotopic labelingC. Pressure measurementD. Volume change observation

Answer

B. Isotopic labeling is used to demonstrate that both the forward and reverse reactions occur simultaneously in dynamic equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 39

Question 39: In a dynamic equilibrium demonstrated by isotopic labeling, what is observed?

A. No further reaction occursB. The reactants stop reactingC. Both forward and reverse reactions occur at equal ratesD. The products are completely formed

Answer

C. In a dynamic equilibrium, isotopic labeling shows that both forward and reverse reactions continue at equal rates. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 40

Question 40: Which statement best describes chemical equilibrium?

A. It occurs when reactants are completely converted into productsB. The rate of the forward reaction equals the rate of the reverse reactionC. No reactions occur after equilibrium is reachedD. The concentrations of reactants and products are equal

Answer

B. Chemical equilibrium occurs when the forward and reverse reaction rates are equal. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 41

Question 41: Which of the following is constant at equilibrium in a chemical reaction?

A. The concentrations of reactantsB. The concentrations of productsC. The rate of the forward and reverse reactionsD. The amount of reactants

Answer

C. The rate of both the forward and reverse reactions is constant at equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 42

Question 42: In a reaction where the equilibrium constant Kc is very large, what is true about the reaction?

A. The reaction proceeds nearly to completionB. The reaction hardly proceedsC. Reactants dominate the equilibrium mixtureD. Both reactants and products are present in equal amounts

Answer

A. A very large Kc indicates that the reaction proceeds nearly to completion, favoring the formation of products. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 43

Question 43: Which reaction would be classified as reactant-favored at equilibrium?

A. A reaction with Kc > 10³B. A reaction with Kc ≈ 1C. A reaction with Kc < 10⁻³D. A reaction with equal amounts of reactants and products

Answer

C. A reaction with a very small Kc (< 10⁻³) is classified as reactant-favored. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 44

Question 44: Which reaction is product-favored at equilibrium?

A. A reaction with Kc = 0B. A reaction with Kc = 1C. A reaction with Kc > 10³D. A reaction with Kc < 10⁻³

Answer

C. A reaction with Kc > 10³ is product-favored, meaning the equilibrium favors the formation of products. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 45

Question 45: When Kc is approximately equal to 1, what can be inferred about the reaction?

A. Only reactants are present at equilibriumB. Only products are present at equilibriumC. The amounts of reactants and products are comparableD. The reaction does not reach equilibrium

Answer

C. When Kc is approximately equal to 1, both reactants and products are present in comparable amounts at equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 46

Question 46: An equilibrium mixture contains:

A. Only reactantsB. Only productsC. Both reactants and products in constant amountsD. Reactants and products in varying amounts

Answer

C. An equilibrium mixture contains both reactants and products in constant amounts. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 47

Question 47: The law of mass action relates the rate of reaction to:

A. TemperatureB. PressureC. Concentrations of reactantsD. Concentrations of products

Answer

C. The law of mass action states that the rate of reaction is proportional to the concentration of reactants. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 48

Question 48: For the reaction A + B ⇌ C + D, the equilibrium constant Kc is expressed as:

A. [A][B]/[C][D]B. [C][D]/[A][B]C. [A]/[B][C]D. [C]/[D][A]

Answer

B. Kc is expressed as the concentration of products over the concentration of reactants. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 49

Question 49: In a reaction at equilibrium, if the concentration of reactants is increased, the reaction will shift towards:

A. ReactantsB. ProductsC. No shift occursD. Depends on temperature

Answer

B. According to Le Chatelier’s principle, increasing the concentration of reactants will shift the reaction towards products. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 50

Question 50: If a system in equilibrium is cooled, the equilibrium will shift:

A. To the reactantsB. To the productsC. Depends on whether the reaction is endothermic or exothermicD. There is no effect

Answer

C. Cooling affects equilibrium depending on whether the reaction is exothermic or endothermic. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 51

Question 51: The equilibrium constant for the reverse reaction is:

A. The square of the forward reaction constantB. Equal to the forward reaction constantC. The inverse of the forward reaction constantD. The same as the rate constant

Answer

C. The equilibrium constant for the reverse reaction is the inverse of that for the forward reaction. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 52

Question 52: If the stoichiometric coefficients in a balanced equation are doubled, the equilibrium constant Kc will be:

A. HalvedB. DoubledC. SquaredD. Unaffected

Answer

C. When stoichiometric coefficients are doubled, the equilibrium constant is squared. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 53

Question 53: In a homogeneous equilibrium, all the reactants and products are in the same:

A. PhaseB. ContainerC. ConcentrationD. Pressure

Answer

A. In a homogeneous equilibrium, all reactants and products are in the same phase. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 54

Question 54: Which of the following is an example of heterogeneous equilibrium?

A. 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)B. CaCO₃(s) ⇌ CaO(s) + CO₂(g)C. H₂(g) + I₂(g) ⇌ 2HI(g)D. N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

Answer

B. CaCO₃(s) ⇌ CaO(s) + CO₂(g) is an example of heterogeneous equilibrium, involving different phases. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 55

Question 55: Which of the following reactions involves homogeneous equilibrium?

A. Fe(s) + O₂(g) ⇌ Fe₂O₃(s)B. N₂(g) + 3H₂(g) ⇌ 2NH₃(g)C. CaCO₃(s) ⇌ CaO(s) + CO₂(g)D. H₂O(l) ⇌ H₂O(g)

Answer

B. N₂(g) + 3H₂(g) ⇌ 2NH₃(g) involves only gaseous species, thus homogeneous equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 56

Question 56: A large equilibrium constant (Kc > 1000) indicates that at equilibrium:

A. Products predominateB. Reactants predominateC. The reaction has not occurredD. The system is at rest

Answer

A. A large Kc indicates that products predominate at equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 57

Question 57: For a reaction with a very small Kc (Kc < 0.001), the reaction will favor:

A. Formation of reactantsB. Formation of productsC. Equal amounts of reactants and productsD. High temperature

Answer

A. A very small Kc indicates that the reaction favors the formation of reactants. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 58

Question 58: If Kc is approximately equal to 1, then at equilibrium:

A. Only reactants will be presentB. Only products will be presentC. Reactants and products will be present in comparable amountsD. The reaction will not occur

Answer

C. When Kc is close to 1, reactants and products are present in comparable amounts at equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 59

Question 59: To calculate equilibrium concentrations, you need to know:

A. The initial concentrations and the equilibrium constantB. The temperature and pressureC. The catalyst used in the reactionD. The speed of the reaction

Answer

A. The initial concentrations and the equilibrium constant are needed to calculate equilibrium concentrations. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 60

Question 60: The expression for Kc is derived from the:

A. Stoichiometric coefficients of the balanced equationB. Concentrations at equilibriumC. Initial concentrations of reactantsD. Temperature and pressure

Answer

A. The equilibrium constant expression is derived from the stoichiometric coefficients of the balanced equation. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 61

Question 61: Kp is used for reactions involving:

A. SolidsB. LiquidsC. GasesD. Aqueous solutions

Answer

C. Kp is used for reactions involving gases, where equilibrium is expressed in terms of partial pressures. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 62

Question 62: The ideal gas equation used to relate Kp to Kc is:

A. pV = nRTB. pV = TnRC. Vp = nTRD. R = pT/nV

Answer

A. The ideal gas equation pV = nRT relates pressure, volume, temperature, and moles. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 63

Question 63: Which of the following correctly expresses the relationship between Kp and Kc?

A. Kp = Kc × RTB. Kp = Kc × (RT)ⁿC. Kp = Kc / RTD. Kp = RT × Kc²

Answer

B. Kp = Kc × (RT)ⁿ, where ⁿ is the change in the number of moles of gas. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Question 64

Question 64: For which reaction would Kp and Kc be equal?

A. 2NO₂(g) ⇌ N₂O₄(g)B. H₂(g) + I₂(g) ⇌ 2HI(g)C. CaCO₃(s) ⇌ CaO(s) + CO₂(g)D. 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

Answer

B. Kp and Kc would be equal if the number of moles of gases in the products and reactants are the same. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. The equilibrium constant Kc changes with temperature. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. Increasing temperature for an exothermic reaction decreases the value of Kc. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. For endothermic reactions, increasing temperature increases Kc. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. Heterogeneous equilibria involve reactants and products in different phases. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. CaCO₃(s) ⇌ CaO(s) + CO₂(g) is an example of heterogeneous equilibrium, as it involves both solids and gases. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

C. In heterogeneous equilibrium, the equilibrium constant expression involves only the gas, so K = pCO₂. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

C. CaCO₃(s) ⇌ CaO(s) + CO₂(g) is a heterogeneous equilibrium involving both solids and gases. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. The concentrations of pure solids and liquids remain constant and are omitted from the equilibrium expression. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

C. Only pCO₂ (the partial pressure of CO₂) appears in the equilibrium constant expression, as solids are omitted. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. A large Kc value indicates that the reaction favors products. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. A small Kc indicates that the reactants predominate at equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. If Qc > Kc, the reaction will proceed in the reverse direction to reach equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. When Qc = Kc, the system is at equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. If Qc < Kc, the reaction will shift in the forward direction to reach equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. Le Chatelier’s principle states that a system at equilibrium will shift to counteract changes in temperature, concentration, or pressure. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. Adding a reactant will shift the reaction towards products to re-establish equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. Removing a product will shift the reaction towards products to replace what was removed. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. Increasing temperature in an endothermic reaction shifts the equilibrium towards products. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. Decreasing temperature in an exothermic reaction shifts the equilibrium towards products. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. Removing ammonia from the system will shift the equilibrium towards ammonia (products) to replace it. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

C. A negative ΔG indicates that the reaction is spontaneous in the forward direction. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. When ΔG = 0, the system is at equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. A positive ΔG indicates that the reaction is non-spontaneous. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

C. The equation ΔG = –RTlnK relates Gibbs free energy to the equilibrium constant. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

C. A very negative ΔG indicates a large value for K, meaning the reaction favors products. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

C. Le Chatelier’s principle helps predict the effect of changes in temperature, concentration, and pressure on equilibrium. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. Decreasing the concentration of a product will shift the reaction towards products. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. Increasing the concentration of a reactant shifts the reaction to the right towards products. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. Decreasing the volume increases pressure, shifting the equilibrium towards the side with fewer moles of gas. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

C. Removing ammonia will shift the equilibrium to the right to produce more ammonia. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. Le Chatelier’s principle is used to maximize product yield by altering temperature, pressure, or concentration. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. To calculate equilibrium concentrations, initial concentrations and the equilibrium constant are necessary. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

B. Kc = [NH₃

Accepted Answer

A. A small equilibrium constant indicates the reaction favors reactants. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Accepted Answer

A. Increasing the concentration of NO₂ will shift the equilibrium to the right to form more N₂O₄. (Equilibrium Class 11 MCQ by Top100MCQ.com)

Equilibrium Class 11 MCQ

Equilibrium Introduction (MCQ 1 to 6)

Importance of Chemical Equilibria in Biological and Environmental Processes

Examples of Equilibria in Systems like Hemoglobin and Oxygen, Carbon Monoxide Toxicity

Concept of Dynamic and Static Equilibrium

Reaching Equilibrium in Closed Systems

Learning Objectives (MCQ 7 to 17)

Identifying Dynamic Nature of Equilibrium

Law of Equilibrium

Writing Expressions for Kp and Kc

Relationship Between Kp and Kc

Classifying Acids and Bases (Arrhenius, Bronsted-Lowry, Lewis)

Factors Affecting Equilibrium State

Buffer Solutions and Solubility Product Constants

Equilibrium in Physical Processes (MCQ 18 to 32)

Phase Transformation and Equilibrium in Different States

Solid-Liquid Equilibrium

Liquid-Vapour Equilibrium

Solid-Vapour Equilibrium

Equilibrium Involving Dissolution of Solids and Gases in Liquids

Characteristics of Equilibrium in Physical Processes

Equilibrium in Chemical Processes (Dynamic Equilibrium) (MCQ 33 to 45)

Dynamic Equilibrium in Reversible Reactions

Example: Synthesis of Ammonia via the Haber Process

Demonstrating Dynamic Equilibrium with Isotopes

Demonstrating Dynamic Equilibrium with Isotopes

General Characteristics of Chemical Equilibrium

Classification of Reactions Based on the Extent of Equilibrium

Law of Chemical Equilibrium and Equilibrium Constant (MCQ 46 to 60)

Equilibrium Mixture and Factors Determining Equilibrium Composition

Law of Mass Action and Equilibrium Constant Expression (Kc)

Examples and Experiments Demonstrating Equilibrium Concentrations

Relationship Between Equilibrium Constants for Forward and Reverse Reactions

Effect of Changes in Stoichiometric Coefficients on Equilibrium Constants

Homogeneous vs. Heterogeneous Equilibria

Predicting Extent of Reactions Using Kc

Calculating Equilibrium Concentrations

Equilibrium Constant in Gaseous Systems (MCQ 61 to 67)

Expressing Equilibrium Constants in Terms of Partial Pressures (Kp)

Relationship Between Kc and Kp for Gaseous Reactions

Influence of Temperature on Kc and Kp

Heterogeneous Equilibria (MCQ 68 to 73)

Definition and Examples of Heterogeneous Equilibrium

Thermal Dissociation of Calcium Carbonate (CaCO₃)

Simplifying Equilibrium Expressions for Heterogeneous Reactions

Applications of Equilibrium Constants (MCQ 74 to 85)

Predicting the Extent of a Reaction Based on Kc or Kp

Calculating Equilibrium Concentrations and Predicting Reaction Direction (Qc vs. Kc)

Application of Le Chatelier’s Principle

Relationship Between Equilibrium Constant (K), Reaction Quotient (Q), and Gibbs Free Energy (G) (MCQ 86 to 90)

Relationship Between Gibbs Free Energy and Spontaneity of Reactions

Mathematical Expressions Linking Gibbs Energy and Equilibrium Constant

Factors Affecting Equilibrium (MCQ 91 to 96)

Le Chatelier’s Principle and Its Applications

Effects of Changes in Concentration, Pressure, and Temperature on Equilibrium