#Le Chatelier's principle

Relationship Between Kp Kc and Factors Affecting Equilibrium - Le Chatelier

In the equilibrium 2A(g) + B(g) 3C(g) , increasing the concentration of A shifts the equilibrium towards which direction

Per Le Chatelier’s principle, increasing [A] shifts the equilibrium right to form more C and consume A .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Relationship Between Kp Kc and Factors Affecting Equilibrium - Le Chatelier

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Relationship Between Kp Kc and Factors Affecting Equilibrium - Le Chatelier

For the equilibrium X₂(g) 2X(g) , if the initial pressure of X₂ is 2 atm and at equilibrium the total pressure is 3 atm,

Let the pressure of X at equilibrium be 2p , X₂ = 2 - p , total pressure = (2 - p) + 2p = 2 + p = 3 , p = 1 . PX₂ = 1 atm , PX = 2 atm . Kp = ((PX)²/PX₂) = ((2)²/1) = 4 .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Relationship Between Kp Kc and Factors Affecting Equilibrium - Le Chatelier

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Relationship Between Kp Kc and Factors Affecting Equilibrium - Le Chatelier

In the equilibrium 2P(g) Q(g) + R(g) , adding Q at constant volume will shift the equilibrium in which direction?

According to Le Chatelier’s principle, adding Q increases its concentration, shifting the equilibrium left to reduce Q by forming more P .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Relationship Between Kp Kc and Factors Affecting Equilibrium - Le Chatelier

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Relationship Between Kp Kc and Factors Affecting Equilibrium - Le Chatelier

In the equilibrium N₂(g) + 3H₂(g) 2NH₃(g) , increasing the pressure shifts the equilibrium towards which direction?

According to Le Chatelier’s principle, increasing pressure favors the side with fewer moles of gas. Here, 4 moles (reactants) become 2 moles (products), so it shifts right.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Relationship Between Kp Kc and Factors Affecting Equilibrium - Le Chatelier

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Physical Equilibrium - Solid-Liquid Gas-Liquid and Henry's Law

In A(g) + 2B(g) 2C(g) , Kc = 4 and [A] = 0.1 M , [B] = 0.2 M , [C] = 0.4 M at equilibrium. What happens if temperature i

For an exothermic reaction, increasing temperature shifts equilibrium left, favoring reactants.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Physical Equilibrium - Solid-Liquid Gas-Liquid and Henry's Law

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Physical Equilibrium - Solid-Liquid Gas-Liquid and Henry's Law

In 2A(g) + B(g) 3C(g) , Kc = 9 and [A] = 0.3 M , [B] = 0.1 M , [C] = 0.9 M at equilibrium. What happens if volume is hal

Halving volume doubles concentrations: Q = ((1.8)³/(0.6)² (0.2)) = 81 > 9 , shifts left.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Physical Equilibrium - Solid-Liquid Gas-Liquid and Henry's Law

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Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant

What is the effect of adding an inert gas at constant volume to the equilibrium 2A(g) B(g) + C(g) ?

Adding an inert gas at constant volume does not change the partial pressures or concentrations of the reactants and products, so the equilibrium position remains unaffected.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant

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Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant

For 2A(g) + B(g) 3C(g) , Kp = 9 at 500 K. If PA = 0.5 atm , PB = 0.5 atm , and PC = 1.5 atm at equilibrium, what happens

Initial: Q = ((1.5)³/(0.5)² (0.5)) = 27 > Kp = 9 , doubling pressure increases concentrations, Q increases further, shifts left.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant

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Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant

In 2A(g) + B(g) 2C(g) , if Kc = 4 and the equilibrium mixture contains 0.2 mol A , 0.1 mol B , and 0.4 mol C in a 1 L ve

Initial equilibrium: [A] = 0.2 M , [B] = 0.1 M , [C] = 0.4 M , Kc = ((0.4)²/(0.2)²(0.1)) = 4 . After adding 0.1 mol A , [A] = 0.3 M , reaction shifts right to restore equilibrium.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant

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Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant

In the equilibrium 2XY(g) X₂(g) + Y₂(g) , decreasing the volume shifts the equilibrium in which direction?

Increasing pressure (decreasing volume) favors the side with fewer moles of gas. Here, 2 mol → 2 mol , so Δ n = 0 , and there is no shift.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant

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Chemical Equilibrium - Law of Mass Action and Equilibrium Constant

In A(g) + 2B(g) 2C(g) , Kc = 2 and [A] = 0.2 M , [B] = 0.4 M , [C] = 0.4 M at equilibrium. What happens if C is added?

Adding C increases Q , shifts left to reduce C .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Chemical Equilibrium - Law of Mass Action and Equilibrium Constant

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Chemical Equilibrium - Law of Mass Action and Equilibrium Constant

For 2X(g) Y(g) + Z(g) , if the volume is halved at constant temperature, the equilibrium shifts towards which direction?

Increasing pressure (halving volume) favors the side with fewer moles of gas. Here, 2 mol → 2 mol , Δ n = 0 , so there is no shift.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Chemical Equilibrium - Law of Mass Action and Equilibrium Constant

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