#reaction

Preparation and Properties of Potassium Dichromate and Permanganate

What happens when K 2 Cr 2 O 7 is treated with an alkali?

Dichromate (Cr 2 O 7 2− ) converts to chromate (CrO 4 2− ) in alkaline medium: Cr 2 O 7 2− + 2OH − → 2CrO 4 2− + H 2 O. The solution turns yellow due to chromate formation.

Ref: NCERT Class 12 Chemistry > Chapter 4: d and f Block Elements > Topic: Preparation and Properties of Potassium Dichromate and Permanganate

View Details

Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant

For the reaction 2A(g) + 2B(g) 3C(g) , Kc = 64 at 500 K. If 2 moles of A and 2 moles of B are placed in a 1 L vessel, wh

Initial: [A] = 2 M , [B] = 2 M , [C] = 0 . Let 3x be moles of C formed, so A and B decrease by 2x . At equilibrium: [A] = 2 - 2x , [B] = 2 - 2x , [C] = 3x . Kc = ([C]³/[A]²[B]²) = ((3x)³/(2 - 2x)² (2 - 2x)²) = (27x³/(2 - 2x)⁴) = 64 , (27x³/(2 - 2x)⁴) = 64 , (3x/2 - 2x) = 4 , 3x = 8 - 8x , 11x = 8 , x ≈ 0.727 , [C] = 3 × 0.727 ≈ 2.18 M .

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

View Details

Homogeneous and Heterogeneous Equilibria and Applications of Equilibrium Constant

For 2A(g) B(g) + C(g) , Kc = 0.0625 at 300 K. If 0.8 mol A is placed in a 2 L vessel with 0.1 mol B , what is [C] at equ

Initial: [A] = (0.8/2) = 0.4 M , [B] = (0.1/2) = 0.05 M , [C] = 0 . Let x = [C] , [A] = 0.4 - 2x , [B] = 0.05 + x . Kc = ([B][C]/[A]²) = ((0.05 + x)x/(0.4 - 2x)²) = 0.0625 . Solving, (0.05 + x)x = 0.0625 (0.4 - 2x)² , test x = 0.05 : (0.05 + 0.05) × 0.05 = 0.005 , 0.0625 × (0.4 - 0.1)² = 0.005625 (close), x ≈ 0.05 M .

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

View Details

Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For the equilibrium 2NO(g) N₂(g) + O₂(g) , if Kc = 4 and initial concentration of NO is 0.4 M with no products, what is

Let [N₂] = [O₂] = x , [NO] = 0.4 - 2x . Kc = ([N₂][O₂]/[NO]²) = (x²/(0.4 - 2x)²) = 4 . Taking square root, (x/0.4 - 2x) = 2 , x = 0.8 - 4x , 5x = 0.8 , x = 0.16 M .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

View Details

Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For the reaction X(g) + Y(g) 2Z(g) , if Kc = 25 and at equilibrium [Z] = 0.5 M , what is [X] if [Y] = 0.02 M ?

Kc = ([Z]²/[X][Y]) = 25 . Substituting, 25 = ((0.5)²/[X](0.02)) = (0.25/0.02 [X]) , 25 × 0.02 [X] = 0.25 , 0.5 [X] = 0.25 , [X] = 0.5 M .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

View Details

Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For the equilibrium CO(g) + H₂O(g) CO₂(g) + H₂(g) , if the initial concentrations of CO and H₂O are 0.2 M each and at eq

At equilibrium, [CO] = [H₂O] = 0.2 - 0.08 = 0.12 M , [CO₂] = [H₂] = 0.08 M . Thus, Kc = ([CO₂][H₂]/[CO][H₂O]) = ((0.08)²/(0.12)²) = (0.0064/0.0144) ≈ 0.444 .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

View Details

Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For 2A(g) B(g) + C(g) , Kc = 0.04 at 300 K. If 0.8 mol A is in a 2 L vessel, what is [B] at equilibrium?

Initial: [A] = 0.4 M , [B] = [C] = 0 . Let x = [B] = [C] , [A] = 0.4 - 2x . Kc = ([B][C]/[A]²) = (x²/(0.4 - 2x)²) = 0.04 , (x/0.4 - 2x) = 0.2 , x = 0.08 - 0.4x , x ≈ 0.057 M .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

View Details

Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For 2A(g) B(g) , Kc = 0.04 at 300 K. If 0.5 mol A is in a 1 L vessel, what is [B] at equilibrium?

Initial: [A] = 0.5 M , [B] = 0 . Let x = [B] , [A] = 0.5 - 2x . Kc = ([B]/[A]²) = (x/(0.5 - 2x)²) = 0.04 , x = 0.04 (0.5 - 2x)² , sqrtx = 0.2 (0.5 - 2x) , x ≈ 0.04 M .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

View Details

Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For the reaction 2A(g) B(g) + C(g) , if Kc = 0.25 and at equilibrium [B] = 0.1 M , [C] = 0.1 M , what is [A] ?

Kc = ([B][C]/[A]²) = 0.25 . Substituting, 0.25 = ((0.1)(0.1)/[A]²) = (0.01/[A]²) , [A]² = (0.01/0.25) = 0.04 , [A] = 0.2 M .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

View Details