Equilibrium Constant and Its Applications

Chemistry ⇒ Chemical Kinetics and Equilibrium

Equilibrium Constant and Its Applications starts at 11 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Equilibrium Constant and Its Applications. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 12

A reaction has K_c = 1.5 × 10³ at 298 K. Is the reaction product-favored or reactant-favored at this temperature?

For the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), write the expression for K_p.

For the reaction H₂(g) + I₂(g) ⇌ 2HI(g), if K_c = 50 at 400°C, what is the value of K_c for the reaction 2HI(g) ⇌ H₂(g) + I₂(g) at the same temperature?

For the reaction: 2A(g) ⇌ B(g) + C(g), if K_c = 0.25 and at equilibrium [A] = 0.4 mol·dm^-3, [B] = [C] = 0.2 mol·dm^-3, verify if the system is at equilibrium.

For the reaction: 2A(g) ⇌ B(g) + C(g), if the initial concentration of A is 1.0 mol·dm^-3 and at equilibrium [A] = 0.6 mol·dm^-3, calculate the equilibrium concentrations of B and C.

For the reaction: 2HI(g) ⇌ H₂(g) + I₂(g), if K_c = 0.02 at 700 K, what is the value of K_c for the reaction: H₂(g) + I₂(g) ⇌ 2HI(g)?

For the reaction: 2NO₂(g) ⇌ N₂O₄(g), if the color intensity of the mixture decreases, what can you infer about the direction of the shift in equilibrium?

For the reaction: 2NO₂(g) ⇌ N₂O₄(g), K_c = 0.36 at 300 K. If [NO₂] = 0.5 mol·dm^-3 and [N₂O₄] = 0.09 mol·dm^-3, is the system at equilibrium?

For the reaction: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), if the volume of the container is halved, what happens to the equilibrium position?

For the reaction: A(g) + B(g) ⇌ C(g), if K_c = 10 and the initial concentrations are [A] = 1 mol·dm^-3, [B] = 1 mol·dm^-3, and [C] = 0 mol·dm^-3, calculate the equilibrium concentration of C.

For the reaction: CO(g) + 2H₂(g) ⇌ CH₃OH(g), write the K_c expression.

For the reaction: H₂(g) + Cl₂(g) ⇌ 2HCl(g), if the equilibrium concentrations are [H₂] = 0.2 mol·dm^-3, [Cl₂] = 0.2 mol·dm^-3, and [HCl] = 0.6 mol·dm^-3, calculate K_c.

For the reaction: N₂O₄(g) ⇌ 2NO₂(g), if the total pressure at equilibrium is increased, what happens to the concentration of NO₂?

For the reaction: PCl₅(g) ⇌ PCl₃(g) + Cl₂(g), if K_c = 0.04 at 300 K, what is the value of K_c for the reaction: PCl₃(g) + Cl₂(g) ⇌ PCl₅(g)?

If Q_c > K_c for a reaction mixture, in which direction will the reaction proceed to reach equilibrium?

If the equilibrium constant for a reaction is 1, what does it indicate about the concentrations of reactants and products at equilibrium?

If the equilibrium constant K_c for a reaction is very large, what does it indicate about the position of equilibrium?

If the value of K_c is much less than 1, what does it indicate about the reaction at equilibrium?

State Le Chatelier’s Principle.

The equilibrium constant for a reaction is 4.0 at 500 K. What will be the value of the equilibrium constant for the reverse reaction at the same temperature?