Chemical Equilibrium

Chemistry ⇒ Chemical Kinetics and Equilibrium

Chemical Equilibrium starts at 10 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Chemical Equilibrium. 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

Calculate the value of K_c for the reaction: A(g) + B(g) ⇌ C(g), if at equilibrium [A] = 0.2 M, [B] = 0.3 M, and [C] = 0.6 M.

Describe the effect of decreasing temperature on the equilibrium position of an endothermic reaction.

Describe what happens to the equilibrium position when an inert gas is added to a reaction mixture at constant volume.

Explain the difference between K_c and K_p.

Explain why changing the concentration of a solid reactant does not affect the position of equilibrium.

For the reaction: 2A(g) ⇌ B(g) + C(g), the equilibrium concentrations are [A] = 0.5 M, [B] = 0.2 M, [C] = 0.2 M. Calculate K_c.

For the reaction: 2NO₂(g) ⇌ N₂O₄(g), what is the effect of decreasing the volume of the container?

For the reaction: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), what will happen to the equilibrium position if the pressure is increased?

For the reaction: H₂(g) + Cl₂(g) ⇌ 2HCl(g), what is the effect of increasing the temperature if the reaction is exothermic?

For the reaction: H₂(g) + I₂(g) ⇌ 2HI(g), if the concentration of HI is increased, what will happen to the equilibrium position?

Given the reaction: CO(g) + 2H₂(g) ⇌ CH₃OH(g), if the system is at equilibrium and more CO is added, what will happen to the concentration of CH₃OH?

State Le Chatelier's Principle.

The value of K_p for a reaction is 0.001 at 500 K. Is the reaction product-favored or reactant-favored at this temperature?

Write the equilibrium constant expression for the reaction: 2A(g) + B(g) ⇌ 3C(g).

Write the general form of the equilibrium constant expression for the reaction: aA + bB ⇌ cC + dD.

A reaction mixture initially contains 1.0 mol of A and 2.0 mol of B in a 1.0 L vessel. The reaction A(g) + 2B(g) ⇌ 3C(g) reaches equilibrium at 400 K, and the equilibrium concentration of C is found to be 1.5 M. Calculate the equilibrium concentrations of A and B.

Consider the reaction: 2HI(g) ⇌ H₂(g) + I₂(g). If the equilibrium mixture is compressed at constant temperature, what will be the effect on the concentrations of HI, H₂, and I₂?

Describe how the equilibrium constant expression changes if the coefficients of a balanced chemical equation are all multiplied by 2.

Explain why the addition of a common ion decreases the solubility of a sparingly soluble salt.

For the reaction: 2A(g) ⇌ B(g) + C(g), the equilibrium constant K_c is 4.0 at 500 K. If the initial concentrations are [A] = 1.0 M, [B] = 0 M, and [C] = 0 M, calculate the equilibrium concentrations of all species.