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 11

A reaction has K_c = 1.0 \times 10^{-5}. Which side is favored at equilibrium?

A reaction mixture contains 0.3\,\mathrm{M} A, 0.2\,\mathrm{M} B, and 0.5\,\mathrm{M} C at equilibrium for the reaction: A + 2B \rightleftharpoons C. Write the K_c expression and calculate its value.

Describe what happens to the equilibrium position if a product is removed from a system at equilibrium.

Describe what is meant by a dynamic equilibrium.

Describe what is meant by the term 'reaction quotient' (Q) and how it is used to predict the direction of a reaction.

Explain the difference between homogeneous and heterogeneous equilibrium.

Explain why changing the volume of a container affects the equilibrium position of a gaseous reaction.

Explain why solids and pure liquids are not included in the equilibrium constant expression.

Explain why the equilibrium constant has no units for some reactions but has units for others.

For the reaction 2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g), what will happen to the equilibrium position if the pressure is increased?

For the reaction: 2A(g) \rightleftharpoons B(g) + C(g), if the equilibrium mixture contains 0.2 mol/L of A, 0.1 mol/L of B, and 0.1 mol/L of C, calculate K_c.

For the reaction: 2A(g) \rightleftharpoons B(g) + C(g), if the initial concentration of A is 1.0 M and at equilibrium it is 0.6 M, calculate the equilibrium concentrations of B and C.

For the reaction: 2NO_2(g) \rightleftharpoons N_2O_4(g), if the volume of the container is halved, what happens to the equilibrium position?

For the reaction: 2NO_2(g) \rightleftharpoons N_2O_4(g), K_c = 4.0 at 25^\circ C. If [NO_2] = 0.2 M and [N_2O_4] = 0.1 M, is the system at equilibrium?

For the reaction: A(g) + B(g) \rightleftharpoons C(g), the equilibrium concentrations are [A] = 0.5 M, [B] = 0.5 M, and [C] = 1.0 M. Calculate K_c.

For the reaction: CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g), what will happen to the equilibrium position if the temperature is increased, given that the reaction is exothermic?

If a reaction is exothermic, what will be the effect of increasing temperature on the value of K_c?

If the concentration of a reactant is increased in a system at equilibrium, what will happen to the position of equilibrium?

If the value of K_c is much greater than 1, what does this indicate about the position of equilibrium?

State Le Chatelier's Principle.