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.

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A reaction has K_{c} = 1.5 \times 10^{3} at 298 K. Is the reaction product-favored or reactant-favored at this temperature?

For the reaction 2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g), write the expression for K_{p}.

For the reaction H_2(g) + I_2(g) \rightleftharpoons 2HI(g), if K_{c} = 50 at 400°C, what is the value of K_{c} for the reaction 2HI(g) \rightleftharpoons H_2(g) + I_2(g) at the same temperature?

For the reaction: 2A(g) \rightleftharpoons 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) \rightleftharpoons 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) \rightleftharpoons H_2(g) + I_2(g), if K_{c} = 0.02 at 700 K, what is the value of K_{c} for the reaction: H_2(g) + I_2(g) \rightleftharpoons 2HI(g)?

For the reaction: 2NO_2(g) \rightleftharpoons N_2O_4(g), if the color intensity of the mixture decreases, what can you infer about the direction of the shift in equilibrium?

For the reaction: 2NO_2(g) \rightleftharpoons N_2O_4(g), K_{c} = 0.36 at 300 K. If [NO_2] = 0.5 mol·dm^-3 and [N_2O_4] = 0.09 mol·dm^-3, is the system at equilibrium?

For the reaction: 2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g), if the volume of the container is halved, what happens to the equilibrium position?

For the reaction: A(g) + B(g) \rightleftharpoons 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) + 2H_2(g) \rightleftharpoons CH_3OH(g), write the K_{c} expression.

For the reaction: H_2(g) + Cl_2(g) \rightleftharpoons 2HCl(g), if the equilibrium concentrations are [H_2] = 0.2 mol·dm^-3, [Cl_2] = 0.2 mol·dm^-3, and [HCl] = 0.6 mol·dm^-3, calculate K_{c}.

For the reaction: N_2O_4(g) \rightleftharpoons 2NO_2(g), if the total pressure at equilibrium is increased, what happens to the concentration of NO_2?

For the reaction: PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g), if K_{c} = 0.04 at 300 K, what is the value of K_{c} for the reaction: PCl_3(g) + Cl_2(g) \rightleftharpoons PCl_5(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?