Le Chatelier's Principle

For the reversible reaction $A(g) + B(g) ightleftharpoons 2C(g)$, increasing the total pressure by adding an inert gas at constant volume will:

Consider an exothermic reaction at equilibrium. Which of the following actions will simultaneously shift the equilibrium towards the reactants and decrease the value of the equilibrium constant (K)?

For the reaction $2SO_2(g) + O_2(g) ightleftharpoons 2SO_3(g)$, ΔH < 0. Which change will NOT increase the production of $SO_3(g)$?

A reaction has an equilibrium constant K = 0.5 at 25°C. If the reaction is endothermic, what will happen to the value of K if the temperature is increased to 50°C?

Consider the equilibrium: $A(g) + B(s) ightleftharpoons C(g)$. Which of the following changes will shift the equilibrium to the right?

For the reaction $N_2(g) + 3H_2(g) ightleftharpoons 2NH_3(g)$ at equilibrium, what effect will decreasing the volume of the container have?

Which of the following statements is correct regarding the effect of a catalyst on a reversible reaction at equilibrium?

Which of the following scenarios will always shift the equilibrium towards the product side?

How does decreasing the temperature affect an endothermic reaction at equilibrium?

Consider a reaction in which Δn = 0 (no change in the number of moles of gas). Which of the following changes will affect the equilibrium?

In the Haber-Bosch process ($N_2 + 3H_2 ightleftharpoons 2NH_3$, ΔH < 0), which conditions favor the production of ammonia?

Which action will increase the value of the equilibrium constant (K) for an endothermic reaction?

For the equilibrium $2NO_2(g) ightleftharpoons N_2O_4(g)$, the reaction is exothermic. Predict the effect of increasing the temperature on the equilibrium.

Which of the following changes affects the value of the equilibrium constant (K)?

For the reaction $A(g) ightleftharpoons B(g) + C(g)$, increasing the pressure will:

Which of the following will increase the production of products in an exothermic reaction at equilibrium?

What effect does increasing the concentration of a reactant have on a system at equilibrium?

Which change will NOT affect the equilibrium position for the reaction $H_2(g) + I_2(g) ightleftharpoons 2HI(g)$?

Consider the reaction $CO(g) + 2H_2(g) ightleftharpoons CH_3OH(g)$. ΔH < 0. Which conditions will favor the production of $CH_3OH(g)$?

How does decreasing the pressure affect the equilibrium of a reaction in which there are more moles of gas on the product side than on the reactant side?

In the reaction $A(g) + B(g) ightleftharpoons C(g) + D(g)$, the forward reaction is endothermic. Which conditions will favor the formation of C and D?

If Q < K for a reversible reaction, what will happen?

Which of the following changes will decrease the value of K for an exothermic reaction?

For the reaction $N_2O_4(g) ightleftharpoons 2NO_2(g)$, the reaction is endothermic. What will happen if the temperature is decreased?

Adding an inert gas at constant pressure to a reaction at equilibrium will:

Which of the following correctly describes the effect of removing products from a system at equilibrium?

For the reversible reaction: $2A(g) + B(g) ightleftharpoons C(s) + D(g)$, which of the following actions would increase the amount of $C(s)$ at equilibrium?

How do changes in pressure typically affect reactions in solution?

Which of the following actions will not change the composition of an equilibrium mixture?

For an endothermic reaction, what happens to the equilibrium constant K as temperature decreases?

If a reversible reaction has Δn = 0, which of the following changes will alter the equilibrium composition?

The Contact process ($2SO_2(g) + O_2(g) ightleftharpoons 2SO_3(g)$) is exothermic. Which strategy will maximize $SO_3$ production?

How does Le Chatelier's principle apply to biological systems?

For a reaction with Q > K, which direction will the reaction proceed to reach equilibrium?

Which of the following is NOT a way to shift the equilibrium of a chemical reaction?

If a reaction is at equilibrium and more product is added, what happens to the reaction quotient, Q?

For a gas-phase reaction, increasing the volume of the container will shift the equilibrium in which direction?

In an endothermic reaction, if temperature decreases, what occurs to the equilibrium?