Le Chatelier's Principle and Equilibrium Constant

Flashcards about Le Chatelier's Principle and Equilibrium Constant

Reversible Reaction

A reaction where reactants form products, which can then react to reform the original reactants, represented by a double arrow.

Dynamic Equilibrium

The state where the forward and backward rates of a reversible reaction are the same and remain constant, resulting in constant concentrations of reactants and products in a closed system.

Le Chatelier’s Principle

When a system is subject to change, the system will alter to lessen the effect of that change.

Effect of Increasing Temperature (Le Chatelier's Principle)

Favors the endothermic reaction (+ve ∆H), increasing the yield of endothermic products.

Effect of Decreasing Temperature (Le Chatelier's Principle)

Favors the exothermic reaction (-ve ∆H), increasing the yield of exothermic products.

Effect of Increasing Pressure (Le Chatelier's Principle)

Favors the side of the reaction with fewer moles, increasing the yield of products on that side.

Effect of Decreasing Pressure (Le Chatelier's Principle)

Favors the side of the reaction with more moles, increasing the yield of products on that side.

Effect of Increasing Reactant Concentration (Le Chatelier's Principle)

Favors the reaction that produces the products, increasing the yield of products.

Effect of Catalysts (Le Chatelier's Principle)

Catalysts do not affect the equilibrium position, but they allow equilibrium to be reached faster.

Equilibrium Constant (Kc)

Indicates the position of equilibrium for a reversible reaction at a certain temperature; it is equal to the concentration of products divided by the concentration of reactants.

Factors Affecting Kc

Kc is affected by temperature change but not by concentration change or the use of a catalyst.