AP Chemistry--Equilibrium Basics

Front

What does a large equilibrium constant (Kc) indicate about a reaction?

Back

A large equilibrium constant (e.g., Kc = 1000) indicates that at equilibrium, the reaction favors the formation of products.

Front

How does increasing temperature affect an endothermic reaction at equilibrium?

Back

Increasing the temperature of an endothermic reaction shifts the equilibrium position to the right, favoring the formation of products.

Front

Given K = 1.2, [CO2] = 0.846M, and [CH4] = 0.0713M, how do you find [H2O]?

Back

Use the equilibrium expression to solve for [H2O]. In this case, [H2O] = 0.318 M.

Front

What effect does adding a catalyst have on a reaction at equilibrium?

Back

Adding a catalyst does not shift the equilibrium position; it only speeds up the rate at which equilibrium is reached.

Front

What is true for a system at equilibrium?

Back

At equilibrium, the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant.

Front

Define dynamic equilibrium in the context of chemical reactions.

Back

Dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of reactants and products.

Front

What is Le Chatelier's Principle?

Back

Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust to counteract the disturbance and restore a new equilibrium.

Front

How does decreasing the volume of a gaseous reaction at equilibrium affect the position of equilibrium?

Back

Decreasing the volume shifts the equilibrium position toward the side with fewer moles of gas.

Front

What is the significance of the equilibrium constant (K) in a chemical reaction?

Back

The equilibrium constant (K) quantifies the ratio of concentrations of products to reactants at equilibrium, indicating the extent of the reaction.

Front

Explain the effect of temperature on the equilibrium constant (K).

Back

The value of the equilibrium constant (K) changes with temperature; for exothermic reactions, increasing temperature decreases K, while for endothermic reactions, it increases K.