Unit 5 Review - Equilibrium and Le Chatelier's Principle

Front

What does a large equilibrium constant (Kc) indicate?

Back

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

Front

What happens to the equilibrium when heat is added to an endothermic reaction?

Back

When heat is added to an endothermic reaction, the equilibrium shifts to the right, favoring the formation of products.

Front

In a chemical equilibrium, what do [A] and [B] represent?

Back

In a chemical equilibrium, [A] and [B] represent the concentrations of reactants.

Front

What is the equilibrium constant expression for the reaction N2O4(g) ↔ 2 NO2(g)?

Back

The equilibrium constant expression is Kc = [NO2]^2 / [N2O4].

Front

What happens to the concentration of N2 when heat is removed from an endothermic reaction?

Back

When heat is removed from an endothermic reaction, the concentration of N2 will increase.

Front

Define Le Chatelier's Principle.

Back

Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium.

Front

What effect does increasing the concentration of reactants have on equilibrium?

Back

Increasing the concentration of reactants will shift the equilibrium to the right, favoring the formation of products.

Front

What is the effect of decreasing the pressure on a gaseous equilibrium with more moles of gas on one side?

Back

Decreasing the pressure will shift the equilibrium towards the side with more moles of gas.

Front

How does temperature affect an exothermic reaction at equilibrium?

Back

Increasing the temperature of an exothermic reaction will shift the equilibrium to the left, favoring the formation of reactants.

Front

What is the relationship between the equilibrium constant and the direction of a reaction?

Back

The value of the equilibrium constant (Kc) indicates the extent to which a reaction favors products or reactants at equilibrium.