Le Châtelier’s Principle and Chemical Equilibrium

The video introduces Le Châtelier’s Principle, explaining how chemical reactions at equilibrium respond to disturbances. It covers the concept of dynamic equilibrium, the role of the equilibrium constant, and how changes in concentration, pressure, and temperature affect equilibrium. The Haber process is used as a practical example to illustrate these concepts. The video concludes by summarizing the importance of Le Châtelier’s Principle in both theoretical and practical chemistry.

What does the equilibrium constant, Keq, represent in a chemical reaction?

• The speed of the reaction

• The ratio of products to reactants at equilibrium

• The total energy of the system

• The amount of reactants converted to products

According to Le Châtelier’s Principle, what happens when a system at equilibrium is disturbed?

• The system remains unchanged

• The system shifts to counteract the disturbance

• The system speeds up the reaction

• The system stops reacting

In the context of Le Châtelier’s Principle, what is considered a disturbance?

• A change in the phase of the reactants

• A change in the color of the reactants

• A change in concentration, pressure, or temperature

• A change in the shape of the reaction vessel

What is the primary goal in the Haber process for ammonia production?

• To increase the temperature

• To produce as much ammonia as possible

• To maintain a constant volume

• To decrease the pressure

How does increasing pressure affect the Haber process according to Le Châtelier’s Principle?

• It shifts the equilibrium to produce more ammonia

• It increases the number of moles of gas

• It decreases the production of ammonia

• It has no effect on the equilibrium

Why is adjusting temperature not always straightforward in shifting equilibrium for exothermic reactions?

• It always speeds up the reaction

• It can slow down the reaction rate significantly

• It always increases the production of reactants

• It has no effect on the equilibrium

What is the effect of removing heat from an exothermic reaction at equilibrium?

• It shifts the equilibrium towards the reactants

• It shifts the equilibrium towards the products

• It increases the reaction rate

• It decreases the reaction rate

What is the significance of dynamic equilibrium in a chemical reaction?

• The forward and reverse reactions occur at the same rate

• The reaction stops completely

• The reaction only proceeds in one direction

• The concentration of reactants is always higher than products

How do chemists practically apply Le Châtelier’s Principle in industrial processes?

• By stopping the reaction at equilibrium

• By increasing the energy input

• By maintaining constant conditions

• By manipulating conditions to favor the desired product

What role does Gibbs free energy play in chemical equilibrium?

• It reflects the balance of enthalpy and entropy

• It indicates the color change in the reaction

• It determines the speed of the reaction

• It measures the total energy of the system