Chemical Equilibrium Concepts and Effects

The video explores dynamic chemical equilibrium, explaining that not all reactions proceed from reactants to products. It introduces the reaction quotient (Qc) and equilibrium constant (Kc) to analyze equilibrium status. Le Chatelier's Principle is discussed, detailing how systems respond to changes in concentration, pressure, and temperature. The video also covers the impact of catalysts and inert gases, emphasizing that they do not alter equilibrium but can speed up the process.

What is a dynamic chemical equilibrium?

• A state where products are completely converted to reactants.

• A state where reactants are completely converted to products.

• A state where the forward and reverse reactions occur at the same rate.

• A state where no reactions occur.

How is the reaction quotient (Qc) used in relation to the equilibrium constant (Kc)?

• To predict the direction in which a reaction will proceed to reach equilibrium.

• To determine the speed of a reaction.

• To compare the concentrations of reactants and products at equilibrium.

• To measure the temperature of a reaction.

What happens if Qc is greater than Kc?

• The reaction will stop.

• The system is at equilibrium.

• The reaction will shift to the right to form more products.

• The reaction will shift to the left to form more reactants.

According to Le Chatelier's Principle, what happens when more reactant is added to a system at equilibrium?

• The system remains unchanged.

• The system shifts to the right, forming more products.

• The system shifts to the left, forming more reactants.

• The system stops reacting.

How does an increase in temperature affect an exothermic reaction at equilibrium?

• It has no effect on the equilibrium.

• It shifts the equilibrium to the left.

• It shifts the equilibrium to the right.

• It stops the reaction.

In an endothermic reaction, what is the effect of decreasing the temperature?

• The reaction stops.

• The equilibrium remains unchanged.

• The equilibrium shifts to the left.

• The equilibrium shifts to the right.

What is the effect of increasing the volume of a container on a gaseous equilibrium system?

• The system stops reacting.

• The pressure remains constant and the system does not shift.

• The pressure decreases and the system shifts to the side with more gas molecules.

• The pressure increases and the system shifts to the side with fewer gas molecules.

How does adding an inert gas affect a system at equilibrium?

• It increases the pressure and shifts the equilibrium.

• It decreases the pressure and shifts the equilibrium.

• It does not affect the equilibrium.

• It stops the reaction.

What role does a catalyst play in a reaction at equilibrium?

• It shifts the equilibrium to the right.

• It shifts the equilibrium to the left.

• It speeds up the attainment of equilibrium without shifting it.

• It stops the reaction.

What is the relationship between pressure and volume in a gaseous equilibrium system?

• Pressure is always constant regardless of volume changes.

• No relationship: volume and pressure are independent.

• Inverse relationship: as volume increases, pressure decreases.

• Direct relationship: as volume increases, pressure increases.