Equilibrium in Reversible Reactions

The video tutorial covers the concept of equilibrium in chemistry, focusing on reversible reactions and how equilibrium can be shifted using Le Chatelier's principle. It explains the effects of temperature, pressure, and concentration on equilibrium, providing real-life examples to illustrate these concepts. The tutorial aims to help students understand how different factors influence chemical reactions and how to predict the direction of equilibrium shifts.

What is a reversible reaction?

• A reaction that requires a catalyst

• A reaction where products can reform reactants

• A reaction that only proceeds in one direction

• A reaction that occurs only at high temperatures

In a reversible reaction, if the forward reaction is exothermic, what is true about the backward reaction?

• It releases more energy than the forward reaction

• It has no energy change

• It is endothermic

• It is also exothermic

What defines equilibrium in a reversible reaction?

• When the temperature of the system is constant

• When the reaction stops completely

• When the concentration of reactants is higher than products

• When the rate of the forward reaction equals the rate of the backward reaction

What happens to the concentrations of reactants and products at equilibrium?

• They both decrease

• They remain constant

• They both increase

• They continue to change

How can the position of equilibrium be shifted?

• By changing the color of the reactants

• By altering the conditions such as temperature or pressure

• By adding more catalysts

• By increasing the volume of the container

According to Le Chatelier's principle, what happens if the temperature of an exothermic reaction is increased?

• The reaction stops

• The equilibrium shifts to the left

• The equilibrium shifts to the right

• The equilibrium remains unchanged

What effect does increasing pressure have on a reaction with more gas molecules on the reactant side?

• Equilibrium shifts to the reactant side

• Equilibrium remains unchanged

• Equilibrium shifts to the side with more molecules

• Equilibrium shifts to the side with fewer molecules

How does decreasing the concentration of a reactant affect the equilibrium?

• Equilibrium shifts to the side with more products

• Equilibrium remains unchanged

• Equilibrium shifts to the left

• Equilibrium shifts to the right

What happens to the equilibrium if the concentration of a product is increased?

• Equilibrium shifts to the right

• Equilibrium shifts to the left

• Equilibrium shifts to the side with more reactants

• Equilibrium remains unchanged

Which factor does NOT affect the position of equilibrium?

• Temperature

• Pressure

• Concentration

• Color of the reactants