Equilibrium Reactions and Le Chatelier's Principle

The video tutorial explains Le Chatelier's Principle, which describes how a system at equilibrium responds to external stresses such as changes in concentration, pressure, volume, or temperature. It illustrates this principle through examples involving iron thiocyanate, iodine gas, and nitrogen dioxide equilibria, showing how these systems adjust to maintain equilibrium. The tutorial highlights the color changes that occur as a result of these adjustments, providing a visual understanding of the principle.

What does Le Chatelier's Principle suggest about a system at equilibrium when an external stress is applied?

• The system will remain unchanged.

• The system will adjust to completely eliminate the stress.

• The system will adjust to partially offset the stress.

• The system will become unstable.

In the Fe(SCN)2+ equilibrium system, what happens when the concentration of thiocyanate ions is increased?

• The solution becomes colorless.

• The red color of the solution deepens.

• The solution turns blue.

• The yellow color of the solution intensifies.

What is the effect of removing iron 3+ ions from the Fe(SCN)2+ equilibrium system?

• The solution becomes colorless.

• The solution turns yellow.

• The solution turns green.

• The red color of the solution deepens.

How does increasing the pressure affect the equilibrium between iodine gas molecules and iodine atoms?

• The system shifts to produce more iodine atoms.

• The system remains unchanged.

• The system shifts to produce more iodine molecules.

• The system becomes unstable.

What happens to the color of the iodine gas equilibrium mixture when the pressure is decreased?

• The color remains unchanged.

• The color turns green.

• The color lightens.

• The color darkens.

In the N2O4 and NO2 equilibrium, what is the effect of increasing the temperature?

• The system becomes unstable.

• The system remains unchanged.

• The system shifts to produce more NO2.

• The system shifts to produce more N2O4.

What is the color change observed when the temperature is increased in the N2O4 and NO2 equilibrium system?

• The color remains unchanged.

• The color turns blue.

• The color darkens.

• The color becomes lighter.

How does decreasing the temperature affect the N2O4 and NO2 equilibrium system?

• The system remains unchanged.

• The system becomes unstable.

• The system shifts to produce more N2O4.

• The system shifts to produce more NO2.

What is the effect on the color of the equilibrium mixture when the temperature is decreased in the N2O4 and NO2 system?

• The color darkens.

• The color remains unchanged.

• The color becomes lighter.

• The color turns green.

Which of the following statements is true about the endothermic reaction of N2O4 and NO2?

• Heat is considered a product.

• Heat is considered a reactant.

• The reaction does not involve heat.

• The reaction releases heat.