Equilibrium Shifts in Chemical Reactions

The video tutorial by MSJ Chem explains Le Chatelier's Principle, focusing on how changes in concentration, pressure, and the addition of catalysts affect chemical equilibrium. It details the effects of these changes on the equilibrium position and the constant KC, using examples like the reaction of hydrogen and iodine, and the Haber process. The tutorial concludes with a summary of how these changes influence equilibrium without altering the KC value.

What is the primary focus of Le Chatelier's Principle?

• To predict the speed of a reaction

• To understand how a system at equilibrium responds to changes

• To calculate the energy change in a reaction

• To determine the equilibrium constant

When hydrogen gas is added to a system at equilibrium, what happens to the equilibrium position?

• It shifts to the right

• It causes the reaction to stop

• It remains unchanged

• It shifts to the left

How does adding hydrogen iodide to a system at equilibrium affect the equilibrium position?

• The equilibrium shifts to the left

• The equilibrium shifts to the right

• The equilibrium remains unchanged

• The reaction rate increases

In the Haber process, what happens to the equilibrium when pressure is increased?

• The equilibrium remains unchanged

• The reaction stops

• The equilibrium shifts to the left

• The equilibrium shifts to the right

What is the effect on ammonia yield when the equilibrium shifts to the right in the Haber process?

• The yield decreases

• The yield remains the same

• The yield becomes zero

• The yield increases

What happens to the equilibrium position when pressure is decreased in a gaseous reaction?

• It shifts to the side with fewer gaseous molecules

• It shifts to the side with more gaseous molecules

• It remains unchanged

• It causes the reaction to stop

How does a change in concentration affect the value of KC?

• It doubles the value of KC

• It has no effect on the value of KC

• It decreases the value of KC

• It increases the value of KC

What is the effect of decreasing the concentration of reactants on the equilibrium position?

• The equilibrium shifts to the right

• The equilibrium shifts to the left

• The equilibrium remains unchanged

• The reaction stops

When pressure is increased in a reaction with equal moles of gaseous reactants and products, what happens to the equilibrium?

• It causes the reaction to stop

• It remains unchanged

• It shifts to the left

• It shifts to the right

What is the effect of decreasing the concentration of products on the equilibrium position?

• The reaction stops

• The equilibrium remains unchanged

• The equilibrium shifts to the left

• The equilibrium shifts to the right