Le Chatelier's Principle and Reaction Equilibrium

The video tutorial explains Le Chatelier's Principle, focusing on how equilibrium shifts in response to changes in volume and pressure. It uses a hypothetical reaction to illustrate these concepts, calculating the reaction quotient to determine equilibrium status. The tutorial also covers the synthesis of ammonia and the effects of adding inert gases, emphasizing that equilibrium is not affected by inert gases. The video concludes with a discussion on reactions with equal moles of gas on both sides, showing that volume changes do not affect equilibrium in such cases.

What does Le Chatelier's Principle predict when a stress is applied to a system at equilibrium?

• The system will speed up the reaction.

• The system will remain unchanged.

• The system will slow down the reaction.

• The system will shift to counteract the stress.

In the hypothetical reaction, what happens to the pressure when the volume of the container is decreased?

• The pressure increases.

• The pressure remains the same.

• The pressure decreases.

• The pressure fluctuates.

When the net reaction moves to the left, what happens to the amount of gas C?

• It doubles.

• It remains constant.

• It decreases.

• It increases.

How is the reaction quotient (Qc) calculated for the hypothetical reaction?

• By using the concentration of solids.

• By using the temperature.

• By using the concentration of gases only.

• By using the total pressure.

What does it mean when Qc is greater than Kc?

• The reaction is moving to the right.

• There are too many products.

• There are too many reactants.

• The reaction is at equilibrium.

In the synthesis of ammonia, what happens when the volume is decreased?

• The reaction remains unchanged.

• The reaction stops.

• The reaction shifts to the right.

• The reaction shifts to the left.

What is the effect of increasing the volume on the equilibrium of the ammonia synthesis reaction?

• It increases the pressure and shifts the reaction to the right.

• It decreases the pressure and shifts the reaction to the left.

• It has no effect on the reaction.

• It stops the reaction.

What happens when there are equal moles of gas on both sides of a reaction and the volume is changed?

• The reaction stops.

• There is no effect on the equilibrium.

• The reaction shifts to the left.

• The reaction shifts to the right.

What is the effect of adding an inert gas like helium to a reaction at equilibrium?

• It increases the reaction rate.

• It shifts the reaction to the left.

• It shifts the reaction to the right.

• It has no effect on the equilibrium.

Why does adding an inert gas not affect the equilibrium of a reaction?

• Because it does not change the concentration of any species involved in the reaction.

• Because it reacts with the reactants.

• Because it changes the concentration of products.

• Because it changes the concentration of reactants.