Le Chatelier's Principle and Equilibrium

This video tutorial covers Le Chatelier's Principle, explaining how systems at equilibrium respond to changes in concentration, temperature, and pressure. It discusses the mathematical and conceptual approaches to understanding these shifts, including the effects of adding or removing substances, changing temperature, and altering volume. The video also explores the impact of noble gases on equilibrium, emphasizing the independence of partial pressures.

What is the main idea behind Le Chatelier's Principle?

• A system at equilibrium will always shift to the right.

• A system at equilibrium will always shift to the left.

• A system at equilibrium will adjust to counteract any applied stress.

• A system at equilibrium will remain unchanged regardless of external stress.

If SO2 is removed from a system at equilibrium, what will happen?

• The system will shift to the left to produce more reactants.

• The system will shift to the right to produce more products.

• The system will remain unchanged.

• The system will produce more SO2.

What happens when O2 is added to a system at equilibrium?

• The system remains unchanged.

• The system shifts to the right to produce more O2.

• The system produces more reactants.

• The system shifts to the left to consume excess O2.

How does adding HCl affect a system at equilibrium?

• It has no effect on the equilibrium.

• It removes OH- ions, causing the system to shift right.

• It decreases the concentration of H+ ions.

• It increases the concentration of OH- ions.

What is the result of increasing temperature in an endothermic reaction at equilibrium?

• The reaction produces less heat.

• The reaction remains unchanged.

• The reaction shifts to the right.

• The reaction shifts to the left.

In an exothermic reaction, what happens when the temperature is increased?

• The reaction shifts to the right.

• The reaction produces more heat.

• The reaction remains unchanged.

• The reaction shifts to the left.

How does reducing the volume of a system affect the equilibrium?

• It shifts towards the side with more moles of gas.

• It shifts towards the side with fewer moles of gas.

• It has no effect on the equilibrium.

• It increases the pressure without shifting the equilibrium.

What is the effect of adding a noble gas to a system at equilibrium?

• It increases the pressure of the system.

• It decreases the pressure of the system.

• It has no effect on the equilibrium.

• It shifts the equilibrium to the right.

When the volume of a system is reduced, which side is favored?

• The side with equal moles of gas.

• Neither side is favored.

• The side with fewer moles of gas.

• The side with more moles of gas.

If a system has equal moles of gas on both sides, what happens when the volume is reduced?

• The system produces more gas.

• The system remains unchanged.

• The system shifts to the right.

• The system shifts to the left.