Understanding Le Chatelier's Principle

The video tutorial explains Le Chatelier's Principle, focusing on how changes in concentration, pressure, and temperature affect chemical equilibrium. It provides examples and personal tricks to understand the principle better, emphasizing that equilibrium will shift to counteract changes. The role of catalysts is also discussed, highlighting that they speed up reactions without affecting equilibrium positions.

What is the condition for a reaction to be in chemical equilibrium?

• The pressure of the system is constant.

• The temperature of the system is constant.

• The rate of the forward reaction is equal to the rate of the backward reaction.

• The concentration of reactants is higher than products.

Which of the following is NOT a method to disturb chemical equilibrium?

• Changing the concentration of reactants or products.

• Changing the temperature of the system.

• Changing the color of the reactants.

• Changing the pressure of the system.

According to Le Chatelier's Principle, what happens when the concentration of a reactant is increased?

• The equilibrium remains unchanged.

• The equilibrium shifts to decrease the temperature.

• The equilibrium shifts to produce more reactants.

• The equilibrium shifts to produce more products.

What is the effect of decreasing the concentration of a product in a reaction at equilibrium?

• The equilibrium remains unchanged.

• The equilibrium shifts to produce more reactants.

• The equilibrium shifts to increase the pressure.

• The equilibrium shifts to produce more products.

How does increasing pressure affect a gaseous equilibrium reaction with more moles of products than reactants?

• The equilibrium shifts to produce more reactants.

• The equilibrium shifts to produce more products.

• The equilibrium shifts to decrease the temperature.

• The equilibrium remains unchanged.

What happens to the equilibrium position when pressure is decreased in a reaction with equal moles of reactants and products?

• The equilibrium shifts to produce more reactants.

• The equilibrium remains unchanged.

• The equilibrium shifts to produce more products.

• The equilibrium shifts to increase the temperature.

In an endothermic reaction, what is the effect of decreasing the temperature?

• The equilibrium shifts to produce more reactants.

• The equilibrium shifts to produce more products.

• The equilibrium remains unchanged.

• The equilibrium shifts to increase the pressure.

What is the effect of increasing temperature on an exothermic reaction at equilibrium?

• The equilibrium shifts to produce more products.

• The equilibrium shifts to produce more reactants.

• The equilibrium remains unchanged.

• The equilibrium shifts to decrease the pressure.

Why does adding a catalyst not affect the position of equilibrium?

• It changes the concentration of reactants.

• It only speeds up the backward reaction.

• It speeds up both forward and backward reactions equally.

• It only speeds up the forward reaction.

Which of the following statements is true about Le Chatelier's Principle?

• It only applies to irreversible reactions.

• It is not affected by changes in pressure.

• It predicts the direction of equilibrium shift when conditions change.

• It only applies to reactions in liquid state.