Chemical Equilibrium Concepts and Effects

The video tutorial explains how dynamic equilibrium shifts in response to changes in concentration, pressure, and temperature. It covers the principles of Le Chatelier and the role of catalysts, emphasizing how these factors affect the position of equilibrium. The tutorial provides detailed explanations and examples to help viewers understand the concepts and apply them in exam scenarios.

What happens to the equilibrium position when the concentration of a reactant is increased?

• It shifts to the side with fewer moles.

• It remains unchanged.

• It shifts to the right to use up the extra reactant.

• It shifts to the left to increase reactants.

If the concentration of a product is decreased, what is the expected shift in equilibrium?

• Shifts to the side with more moles.

• Shifts to the left to increase reactants.

• Shifts to the right to produce more products.

• Remains unchanged.

How does an increase in pressure affect the equilibrium position in a gaseous reaction?

• Shifts to the side with more moles.

• Shifts to the side with equal moles.

• Shifts to the side with fewer moles.

• Remains unchanged.

What is the effect of decreasing pressure on the equilibrium position?

• Shifts to the side with more moles.

• Shifts to the side with fewer moles.

• Remains unchanged.

• Shifts to the side with equal moles.

In the context of equilibrium, what does a decrease in volume imply?

• Increase in temperature.

• Decrease in pressure.

• Increase in pressure.

• No change in pressure.

When temperature is increased, in which direction does the equilibrium shift?

• Towards the exothermic direction.

• Towards the endothermic direction.

• Remains unchanged.

• Towards the side with more moles.

What happens to the equilibrium position when the temperature is decreased?

• Shifts towards the exothermic direction.

• Shifts towards the endothermic direction.

• Shifts towards the side with fewer moles.

• Remains unchanged.

What is the role of a catalyst in a chemical equilibrium?

• Decreases the rate of reaction.

• Shifts the equilibrium to the right.

• Speeds up the attainment of equilibrium without shifting it.

• Shifts the equilibrium to the left.

How does a catalyst affect the rates of the forward and backward reactions?

• Increases the rate of the forward reaction only.

• Decreases the rates of both reactions.

• Increases the rate of the backward reaction only.

• Increases the rates of both reactions equally.

Which statement is true about catalysts in equilibrium reactions?

• They change the position of equilibrium.

• They have no effect on the rate of attainment.

• They decrease the time taken to reach equilibrium.

• They increase the concentration of products.