Understanding Chemical Equilibrium

The video tutorial covers the concept of chemical equilibrium, focusing on reversible reactions where the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of reactants and products. It explains dynamic equilibrium using examples, such as car movement between two cities, and illustrates the concept with concentration profiles. The tutorial also delves into equilibrium constants (Kc and Kp), their calculations, and the law of mass action. Several practice problems are solved to reinforce understanding, including calculating equilibrium constants and adjusting reactions.

What happens to the concentrations of reactants and products at equilibrium?

• They fluctuate randomly.

• They increase continuously.

• They decrease continuously.

• They remain constant.

In the traffic analogy, what does the constant number of cars in each city represent in a chemical reaction?

• The concentration of reactants and products.

• The speed of the reaction.

• The rate of reaction.

• The temperature of the reaction.

What does a horizontal line in a concentration profile graph indicate?

• The reaction has stopped.

• The reaction is slowing down.

• The reaction is at equilibrium.

• The reaction is speeding up.

How is the equilibrium constant Kc expressed?

• As the sum of reactants and products.

• As the difference between reactants and products.

• As the ratio of products to reactants.

• As the product of reactants and products.

What is the relationship between Kc and Kp?

• Kc is always greater than Kp.

• Kp is always greater than Kc.

• Kc and Kp are equal.

• Kc and Kp are related through the ideal gas law.

How do you calculate the equilibrium constant Kc from concentrations?

• By multiplying the concentrations of reactants and products.

• By adding the concentrations of products and reactants.

• By subtracting the concentrations of reactants from products.

• By dividing the concentration of products by reactants.

What happens to the equilibrium constant if the reaction is reversed?

• It is squared.

• It is inverted.

• It is halved.

• It remains the same.

If the coefficients of a balanced reaction are doubled, how is the equilibrium constant affected?

• It remains unchanged.

• It is halved.

• It is squared.

• It is doubled.

What is the effect on the equilibrium constant when the reaction is divided by a factor of two?

• It remains unchanged.

• It is halved.

• It is squared.

• It is raised to the power of one-half.

What is the significance of the equilibrium constant being greater than 1?

• The reaction favors the formation of reactants.

• The reaction favors the formation of products.

• The reaction is at equilibrium.

• The reaction is not feasible.