Equilibrium Constant (Kc)

The video tutorial explains the concept of equilibrium constants in reversible reactions, highlighting the inverse relationship between forward and backward reactions. It uses Haber's process for ammonia synthesis as an example, demonstrating how the equilibrium constant changes when the reaction is reversed. The tutorial also explores the effect of multiplying a reaction by a factor on the equilibrium constant, showing that the new constant is the original raised to the power of the factor. Finally, it discusses the impact of changing stoichiometric coefficients on equilibrium, concluding that the equilibrium constant is affected by the power of the change factor.

What is the relationship between the equilibrium constants of a forward and reverse reaction?

• They are both zero.

• They are unrelated.

• They are inverses of each other.

• They are equal.

In Haber's process, if the equilibrium constant for the forward reaction is 3 x 10^8, what is the equilibrium constant for the reverse reaction?

• 1 / 9 x 10^16

• 1 / (3 x 10^8)

• 9 x 10^16

• 3 x 10^8

How does multiplying a reaction by a factor affect its equilibrium constant?

• The equilibrium constant remains unchanged.

• The equilibrium constant is raised to the power of the factor.

• The equilibrium constant is multiplied by the same factor.

• The equilibrium constant is divided by the factor.

If a reaction is multiplied by a factor of 0.5, how is the new equilibrium constant related to the original?

• It is the square root of the original.

• It is the square of the original.

• It is double the original.

• It is half of the original.

What happens to the equilibrium constant if the stoichiometric coefficients of a reaction are changed?

• It becomes zero.

• It is unaffected.

• It is raised to the power of the change factor.

• It is multiplied by the change factor.