CHEM 115. Chapter 14 Pages 1-6

These flashcards cover key concepts and definitions from the lecture notes on chemical equilibrium.

What happens during the forward reaction in a chemical equilibrium?

Reactants are converted into products, resulting in a decrease in reactant concentrations and an increase in product concentrations.

What is dynamic equilibrium?

Dynamic equilibrium is the condition where the rates of the forward reaction and reverse reaction are equal, leading to constant concentrations of reactants and products.

What does the equilibrium constant (K) represent?

K is the numerical value of the equilibrium constant expression of a reversible chemical reaction at a particular temperature.

How is the equilibrium constant expression derived according to the Law of Mass Action?

It is the ratio of the equilibrium concentrations or partial pressures of products to reactants, with each term raised to the power equal to its coefficient in the balanced equation.

What does a large value of Keq (Keq >> 1) indicate about a reaction?

It indicates that there will be many more product molecules present than reactant molecules at equilibrium, favoring products.

What does a small value of Keq (Keq << 1) indicate about a reaction?

It indicates that there will be many more reactant molecules present than product molecules at equilibrium, favoring reactants.

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

The equilibrium constant is inverted.

If the coefficients in a balanced equation are multiplied by a factor, what happens to K?

The equilibrium constant is raised to the same factor.

Are pure solids and liquids included in the equilibrium constant expression?

No, pure solids and liquids are not included because their concentrations do not change during the reaction.

What relationship exists between Kp and Kc at constant temperature?

Kp = Kc(RT)∆n, where ∆n is the change in moles of gas between products and reactants.