Equilibrium Constant Concepts

The video tutorial explains how to calculate an equilibrium constant (Kc) from equilibrium constant expressions. It begins with an introduction to the concept of equilibrium in chemical reactions, emphasizing the importance of balanced chemical equations. The tutorial then guides viewers through writing equilibrium constant expressions and calculating Kc using given equilibrium concentrations. Finally, it interprets the significance of Kc values, highlighting how a small Kc indicates a reaction favoring reactants.

Why is it important to ensure that a chemical equation is balanced before calculating the equilibrium constant?

• To ensure the reaction proceeds

• To make the calculation easier

• To determine the initial concentrations

• To accurately reflect the stoichiometry of the reaction

What does it mean when a reaction reaches equilibrium?

• The temperature of the system decreases

• The reaction stops completely

• The concentrations of reactants and products are equal

• The forward and reverse reactions occur at the same rate

Why do we use Kc instead of Kp in this scenario?

• Because the reaction is exothermic

• Because the concentrations are given in molarity

• Because the substances are solids

• Because the reaction is irreversible

In the equilibrium constant expression, why are products placed on top?

• Because the expression is a ratio of products to reactants

• To emphasize the importance of products

• To ensure the units cancel out

• To simplify the calculation

How does the stoichiometry of a reaction affect the equilibrium constant expression?

• It affects the temperature dependence

• It changes the units of Kc

• It has no effect on the expression

• It determines the exponents in the expression

What is the significance of using equilibrium concentrations in the Kc expression?

• They simplify the calculation

• They are always higher than initial concentrations

• They reflect the system at equilibrium

• They are easier to measure

How is the equilibrium constant Kc calculated from equilibrium concentrations?

• By dividing the concentration of products by reactants, each raised to their stoichiometric coefficients

• By multiplying the concentrations of reactants

• By adding the concentrations of reactants and products

• By subtracting the concentration of reactants from products

What is the relationship between the reaction quotient Q and the equilibrium constant Kc?

• Q is the same as Kc at all times

• Q is used to determine if a system is at equilibrium

• Q is only used for gaseous reactions

• Q is always greater than Kc

What does a small Kc value indicate about a reaction?

• The reaction is very fast

• The reaction favors the formation of reactants

• The reaction is at a high temperature

• The reaction favors the formation of products

Why does a small Kc value suggest that the reactant concentrations are greater than the product concentrations at equilibrium?

• Because the reaction is incomplete

• Because the forward reaction is faster

• Because the system is not at equilibrium

• Because the reverse reaction is favored