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Differentiate between a product-favored and a reactant-favored reaction.
Product-favored: More products than reactants at equilibrium. K > 1. | Reactant-favored: More reactants than products at equilibrium. K < 1.
Compare forward and reverse reaction rates at equilibrium.
At equilibrium: Forward reaction rate = Reverse reaction rate.
Compare a reaction with K > 1 and a reaction with K < 1.
K > 1: Product-favored, more products at equilibrium. | K < 1: Reactant-favored, more reactants at equilibrium.
Compare a reaction with a large K value and a small K value.
Large K value: Reaction goes further to completion, more products. | Small K value: Reaction does not go far, more reactants.
Compare the dissociation of acetic acid and carbonic acid based on their K values.
Acetic acid (K = 1.8 * 10⁻⁵): Dissociates more, stronger acid. | Carbonic acid (K = 4.3 * 10⁻⁷): Dissociates less, weaker acid.
Define chemical equilibrium.
The state where the forward and reverse reaction rates are equal, resulting in constant reactant and product concentrations.
What is a reversible reaction?
A reaction where reactants form products and products can revert back to reactants (A ⇌ B).
Define 'product-favored' reaction.
A reaction where, at equilibrium, there are more products than reactants.
Define 'reactant-favored' reaction.
A reaction where, at equilibrium, there are more reactants than products.
What does the equilibrium constant, K, represent?
K indicates the ratio of products to reactants at equilibrium and reveals the extent to which a reaction proceeds to completion.
What is the effect of a large K value on the amount of product at equilibrium?
A large K value indicates that the reaction favors product formation, resulting in more product at equilibrium.
What is the effect of a small K value on the amount of reactant at equilibrium?
A small K value indicates that the reaction favors reactants, resulting in more reactant at equilibrium.
What happens to the equilibrium position if K >> 1?
The equilibrium position shifts far to the right, favoring product formation.
What happens to the equilibrium position if K << 1?
The equilibrium position shifts far to the left, favoring reactant formation.
For an exothermic reaction, what happens to K if temperature increases?
K decreases, shifting the equilibrium towards reactants.