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Compare a reaction with K >> 1 to one with K << 1.
K >> 1: Product-favored, reaction proceeds nearly to completion. | K << 1: Reactant-favored, reaction hardly proceeds forward.
Compare the acid dissociation of a strong acid (large K) to a weak acid (small K).
Strong acid (large K): Dissociates almost completely into ions. | Weak acid (small K): Dissociates only slightly into ions.
Differentiate between kinetics and equilibrium regarding reaction understanding.
Kinetics: Determines the rate at which a reaction reaches equilibrium. | Equilibrium: Determines the extent of the reaction at equilibrium (product vs reactant favorability).
Define equilibrium constant (K).
K is the ratio of products to reactants at equilibrium. It indicates the extent to which a reaction proceeds.
What does K > 1 indicate?
Product-favored reaction; more products than reactants at equilibrium.
What does K < 1 indicate?
Reactant-favored reaction; more reactants than products at equilibrium.
What does K = 1 indicate?
Neither product nor reactant favored; product and reactant concentrations are equal at equilibrium.
Define 'product-favored'.
At equilibrium, the concentration of products is significantly higher than the concentration of reactants (K > 1).
Define 'reactant-favored'.
At equilibrium, the concentration of reactants is significantly higher than the concentration of products (K < 1).
What is the effect of a very large K value on the equilibrium position?
The equilibrium position lies far to the right, favoring the products.
What is the effect of a very small K value on the equilibrium position?
The equilibrium position lies far to the left, favoring the reactants.
Cause: K for a reaction increases significantly. Effect?
More products are formed at equilibrium.