Revise later
SpaceTo flip
If confident
All Flashcards
Define reversible reaction.
A reaction that proceeds in both forward (reactants to products) and reverse (products to reactants) directions simultaneously.
What is chemical equilibrium?
The state where the rate of the forward reaction equals the rate of the reverse reaction; a dynamic, not static, process.
Define a closed system in the context of equilibrium.
A system that does not exchange matter or energy with its surroundings, allowing equilibrium to be established.
What is the equilibrium constant (\(K_c\))?
A value that measures how far a reaction proceeds toward products at equilibrium; the ratio of product concentrations to reactant concentrations at equilibrium.
What is the equilibrium constant (\(K_p\))?
Similar to \(K_c\) but uses partial pressures instead of concentrations, specifically for gases.
Define dynamic equilibrium.
A state where the forward and reverse reactions occur at equal rates, resulting in no net change in reactant or product concentrations, but the reactions are still actively occurring.
What happens to the forward reaction rate as reactant concentrations decrease?
The forward reaction rate slows down.
What happens to the reverse reaction rate as product concentrations increase?
The reverse reaction rate speeds up.
What is the effect of adding more reactant to a system at equilibrium?
The rate of the forward reaction will temporarily increase to re-establish equilibrium.
In an exothermic reaction at equilibrium, what happens to the value of \(K_c\) if the temperature is increased?
The value of \(K_c\) will decrease because the reverse reaction is favored.
What happens to a system at equilibrium if it is not in a closed container?
Equilibrium cannot be established or maintained due to the exchange of matter and/or energy with the surroundings.
What happens to the rates of forward and reverse reactions at equilibrium?
The rates of the forward and reverse reactions are equal.
What are the key differences between \(K_c\) and \(K_p\)?
\(K_c\): Uses concentrations of reactants and products. | \(K_p\): Uses partial pressures of gaseous reactants and products.
Differentiate between a system at equilibrium and a reaction that has stopped.
Equilibrium: Forward and reverse rates are equal, dynamic process. | Stopped Reaction: No forward or reverse reaction occurring.
Compare open and closed systems in the context of chemical equilibrium.
Closed System: No exchange of matter or energy, equilibrium can be reached. | Open System: Exchange of matter and/or energy, equilibrium cannot be maintained.
What is the difference between equal rates and equal concentrations at equilibrium?
Equal Rates: The rate of the forward and reverse reactions are equal. | Equal Concentrations: The concentrations of reactants and products are constant, but not necessarily equal.