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Define the reaction quotient, Q.
Q is a measure of the relative amount of products and reactants present in a reaction at any given time. It predicts the direction the reaction will shift to reach equilibrium.
Define the equilibrium constant, K.
K is the value of the reaction quotient when the reaction has reached equilibrium. It indicates the ratio of products to reactants at equilibrium.
Define Le Châtelier's Principle.
Le Châtelier's Principle states that if a change of condition is applied to a system in equilibrium, the system will shift in a direction that relieves the stress.
Define Q < K.
The ratio of products to reactants is less than that at equilibrium. The reaction will shift towards the products.
Define Q > K.
The ratio of products to reactants is greater than that at equilibrium. The reaction will shift towards the reactants.
What are the key differences between Q and K?
Q: Calculated at any point in the reaction. Indicates the direction of shift to reach equilibrium. | K: Calculated only at equilibrium. Represents the ratio of products to reactants at equilibrium.
How does temperature affect Q vs. K?
Q: Temperature does not directly affect Q in the same way as concentration or pressure. | K: Temperature changes the value of K itself; K is temperature-dependent.
What is the effect of adding reactants to a system at equilibrium?
Adding reactants decreases the value of Q, making Q < K. The system shifts towards the products to re-establish equilibrium.
What is the effect of adding products to a system at equilibrium?
Adding products increases the value of Q, making Q > K. The system shifts towards the reactants to re-establish equilibrium.
What is the effect of increasing pressure on a gaseous system at equilibrium?
Increasing pressure favors the side of the reaction with fewer moles of gas.
What is the effect of decreasing pressure on a gaseous system at equilibrium?
Decreasing pressure favors the side of the reaction with more moles of gas.
What is the effect of increasing temperature on an exothermic reaction at equilibrium?
Increasing temperature decreases the value of K, favoring the reverse reaction (shift towards reactants).
What is the effect of increasing temperature on an endothermic reaction at equilibrium?
Increasing temperature increases the value of K, favoring the forward reaction (shift towards products).