All Flashcards
What are the steps to set up an ICE table?
- Write out the balanced equation. 2. Set up the ICE table with initial concentrations. 3. Use the change in concentration based on reaction stoichiometry. 4. Use the equilibrium constant expression to solve for x, and calculate equilibrium concentrations.
What happens to the equilibrium when you increase the concentration of a reactant?
The equilibrium shifts towards the products to consume the added reactant.
What happens to the equilibrium constant (K) when you reverse a reaction?
The new equilibrium constant becomes the inverse of the original (1/K).
What happens to the solubility of a sparingly soluble salt when a common ion is added?
The solubility of the salt decreases (Common Ion Effect).
What happens to the equilibrium of an exothermic reaction when temperature is increased?
The equilibrium shifts towards the reactants.
What happens to Gibbs Free Energy at equilibrium?
ΔG = 0.
What are the differences between Q and K?
Q: Ratio of products to reactants at any time, used to predict shift. | K: Ratio of products to reactants at equilibrium, constant at a given temperature.
What are the differences between product-favored and reactant-favored reactions?
Product-favored: K > 1, more products at equilibrium. | Reactant-favored: K < 1, more reactants at equilibrium.