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What are the steps to solve for equilibrium concentrations using an ICE table?
- Write the balanced chemical equation. 2. Set up the ICE table. 3. Write the equilibrium expression. 4. Plug in equilibrium concentrations from the ICE table. 5. Use the 5% approximation (if applicable). 6. Solve for x. 7. Find equilibrium concentrations.
How do you set up the 'Change' row in an ICE table?
Reactants decrease in concentration (-x), and products increase in concentration (+x), considering stoichiometric coefficients.
How do you determine if the 5% approximation is valid?
If the change in concentration ('x') is less than 5% of the initial concentration, the approximation is valid.
What is the first step in solving an equilibrium problem?
Write the balanced chemical equation for the reaction.
What do you do after setting up the ICE table?
Write the equilibrium expression (K = [Products]/[Reactants]).
What do you do after writing the equilibrium expression?
Plug in the equilibrium concentrations from the ICE table into the equilibrium expression.
What is the difference between initial concentration and equilibrium concentration?
Initial concentration: Concentration at the start of the reaction. Equilibrium concentration: Concentration when the reaction reaches equilibrium.
When should you use the 5% approximation, and when should you avoid it?
Use: When K is small (usually < 10⁻⁴) and 'x' is added/subtracted. Avoid: When 'x' is the only term or multiplied by a coefficient.
What are ICE Tables?
Tables that organize initial concentrations, changes, and equilibrium concentrations to solve equilibrium problems.
Define 'Initial' in an ICE table.
The concentrations of reactants and products at the start of the reaction.
Define 'Change' in an ICE table.
The change in concentration of reactants and products as the reaction proceeds to equilibrium, usually represented by 'x'.
Define 'Equilibrium' in an ICE table.
The final concentrations of reactants and products when the reaction has reached equilibrium.
What is the equilibrium constant (K)?
The ratio of products to reactants at equilibrium, indicating the extent of a reaction.
What is the 5% approximation?
An assumption that 'x' is negligible compared to initial concentrations if K is small, simplifying calculations.