1. Equilibrium Constant (K):
* The equilibrium constant (K) is a value that expresses the ratio of products to reactants at equilibrium.
* You can calculate K using the law of mass action:
* K = [products]^coefficients / [reactants]^coefficients
* Where [ ] represents the molar concentration of each species.
2. Reaction Quotient (Q):
* The reaction quotient (Q) is similar to K, but it can be calculated at any point in the reaction, not just at equilibrium.
* It tells you the relative amounts of products and reactants at a given moment.
* Q = [products]^coefficients / [reactants]^coefficients
3. Gibbs Free Energy Change (ΔG):
* The Gibbs free energy change (ΔG) indicates the spontaneity of a reaction.
* You can calculate ΔG using the equation:
* ΔG = -RTlnK
* Where R is the ideal gas constant, T is the temperature in Kelvin, and K is the equilibrium constant.
4. Standard Gibbs Free Energy Change (ΔG°):
* The standard Gibbs free energy change (ΔG°) is the Gibbs free energy change under standard conditions (298 K and 1 atm).
* You can calculate ΔG° using the equation:
* ΔG° = -RTlnK°
* Where K° is the equilibrium constant under standard conditions.
5. Degree of Completion:
* You can determine the extent to which a reaction has proceeded to completion by comparing the initial and final concentrations of reactants and products.
* This can be used to calculate the percentage yield of the reaction.
6. Rate Constant (k):
* If the reaction is reversible, you can use the equilibrium constant (K) and the rate constants for the forward (kf) and reverse (kr) reactions to determine the individual rate constants:
* K = kf / kr
7. Activation Energy (Ea):
* You can use the Arrhenius equation to calculate the activation energy (Ea) of a reaction if you know the rate constant at two different temperatures:
* k = Ae^(-Ea/RT)
* Where A is the pre-exponential factor, R is the ideal gas constant, and T is the temperature in Kelvin.
Note: These calculations assume that the reaction is in equilibrium or that the concentrations of products and reactants are known at a specific point in time.
