How do you calculate the overall Keq for multiple reactions added together?
Multiply the individual Keq values of each reaction (K_total = K₁ * K₂ * ...).
Describe the steps to find the equilibrium constant for a multi-step reaction.
1. Manipulate individual reactions to match the target reaction.
2. Apply corresponding changes to K values (inverse, exponentiate).
3. Add the manipulated reactions.
4. Multiply the adjusted K values to find the overall K.
Define equilibrium constant (Keq).
A value that expresses the ratio of products to reactants at equilibrium.
What does K > 1 indicate?
The products are favored at equilibrium.
What does K < 1 indicate?
The reactants are favored at equilibrium.
Define Hess's Law.
The enthalpy change of a reaction is the same regardless of the number of steps.
What happens to K when a reaction is reversed?
The new equilibrium constant is the inverse of the original (K_new = 1/K_old).
What happens to K when a reaction is multiplied by a factor 'n'?
The new equilibrium constant is the original raised to the power of 'n' (K_new = K_old^n).
What is the effect of flipping a reaction on the equilibrium constant?
The new equilibrium constant becomes the inverse of the original (K_new = 1/K_old).
What is the effect of multiplying a reaction by a coefficient 'n' on the equilibrium constant?
The equilibrium constant is raised to the power of 'n' (K_new = K_old^n).
What is the effect of adding two reactions on their equilibrium constants?
The equilibrium constants are multiplied (K_total = K₁ * K₂).
