All Flashcards
Compare the manipulation of ΔH and K when reversing a reaction.
ΔH: The sign is flipped. | K: The value is inverted (K_new = 1/K_old).
Compare the manipulation of ΔH and K when multiplying a reaction by 'n'.
ΔH: Multiplied by 'n'. | K: Raised to the power of 'n' (K_new = K_old^n).
Compare the manipulation of ΔH and K when adding reactions.
ΔH: Add the ΔH values. | K: Multiply the K values.
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).
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.
- Manipulate individual reactions to match the target reaction.
- Apply corresponding changes to K values (inverse, exponentiate).
- Add the manipulated reactions.
- Multiply the adjusted K values to find the overall K.