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.
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).