5.1.2 equilibrium Flashcards
what is homogeneous equilibrium?
an equilibrium in which all the species making up the reactants and products have the same physical state
what is heterogeneous equilibrium?
an equilibrium in which the species making up the reactants and products have different physical states
Kc equation for heterogeneous equilibrium
concentration of solids and liquids are omitted as essentially constant
mole fraction x(A) equation
number of moles of A / total number of moles in gas mixture
partial pressure p(A) equation
mole fraction of A x total pressure P
what is the sum of mole fractions?
1
what is the sum of partial fractions?
total pressure
Kp expression for A + B ⇌ C
Kp = p(C) / p(A) x p(B)
what is the effect on K when temperature is increased?
for a exothermic reaction - K decreases, equilibrium shifts to the left, decreasing yield of products
for a endothermic reaction - K increases, equilibrium shifts to the right, increasing yield of products
explain effect of increasing temperature on an exothermic reaction
A + B ⇌ C
K decreases
system no longer in equilibrium
ratio C / A x B greater than K
- the concentration/partial pressure of C must decrease
- the concentration/partial pressure of A and B must increase
- position of equilibrium shifts to the left
- new equilibrium reached where C / A x B = new K
explain effect of increasing temperature on an exothermic reaction
A + B ⇌ C
K increases
system no longer in equilibrium
ratio C / A x B less than K
- the concentration/partial pressure of C must increase
- the concentration/partial pressure of A and B must decrease
- position of equilibrium shifts to the right
- new equilibrium reached where C / A x B = new K
what is the effect on K when concentration is changed?
no effect on K
what is the effect on K when pressure is changed?
no effect on K
explain, in terms of K, the effect of changing concentration
A ⇌ 2B
- if [A] is increased
- ratio of [B]² / [A] is less than Kc
- system no longer in equilibrium
- [A] must decrease
- [B] must increase
- new equilibrium established where [B]² / [A] is restored to Kc
explain, in terms of K, the effect of changing pressure
A ⇌ 2B
- if the total pressure is doubled
- ratio of p(B)² / p(A) is greater than Kp
- system no longer in equilibrium
- p(A) must increase
- p(B) must decrease
- new equilibrium established where [B]² / [A] is restored to Kp