3.1.10 Equilibrium constant Kp for homogeneous systems

Question 1

Partial pressure equation

Answer 1

(Moles of A / Total Moles) x Total Pressure

Question 2

How are partial pressures written

Answer 2

(ppA)^b
DO NOT USE [ppA]^b

Question 3

What is partial pressure normally measured in

Answer 3

Pascals (Pa)

Question 4

Kp equation for 2A +3B –> Y + 2Z

Answer 4

Kp = (ppY) (ppZ)^2 / (ppA)^2 (ppB)^3

Question 5

What state do all reactants and products need to be to find partial pressure

Answer 5

Gaseous

Question 6

What effect would a decrease in temperature have on equilibrium (forward reaction is exothermic)

Answer 6

Equilibrium shifts to favour forward (exothermic reaction) to increase temperature so more products formed. So higher Kp

Question 6

What effect would a decrease in pressure have on equilibrium (LHS has more moles)

Answer 6

Equilibrium shifts to favour backward reaction to counteract change in pressure. So more reactants formed, resulting in lower Kp.

Question 7

What effect does a catalyst have on equilibrium and Kp

Answer 7

Equilibrium is reached quicker but is NOT changed
Kp is unchanged by catalyst as equilibrium isn’t