Equilibrium constant Kp
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What is partial pressure
Each gas’s contribution to the total pressure
How would you calculate the partial pressure of a gas
Partial pressure p = mole fraction x total pressure
What is the mole fraction
Mole fraction of gas X = number of moles of gas X in the mixture / total number of moles of gas in the mixture
A reaction is represented by Aa (g) + bB (g) ⇋ cC (g) + dD (g)
For the reaction: aA + bB ⇋ cC + dD Kp = (pC^c pD^d) / (pA^a pB^b) Where pA = partial pressure of A and a = number of moles of A
How do you calculate the units for Kp
Write out the units for the partial pressures in the same arrangement as the Kp equation and cancel out / multiply together Usually in Pa, kPa, atm etc DO NOT CHANGE UNITS
What is the effect of increasing temperature on Kp for an endothermic reaction
Equilibrium shifts to the right so partial pressure of products increase so Kp increases
What is the effect of increasing the overall pressure on Kp for this reaction
Pressure does not affect Kp as, if moles of are not the same on each side, either top or bottom of Kp expression will have a total pressure term that does not cancel
What would be the kinetic effect of increasing the temperature and pressure for any reaction
Increasing both will increase the rate of reaction as: Temperature - many more particles have energy greater than or equal to activation energy —> more successful collisions per second Pressure - more particles in the same volume —> more successful collisions per seconf