1.10 Equilibrium constant Flashcards
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 eqn
Mole fraction of gas X = number of moles of gas X in the mixture / total number of moles of gas in mixture
A reaction is
aA(g) + bB(g) <–> cC(g) + dD(g)
What is Kp for system
pC^c x pD^d
/
pA^a x pB^b
Pa = partial pressure of A
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
What is the effect of increasing temperature on Kp for an endothermic reaction
Equilibrium shifts to the right, partial pressure of products increase so Kp increases
What is the effect of increasing the overall pressure on Kp for this reaction
pC^c x pD^d
/
pA^a x pB^b
No effect as if moles of gas are not the same on each side, either top or bottom of expression will have a total pressure term that does not cancel
What will be the kinetic effect of increasing the temperature and pressure for any reaction
Increasing both will increase rate of reaction
Temperature - many more particles will have the activation energy, more successful collisions
Pressure - more particles in same volume - more frequent collisions
