equilibrium constant Flashcards
what is partial pressure
each gas’ contribution to the total pressure
how would you calculate the partial pressure of a gas
partial pressure = mole fraction x total pressure
what is the mole fraction
mole fraction = number of moles of gas X in mixture / total number of moles if mixture
reaction is represented by aA + bB <–> cC
what is the Kp for the system
Kp = (pC^c x pD^d) / (pA^a x pB^b)
how do you calculate units for Kp
units of partial pressure and cancel them out
what is the effect of increasing temperature on Kp for an endothermic reaction
equilibrium shifts to the right, so partial pressures of products increase, so Kp increases
what is the effect of increasing the overall pressure on Kp for this reaction
Kp = (pC^c x pD^d) / (pA^a x pB^b)
pressure does not affect Kp as, if moles of gas 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 will 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 the activation energy –> more successful collisions per second
- pressure : more particles in the same volume –> more successful collisions per second
