Chapter 19 - Kp
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what is Kp
it is a measure of equilibrium for a reaction with gaseous species
what is partial pressure
the pressure that a gas would give if alone occupying the same volume as the total gases
how is partial pressure calculated
total pressure * mole fraction
what is mole fraction
mole of a species / total moles of a reaction mixture
what is Kp given by
partial pressure of products to the powers of their stoichiometry / partial pressure of reactants to the powers of their stoichiometry
what changes in conditions affects Kp
only temperature
what restrictions are there on calculating Kp
you must only use the partial pressures of the gaseous species
how does Kp change for an exothermic reaction if temp increases
Kp decreases
why does pressure not affect Kp
any shift in the equilibrium position (towards fewer moles of gas) caused by a pressure change is perfectly counteracted by the changes in partial pressures, ensuring the ratio (Kp) remains constant