Gas Equilibria - Kp
In a mixture of gases all the gases exert their own pressure called a partial pressure.
The partial pressure is the pressure the gas exerts in a mixture of gases if it occupied the
volume of the entire container.
Partial pressure = px (pO2).
Daltons Law states that the total pressure = the sum of partial pressure. Total pressure = p1 +
p2 + p3.
Kp is the gas equilibrium constant for a reversible reaction when some/all the reactants are
gases.
Mole fraction is the proportion of a gas mixture made up of a particular gas.
Mole fraction has no units because it is moles over moles. Sum of all mole fractions = 1. The
mole fraction should be expressed as a decimal.
The moles is proportional to the pressure - greater the number of moles = greater pressure.
partial pressure = pX (partial pressure O2 = pO2)
partial pressure = mole fraction x total pressure of the gas
mole fraction = the number of moles of the gas/moles of all the gases
Kp kPa but u make your
own
Mole Fraction no units
Partial kPa
Pressure
In a mixture of gases all the gases exert their own pressure called a partial pressure.
The partial pressure is the pressure the gas exerts in a mixture of gases if it occupied the
volume of the entire container.
Partial pressure = px (pO2).
Daltons Law states that the total pressure = the sum of partial pressure. Total pressure = p1 +
p2 + p3.
Kp is the gas equilibrium constant for a reversible reaction when some/all the reactants are
gases.
Mole fraction is the proportion of a gas mixture made up of a particular gas.
Mole fraction has no units because it is moles over moles. Sum of all mole fractions = 1. The
mole fraction should be expressed as a decimal.
The moles is proportional to the pressure - greater the number of moles = greater pressure.
partial pressure = pX (partial pressure O2 = pO2)
partial pressure = mole fraction x total pressure of the gas
mole fraction = the number of moles of the gas/moles of all the gases
Kp kPa but u make your
own
Mole Fraction no units
Partial kPa
Pressure
