tarchon
First Post
The term comes from Dalton's Law of partial pressures. For a mixture of gasses, the total pressure is the sum of the pressures of the component gases, like Pair=PN2+PO2+PCO2glass said:If the OP will forgive a slight threadjack, what exactly is 'partial pressure'? I've been hearing it around for years, but nobody has been able to give me an explanation I could really assimilate.
If you combine this with the ideal gas law (PV=nRT), the partial pressure of a particular ideal gas is then just the (molar) percentage of that gas in the mixture times the total pressure. The reason this is usually significant is that most chemical reaction rates depend on the number of reactant molecules per volume, which is proportional to pressure (again, for an ideal gas). Since only the reactant gas is involved in the reaction, not all the other gasses, if you want to find the reaction rate of, for example, oxidation, you have to use the partial pressure of the reactant gas, oxygen, in the rate equation.
Another way to look at it is that the partial pressure of O2 is the pressure the gas would have if you took away everything but the O2.
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