partial pressures

So all the, both of the partial pressures and the total pressure are going to go lower than indicated here.

Which is the form of the equilibrium constant not in terms of the partial pressures, but in terms of the mole fraction.

p And we're going to put a little p here, because it's in terms of the partial pressures.

And since both partial pressures are bigger, the total pressure has to be bigger.

OK, so it's obvious just from looking at this that each of the partial pressures is bigger than it is in the ideal case.

Somehow we're going to have to get partial pressures in there.

Blood gas analyses measure directly the pH and the partial pressures of oxygen and carbon dioxide in a blood sample.

These log partial pressures all come from expanding out the chemical potential as mu naught plus RT log p.

I shouldn't really have written this for the specific case of partial pressures.

English chemist and physicist who formulated atomic theory and the law of partial pressures (1766-1844).

But we know now how to go from chemical potentials to partial pressures. It's written right here.

And in each of the individual partial pressures.

Sum of the two partial pressures.

The partial pressures are given by these lines.

The relationship between isoflurane partial pressures in arterial blood and in oxygenator outlet gas during cardiopulmonary bypass

Dalton's law of partial pressures