[hwgw]

Hi all,

If given
N2: kH = 8.57×10^4 atm
O2: kH = 4.34×10^4 atm

How can I find the N2 to O2 equilibrium molar ratio knowing there's 78% N2 and 21% O2 in the air @ 25 degC?

I initially tried using ideal gas law equation

PV = nRT
n/V = P/RT
M= P/RT

then i solved for the individual partial pressures and plugged it into the ideal gas law equation to compare their molarities.

Apparently this was not the correct way of solving. Could anyone please shed some light on why this is the wrong approach and maybe lead me into the correct path?

Thanks

[Rabn]

Henry's Law refers to the amount of gas dissolved in a liquid. This link will show you the equation. and possibly more....http://en.wikipedia.org/wiki/Partial_pressure. I'm a little confused as to wht you are trying to find.  You need to clarify this.  Maybe type the question as it is written.

also take a look at this site http://en.wikipedia.org/wiki/Air It should help clarify it for you a little more.