OK, some of you may have read my previous OP on my equilibrium constant woes, and now I have another (but final) question.
Dont worry, I’m not asking you to do my homework, merely how I can go about doing it myself…
Right, I’ve been asked to work out Kp (and the mole fractions and partial pressures of the gasses, but you need them for finding Kp) for a system;
N[sub]2[/sub]O[sub]4(g)[/sub] <==> 2NO[sub]2(g)[/sub]
I’ve only been given limited data, and I can’t quite see how to use it:
- The pressure of the system is 0.200atm
- At equilibrium, the relative molecular mass of the equilibrium mixture was 59.8g mol[sup]-1[/sup]
How do I work it out with only these?
I know that once I have the mole fractions, it will become easy, because…
Kp = (P[sub]NO2[/sub])[sup]2[/sup] / (P[sub]N2O4[/sub])
Do I assume that I have a certain amount in total, even though it’s not given, and work out the mole fractions from there?
Sorry to bother you people again, but I was absent from college last week due to illness, so I missed my chance to get help from my teacher, and it’s due in next week.
Thanks in advance,