after doing a search for kp and kc i stumbled on this age-old post so i guess i'll *Ignore me, I am impatient* this up instead of creating a new one, i mean god knows our forum could use a break from so many threads
my question is that,
as K
c is applicable to liquids and gases, does that mean a gaseous reaction will have the same K
c as a liquid reaction?
for example this reaction...
N
2 (g) + 3 H
2 (g) --> 2 NH
3 (g)
now under high pressure and
low temperature (-edit- changing the temperature would change the K value anyway) to liquefy the reactants and products as in the haber process (well maybe the reactants arent liquefied but lets say in a hypothetical scenario that they are all subjected to conditions that liquefy all of them), we have
N
2 (l) + 3 H
2 (l) --> 2 NH
3 (l)
instead.
will the K
c value be different for both?
also, is there any significance of raising the concentrations/partial pressures to the power of their stoichiometric ratio, apart from giving a certain variable more 'weight' in the equation?