Effect of Temperature on Chemical Reaction Equilibrium

here is the question (part I):
MwGKy.png



For part I, I need some assistance, I cannot figure out how to do the question. I know eventually what to do, it's just working out the equilibrium constants I'm having trouble with. So to start, I want to work out the K values at 600K and 800K, I do this by considering the total pressure:

$$
\text{Total Pressure} = 1 \text{ bar}
$$

Initially:

$$
P^{o_2} + P^{HCl} = 1
$$
Since there are 4 mols of hcl per o2 we can write:

$$
5P^{o_2} = 1 \implies P^{O_2} = 0.2 \text{bar}
$$

85% conversion means that in the end, 85% of the oxygen has reacted therefore, there is 0.2*0.15 = 0.03 bar oxygen remaining, therefore 0.12 bar HCl remaining. In addition to this, each mol of oxygen reacted results in 4 new mols being created, therefore there are (0.85*0.2*2) bar of water (and also chlorine) produced, with this information, I can calculate my equilibrium constant, is this correct?
 
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Thanks for the thread! This is an automated courtesy bump. Sorry you aren't generating responses at the moment. Do you have any further information, come to any new conclusions or is it possible to reword the post? The more details the better.
 

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