Effect of Temperature on Chemical Reaction Equilibrium

Tom Hardy

here is the question (part I): 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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"Effect of Temperature on Chemical Reaction Equilibrium"

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