Consider the decomposition of the compound C5H6O3 as follows: C5H6O3(g)  C2H6(g) + 3CO(g) A 5.63 g sample of pure C5H6O3(g) was placed in an evacuated 2.50 L flask and heated to 200.ºC. At equilibrium, the pressure in the flask was 1.63 atm. Calculate K for this reaction.

Explanation:

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In this case, the first step is to compute the initial moles of C₅H₆O₃ as shown below:

After that, by knowing that the final pressure is 1.63 atm, one computes the total moles at the equilibrium as follows:

Then, by knowing the moles at the equilibrium considering the change "", which yields to:

The total moles at the equilibrium turn out:

By solving for "", we've got:

Finally, the equilibrium constant is:

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