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In this question he has given the G of formation for X and HX.So we will find the G of the reaction by subtracting 130.48 and 131.17.This gives us G to be -0.69.
Now we will use the formula G=-RTlnK to get the value of equilibrium constant.Taking R to be 8.314 ant the temperture as 500K we will get the value of K eo be exactly 1.
Since the the phases of the other products are aqueous we simply equate the the partial pressure of HX to the K we got.So the partial pressure is 1.
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