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I've noticed that when all the species are in the gas phase, the book has been using partial pressures and then converting them into concentrations using the ideal gas law and the ice table, so my question is when calculating the equilibrium constant for a reaction with all species in gas phase should we use Kp or it depends on the question, meaning we could use both Kc or Kp?
I also think it depends on what the question is asking for. I'm pretty sure that on the exam, Professor Lavelle will specify which one he's looking for. Since the only two states we can use in Kc/Kp calculations are gases and aqueous solutions anyway, we're bound to have problems with only gases reacting where we're only asked to find the Kc, or vice versa. In that case, there's no need to do both calculations when only one value is required.
Kp can actually be converted into Kc using the equation Kp=Kc(RT)^delta n, showing that Kp and Kc are not always interchangeable. You solve for the equilibrium constant using what the question gives you (whether it is Kp or Kc), unless noted otherwise.
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