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Adding inert gas under constant volume will not disturb equilibrium. But I want to know what would happen if inert gases are added at constant pressure. If total pressure remains constant and inert gases are added, then mole fraction of any gas participating in equilibrium decreases and hence partial pressure decreases. If $\Delta n$ is non zero, then $K$ changes. But how can $K$ change if temperature remains constant?

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marked as duplicate by Loong, user15489, M.A.R., Todd Minehardt, ron Aug 29 '15 at 13:11

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    $\begingroup$ Try to reason backwards: you know K does not change when the temperature remains constant, what should happen to the equilibrium position and the partial pressure to make it so? Does the system still remain at equilibrium? $\endgroup$ – ℵ_ϵ Aug 29 '15 at 8:09
  • $\begingroup$ I was using the android app. It did not suggest any results bases on the title. I will delete the thread. $\endgroup$ – Aditya Dev Aug 29 '15 at 8:11
  • $\begingroup$ How do I delete it? $\endgroup$ – Aditya Dev Aug 29 '15 at 8:11
  • $\begingroup$ Under your post there should be a delete button. I'm accessing the question via a computer but there should be something similar on Android. $\endgroup$ – ℵ_ϵ Aug 29 '15 at 8:18