When solid NH4HS and 0.400 mol NH3(g) were placed in a vessel of volume 2.0 L at 24 8C, the equilibrium NH4HS(s) ->NH3(g) + H2S(g), for which Kc=1.6*10^-4, was reached. What are the equilibrium concentrations of NH3 and H2S?
Does anyone know how to do this problem? I think it's and ICE Table problem, but I'm confused because NH3 is a product rather than a reactant. Please let me know!
Textbook Problem 5I #15
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Re: Textbook Problem 5I #15
It would be an ice table but instead of starting with 0 for your initial concentration of products, you start with .2M. Then you add to the left and subtract from the right and solve as you would normally! Don’t forget that you only ever include aqueous and gaseous in your equilibrium constant.
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Re: Textbook Problem 5I #15
Since the problem gives the moles of NH3 in the beginning of the reaction, you would write 0.2 mol/L for the initial concentration for NH3. Then, you would solve for x just how you would for any other ICE box.
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Re: Textbook Problem 5I #15
Hi! For this problem, you would set up an ICE box the way you normally do and solve for the equilibrium concentrations. Make sure that before you start the problem that you solve for Q to know which way the reaction will proceed. Also, make sure that when you set up your K and Q equations that you don't include NH4HS because it's a solid. I hope this helps!
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