Textbook Problem 5I #15

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SLai_1I
Posts: 106
Joined: Wed Sep 30, 2020 9:52 pm

Textbook Problem 5I #15

Postby SLai_1I » Fri Jan 15, 2021 4:47 pm

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!

Lucy_Balish_3G
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Re: Textbook Problem 5I #15

Postby Lucy_Balish_3G » Fri Jan 15, 2021 5:05 pm

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.

Andrew Yoon 3L
Posts: 93
Joined: Wed Sep 30, 2020 9:36 pm

Re: Textbook Problem 5I #15

Postby Andrew Yoon 3L » Fri Jan 15, 2021 8:53 pm

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.

Shrinidhy Srinivas 3L
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Re: Textbook Problem 5I #15

Postby Shrinidhy Srinivas 3L » Fri Jan 15, 2021 8:55 pm

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!

SLai_1I
Posts: 106
Joined: Wed Sep 30, 2020 9:52 pm

Re: Textbook Problem 5I #15

Postby SLai_1I » Sun Jan 17, 2021 3:49 pm

Ahh I see it now. Thank you so much!


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