anonymous
  • anonymous
At 400K, an equilibrium mixture of H2, I2, and HI consists of 0.054 mol H2, 0.019 mol I2, and 0.059 mol HI in a 1L flask. What is the value of KP for the following equilibrium? 2HI(g) <--> H2(g) + I2 (g) I understand you convert to Molarity from moles first, then plug that into the Kc equation, but then I keep making a mistake at about that point. Thanks!
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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schrodinger
  • schrodinger
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chmvijay
  • chmvijay
just write the Kp for the following and put in that equation and solve
anonymous
  • anonymous
Right, I did that but still got the wrong answer. \: I think I'm not converting something correctly or something.
chmvijay
  • chmvijay
Kp = Kc (RT)∆n did u do this

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anonymous
  • anonymous
Yes, I think the moles are screwing me up though. I got 0 change in moles, is this correct?
chmvijay
  • chmvijay
yaa its correct delta n =0
anonymous
  • anonymous
Hmm well, wouldn't to the ^0 power make it = 1 then? That's where I am confused. It says the correct answer was the value I got for Kc. (0.29)
anonymous
  • anonymous
OH NO, I just realized I multiplied all of it together! I did ((0.29)(0.0821)(400))^0. Oops! Thank you!! (:
chmvijay
  • chmvijay
you are confusing me to LOL
anonymous
  • anonymous
Hahaha thank you for sticking it out with me anyways, I have a final tomorrow & you're helping tons (:
chmvijay
  • chmvijay
:)

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