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Date Posted: 6/27/2008 1:24:53 AM  Status: Live
equilibrium
Course Textbook Chapter Problem
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Question Details:
  Stuck! Please help! ASAP!
 
The formation of methanol is important to the processing of new fuels.  At 298.0 K, Kp = 2.25 x 10^4 for the reaction
 
CO(g) + 2H2(g) ↔ CH3OH(l)
 
If ΔHο rxn = -128 kJ/mol CH3OH, calculate Kp at 2.0 οC.
 
 
Thanks!!

Answers:

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Sage
Karma Points: 3,963
Date Posted: 6/27/2008 1:37:09 AM  Status: Live
Asker's Rating: Helpful   
Response:
given, k1= 2.25x104 at T1= 298K
          k2=?   at     T2= 20C=2+273=275K
ΔHrxn= -128KJ/mol= -128x103J/mol,R= 8.314J/mol.K
from arrhenius equation, we have
ln (k2/k1) = (ΔH/R)[(1/T1)-(1/T2)]
ln (k2/k1) = (-128x103/8.314)[(1/298)-(1/275)] =4.321
k2= 75.26*(2.25x104 )=1.69x106
babi3manic49's Comment:
Thanks! =)

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Date Posted: 6/27/2008 1:50:45 AM  Status: Live
Asker's Rating: N/A-Posted by Person Asking Question   
Response:
When I submitted that answer, it said incorrect. I think it could be the program, but I'm not sure. Thank you for answering so quickly though.



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