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Partial Pressures

  • Thread starter jtruth914
  • Start date
  • #1
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a) Determine K at 298K for the reaction H2(g) + Cl2(g) <---> 2HCl(g)
b) The equilibrium partial pressure of HCl is 1 bar. Determine the equilibrium partial pressures of H2 and Cl2.


This question was on my test. I got K= 3.2 x 10^-34 using dG*=-RTlnK when dG=0 at equilibrium. I'm having trouble determining the partial pressures. I know that Pj=(xj)(Ptot). I also know that K= (PHCl)^2/(PH2)(PCl2), but I still don't know how to determine the partial pressure just based off of PHCl=1 bar???
 

Answers and Replies

  • #2
Borek
Mentor
28,357
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You are most likely to assume you started with HCl and all H2 and Cl2 are products of dissociation. This, plus stoichiometry, gives you all information you need to solve the problem.
 
  • #3
21
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I figured it out. thanks
 

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