January 29, 2023, 02:38:49 PM
Forum Rules: Read This Before Posting


Topic: equilibrium pressure trouble  (Read 2486 times)

0 Members and 1 Guest are viewing this topic.

Offline docpar

  • Regular Member
  • ***
  • Posts: 9
  • Mole Snacks: +0/-0
equilibrium pressure trouble
« on: March 23, 2009, 06:22:40 PM »
HI, i am having trouble with a homework question:

At 298K,
2PCL3(g) + O2(g) = 2POCL3 (L)

A) If it starts at 1 atm pressure of PCl3(g) and 1 atm of O2 (g), what will be the equilibrium pressure of O2?

B) Will changing the temperature result in a larger mole fraction of O2, smaller or unchanged?

I think i should use an ICE table, but have no clue how to implement anything.

thanks for any *delete me*

Offline Loyal

  • Regular Member
  • ***
  • Posts: 84
  • Mole Snacks: +7/-5
  • Gender: Male
Re: equilibrium pressure trouble
« Reply #1 on: March 23, 2009, 06:38:49 PM »
Partial Pressure of a gas is modeled the same as concentration of a species in solution.   There isn't any difference in this case. Just set this up like any other problem.
Chemistry Student(Senior) at WSU

Offline docpar

  • Regular Member
  • ***
  • Posts: 9
  • Mole Snacks: +0/-0
Re: equilibrium pressure trouble
« Reply #2 on: March 23, 2009, 06:43:42 PM »
What would I set K equal to though (that is if I use the ICE table)?

Would it be somethign like this

K= 1/(1^2)1

This is using the partial pressure method.
The numerator would be 1 because the ;product is a liquid.

Sponsored Links