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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: docpar on March 23, 2009, 06:22:40 PM

Title: equilibrium pressure trouble
Post by: docpar 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*

Title: Re: equilibrium pressure trouble
Post by: Loyal 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.

Title: Re: equilibrium pressure trouble
Post by: docpar 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.