Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: _cheers on April 16, 2007, 08:14:43 PM
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Suppose Kp is 81 at some temperature. In one experiment, the flask was charged with initial pressure, P atm, of PCl5 (no other gases) and equil established. What would the pressure have to be in order to make 10% of PCl5 decompose?
PCl3 + Cl2 <----> PCl5 (all gaseous)
HELP??? Ice table? can I make any assumptions? Sorry, I dont even know where to start!
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In terms of the original amount of PCl5, how much products and reactants would you have at equilibrium if 10% of the PCl5 were to decompose?
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Well, I'd have 90% PCl5, and 10% products?
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And how would that look if you plugged it into the equation for Kp?
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hmmm...I'll get back to you on that ;D