[calvin coolidge]

I'm trying to figure out the reaction rate for the following:

Cl2(g)+3F2(g)-->2ClF3(g)
Where  :delta:[Cl2]/ :delta:t= -.073

Okay, I solved for both  :delta:[F2]/ :delta:t and  :delta:[ClF3]/ :delta:t (-.22 and .15, respectively), using the rate equation -1/a  :delta:[A]/ :delta:t= -1/b  :delta:/ :delta:t= 1/c  :delta:[C]/ :delta:t....but how do I get the reaction rate from these values? I can't use a rate law since I'm not given the reaction orders or any experimental  data to come up with the reaction orders..

I've been staring at this problem for awhile....maybe I'm overlooking something obvious

Any help would be appreciated.

Thanks,

~CC

[rabolisk]

Did the problem ask you to find the reaction rate? Because what you have is, by definition, the reaction rate. There is nothing more to do.

[calvin coolidge]

The question had three parts: 1) Find  :delta:[F2]/ :delta:t, 2) Find  :delta:[ClF3]/ :delta:t, and 3) find the rate of the reaction.

~CC


 

[rabolisk]

The reaction rate is simply 1/a * d[A]/dt, where a is the coefficient of A, the product, in the balanced chemical reaction. For a reactant, you reverse the sign so that you always get a positive value for reaction rate. So the rate for this problem would be .073.

[calvin coolidge]

That was the correct answer! ...I looked EVERYWHERE in the chapter of my textbook and saw nothing that would have lead me to that answer..

Thanks Rabolisk, you've saved my bacon again!

Enjoy a mole snack...

~CC