i'm stumped on how to write this in mathematical form. it says the rate increased by a factor of 2000, I am supposed to determine by what percent the Energy of activation will be reduced. The answer is 25% in the book. I don't know how they get the answer using this formula: k1/k2=Ae^-Ea/RT. A is constant for both reactions. T = 298 K, R = 8.3145
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I am not sure, and someone can come along after I am done and check what I am telling you, but I believe you are missing some information like the temperature change. The question seems to be incomplete.
yeah I'm not sure...an example in the book just equates them, its for a catalyzed reaction by saying k1/k2=(Ae^-Ea/RT)/(Ae^-Ea/Rt)=e^-Ea/RT but I'm not sure about that way.
Is this a multipart problem; i.e., is there another part of the problem in which Ea is calculated? or given? If so, what is the value of Ea in that part of the problem?
no they didn't give anything else
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