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**1. Homework Statement**

The activation energy for the reaction

N2O(g) --> N2(g) + O(g)

is 250 kJ/mol. If the rate constant is 3.4 s–1 at 1050 K, at what temperature will the rate constant be one thousand times smaller?

The correct answer is : 846 K

**2. Homework Equations**

Arrhenius equation:

ln{k2/k1} = Ea/R {(1/T1) - (1/T2)}

**3. The Attempt at a Solution**

Ok, I can use this equation to find other variables, and I know that I am making some sort of calculator error or something, and I know its probably the stupidest of mistakes. I am trying to study for an exam, and Im aware that this probably wont even show up, but its driving me crazy that I continually get the wrong answer, and Im off by soooo much.it looks simple, plug in the numbers and out pops an answer but I just cant get it.

T1 =1050K

K1 = 3.14/s

Ea = 250KJ

K2 = 3.14E3

I have tried this a number of ways and its only confused me more. Do I change KJ to J? I know Temp. should be in Kelvin, what about R, could I be using the wrong one? I cant look at this question any longer, any help would be much appreciated.

(when I emailed my T.A. he emailed me back to inform me that I wont fail the exam just because I dont know how to do this question.... thats real helpful!)

Thank you,

M

**1. Homework Statement**

**2. Homework Equations**

**3. The Attempt at a Solution**