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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
Homework Equations
Arrhenius equation:
ln{k2/k1} = Ea/R {(1/T1) - (1/T2)}
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 I am aware that this probably won't even show up, but its driving me crazy that I continually get the wrong answer, and I am off by soooo much.it looks simple, plug in the numbers and out pops an answer but I just can't 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 can't 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 won't fail the exam just because I don't know how to do this question... that's real helpful!)
Thank you,
M